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Problems in Physical Chemistry for JEE

Narendra Avasthi

Chapter 5

Chemical Equilibrium - all with Video Answers

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Chapter Questions

01:23

Problem 1

A reversible reaction is one which :
(a) Proceeds in one direction
(b) Proceeds in both directions
(c) Proceeds spontaneously
(d) All the statements are wrong

Ishu Khandelwal
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01:01

Problem 2

The equilibrium constant $K_{c}$ for the reaction
$$
\mathrm{P}_{4}(g) \rightleftharpoons 2 \mathrm{P}_{2}(g)
$$
is $1.4$ at $400^{\circ} \mathrm{C}$. Suppose that 3 moles of $\mathrm{P}_{4}(g)$ and 2 moles of $\mathrm{P}_{2}(g)$ are mixed in 2 litre container at $400^{\circ} \mathrm{C}$. What is the value of reaction quotient $\left(Q_{c}\right)$ ?
(a) $\frac{3}{2}$
(b) $\frac{2}{3}$
(c) 1
(d) None of these

Narayan Hari
Narayan Hari
Numerade Educator
02:09

Problem 3

In a chemical reaction equilibrium is established when :
(a) Opposing reaction ceases
(b) Concentrations of reactants and product are equal
(c) Velocity of opposing reaction is the same as that of forward reaction
(d) Reaction ceases to generate heat

Ishu Khandelwal
Ishu Khandelwal
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05:37

Problem 4

The equilibrium constant for a reaction is $K$, and the reaction quotient is $Q .$ For a particular reaction mixture, the ratio $\frac{K}{Q}$ is $0.33 .$ This means that :
(a) the reaction mixture will equilibrate to form more reactant species
(b) the reaction mixture will equilibrate to form more product species
(c) the equilibrium ratio of reactant to product concentrations will be 3
(d) the equilibrium ratio of reactant to product concentrations will be $0.33$

Shahina -
Shahina -
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05:30

Problem 5

Consider the reaction $2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{SO}_{3}(g)$ for which $K_{\mathrm{c}}=278 \mathrm{M}^{-1} .0 .001 \mathrm{~mole}$ of
each of the reagents $\mathrm{SO}_{2}(g), \mathrm{O}_{2}(g)$ and $\mathrm{SO}_{3}(g)$ are mixed in a $1.0 \mathrm{~L}$ flask. Determine the reaction quotient of the system and the spontaneous direction of the system :
(a) $Q_{c}=1000$, the equilibrium shifts to the right
(b) $Q_{c}=1000 ;$ the equilibrium shifts to the left
(c) $Q_{c}=0.001$; the equilibrium shifts to the left
(d) $Q_{c}=0.001$; the equilibrium shifts to the right

Shahina -
Shahina -
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03:21

Problem 6

In Q. No. 5 , if the mixture of gases was allowed to come to equilibrium. The volume of the reaction vessel was then rapidly increased by a factor of two. As a result of the change the reaction quotient $\left(Q_{c}\right)$ would :
(a) increase because of the pressure decrease
(b) decrease because of the pressure decrease
(c) remain the same because the equilibrium constant is independent of volume
(d) increase because the reaction is endothermic

Shahina -
Shahina -
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01:01

Problem 7

For the reaction $A(g)+3 B(g) \rightleftharpoons 2 C(g)$ at $27^{\circ} \mathrm{C}, 2$ moles of $A, 4$ moles of $B$ and 6 moles of $C$ are present in 2 litre vessel. If $K_{c}$ for the reaction is $1.2$, the reaction will proceed in :
(a) forward direction
(b) backward direction
(c) neither direction
(d) none of these

Narayan Hari
Narayan Hari
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03:38

Problem 8

For a reversible gaseous reaction $\mathrm{N}_{2}+3 \mathrm{H}_{2} \rightleftharpoons 2 \mathrm{NH}_{3}$ at equilibrium, if some moles of $\mathrm{H}_{2}$ are replaced by same number of moles of $\mathrm{T}_{2}$ (T is tritium, isotope of $\mathrm{H}$ and assume isotopes do not have different chemical properties) without affecting other parameters, then :
(a) The sample of ammonia obtained after sometime will be radioactive.
(b) Moles of $\mathrm{N}_{2}$ after the change will be different as compared to moles of $\mathrm{N}_{2}$ present before the change
(c) The value of $K_{p}$ or $K_{c}$ will change
(d) The average molecular mass of new equilibrium will be same as that of old equilibrium

Shahina -
Shahina -
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03:36

Problem 9

For the synthesis of ammonia by the reaction $N_{2}+3 H_{2} \rightleftharpoons 2 N H_{3}$ in the Haber's process, the attainment of equilibrium is correctly predicted by the curve

Shahina -
Shahina -
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02:58

Problem 10

The figure shows the change in concentration of species $A$ and $B$ as a function of time. The equilibrium constant $K_{c}$ for the reaction $A(g) \rightleftharpoons 2 B(g)$ is:
(a) $K_{c}>1$
(b) $K<1$
(c) $K=1$
(d) data insufficient

Shahina -
Shahina -
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03:24

Problem 11

Attainment of the equilibrium $A(g) \rightleftharpoons 2 C(g)+B(g)$ gave the following graph. Find the correct option. (\% dissociation = fraction dissociated $\times 100$ )
(a) At $t=5 \mathrm{sec}$ equilibrium has been reached and $K_{c}=40$ (mol/litre) $^{2}$
(b) At $t=5 \mathrm{sec}$ equilibrium has been reached and $\%$ dissociation of $A$ is $20 \%$
(c) At $t=5$ sec equilibrium has been reached and $\%$ dissociation of $A$ is $30 \%$
(d) None of these

Shahina -
Shahina -
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01:32

Problem 12

Using molar concentrations, what is the unit of $K_{c}$ for the reaction?
$$
\mathrm{CH}_{3} \mathrm{OH}(g) \rightleftharpoons \mathrm{CO}(g)+2 \mathrm{H}_{2}(g)
$$
(a) $M^{-2}$
(b) $M^{2}$
(c) $M^{-1}$
(d) $M$

Ishu Khandelwal
Ishu Khandelwal
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02:13

Problem 13

What is the unit of $K_{p}$ for the reaction?
$$
\mathrm{CS}_{2}(g)+4 \mathrm{H}_{2}(g) \rightleftharpoons \mathrm{CH}_{4}(g)+2 \mathrm{H}_{2} \mathrm{~S}(g)
$$
(a) atm
(b) $\mathrm{atm}^{-2}$
(c) $\mathrm{atm}^{2}$
(d) $\mathrm{atm}^{-1}$

Ishu Khandelwal
Ishu Khandelwal
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01:26

Problem 14

What is the equilibrium expression for the reaction $\mathrm{P}_{4}(s)+5 \mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{P}_{4} \mathrm{O}_{10}(s)$
(a) $K_{c}=\left[\mathrm{O}_{2}\right]^{5}$
(b) $K_{c}=\left[P_{4} \mathrm{O}_{10}\right] \% 5\left[\mathrm{P}_{4}\right]\left[\mathrm{O}_{2}\right]$
(c) $K_{c}=\left[\mathrm{P}_{4} \mathrm{O}_{10}\right] /\left[\mathrm{P}_{4}\right]\left[\mathrm{O}_{2}\right]^{5}$
(d) $K_{c}=1 /\left[\mathrm{O}_{2}\right]^{5}$

Ishu Khandelwal
Ishu Khandelwal
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03:36

Problem 15

At $527^{\circ} \mathrm{C}$, the reaction given below has $K_{c}=4$
$$
\mathrm{NH}_{3}(g) \rightleftharpoons \frac{1}{2} \mathrm{~N}_{2}(g)+\frac{3}{2} \mathrm{H}_{2}(g)
$$
What is the $K_{p}$ for the reaction?
$$
\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \rightleftharpoons 2 \mathrm{NH}_{3}(g)
$$
(a) $16 \times(800 R)^{2}$
(b) $\left(\frac{800 R}{4}\right)^{-2}$
(c) $\left(\frac{1}{4 \times 800 R}\right)^{2}$
(d) None of these

Shahina -
Shahina -
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04:48

Problem 16

The equilibrium constant for the reaction $\mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{NO}(g)$ at temperature $(\mathrm{T})$ is $4 \times 10^{-4} .$ The value of $K_{c}$ for the reaction $\mathrm{NO}(g) \rightleftharpoons \frac{1}{2} \mathrm{~N}_{2}(g)+\frac{1}{2} \mathrm{O}_{2}(g)$ at the same
temperature is :
(a) $4 \times 10^{-4}$
(b) 50
(c) $2.5 \times 10^{2}$
(d) $0.02$

Shahina -
Shahina -
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03:03

Problem 17

The equilibrium constant $K_{c}$ for the following reaction at $842^{\circ} \mathrm{C}$ is $7.90 \times 10^{-3} .$ What is $K_{p}$ at same temperature?
$$
\frac{1}{2} \mathrm{~F}_{2}(g) \rightleftharpoons \mathrm{F}(g)
$$
(a) $8.64 \times 10^{-5}$
(b) $8.26 \times 10^{-4}$
(c) $7.90 \times 10^{-2}$
(d) $7.56 \times 10^{-2}$

Ishu Khandelwal
Ishu Khandelwal
Numerade Educator
03:03

Problem 18

The equilibrium constant $K_{p}$ for the following reaction at $191^{\circ} \mathrm{C}$ is $1.24 .$ What is $K_{c} ?$
$$
\mathrm{B}(s)+\frac{3}{2} \mathrm{~F}_{2}(g) \rightleftharpoons \mathrm{BF}_{3}(g)
$$
(a) $6.7$
(b) $0.61$
(c) $8.30$
(d) $7.6$

Ishu Khandelwal
Ishu Khandelwal
Numerade Educator
01:47

Problem 19

For the equilibrium $\mathrm{SO}_{2} \mathrm{Cl}_{2}(g) \rightleftharpoons \mathrm{SO}_{2}(g)+\mathrm{Cl}_{2}(g)$, what is the temperature at which
$\frac{K_{p}(\mathrm{~atm})}{K_{c}(\mathrm{M})}=3 ?$
(a) $0.027 \mathrm{~K}$
(b) $0.36 \mathrm{~K}$
(c) $36.54 \mathrm{~K}$
(d) $273 \mathrm{~K}$

Ishu Khandelwal
Ishu Khandelwal
Numerade Educator
05:06

Problem 20

For the reversible reaction, $\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \rightleftharpoons 2 \mathrm{NH}_{3}(g)$
at $500^{\circ} \mathrm{C}$, the value of $K_{p}$ is $1.44 \times 10^{-5}$ when partial pressure is measured in atmospheres. The corresponding value of $K_{c}$ with concentration in mole litre $^{-1}$, is:
(a) $1.44 \times 10^{-5} /(0.082 \times 500)^{-2}$
(b) $1.44 \times 10^{-5} /(8.314 \times 773)^{-2}$
(c) $1.44 \times 10^{-5} /(0.082 \times 773)^{2}$
(d) $1.44 \times 10^{-5} /(0.082 \times 773)^{-2}$

Shalini Tyagi
Shalini Tyagi
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02:32

Problem 21

For the reaction $\mathrm{CO}(g)+\mathrm{Cl}_{2}(g) \rightleftharpoons \mathrm{COCl}_{2}(g)$ the value of $\frac{\mathrm{N}_{\mathrm{c}}}{K_{p}}$ is equal to :
(a) $\sqrt{R T}$
(b) $R T$
(c) $\frac{1}{R T}$
(d) $1.0$

Shahina -
Shahina -
Numerade Educator
01:58

Problem 22

The concentration of a pure solid or liquid phase is not included in the expression of equilibrium constant because :
(a) solid and liquid concentrations are independent of their quantities.
(b) solids and liquids react slowly.
(c) solids and liquids at equilibrium do not interact with gaseous phase.
(d) the molecules of solids and liquids cannot migrate to the gaseous phase.

Shahina -
Shahina -
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02:15

Problem 23

A catalyst is a substance which :
(a) increases the equilibrium concentration of the product.
(b) changes the equilibrium constant of the reaction.
(c) shortens the time to reach equilibrium.
(d) supplies energy to the reaction.

Ishu Khandelwal
Ishu Khandelwal
Numerade Educator
02:50

Problem 24

What will be the effect on the equilibrium constant on increasing temperature, if the reaction neither absorbs heat nor releases heat?
(a) Equilibrium constant will remain constant.
(b) Equilibrium constant will decrease.
(c) Equilibrium constant will increase.
(d) Can not be predicted.

Shahina -
Shahina -
Numerade Educator
02:09

Problem 25

The equilibrium constant for the reaction $\mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{NO}(g)$ is $4 \times 10^{-4}$ at $200 \mathrm{~K} .$ In presence of a catalyst, equilibrium is attained ten times faster. Therefore, the equilibrium constant in presence of the catalyst at $200 \mathrm{~K}$ is :
(a) $40 \times 10^{-4}$
(b) $4 \times 10^{-4}$
(c) $4 \times 10^{-3}$
(d) difficult to compute without more data

Shahina -
Shahina -
Numerade Educator
01:45

Problem 26

For the reaction $\mathrm{H}_{2}(g)+\mathrm{I}_{2}(g) \rightleftharpoons 2 \mathrm{HI}(g)$, the equilibrium constant changes with :
(a) total pressure
(b) catalyst
(c) concentration of $\mathrm{H}_{2}$ and $\mathrm{I}_{2}$
(d) temperature

Ishu Khandelwal
Ishu Khandelwal
Numerade Educator
02:27

Problem 27

Consider the reactions $\alpha$
(i) $2 \mathrm{CO}(\mathrm{g})+2 \mathrm{H}_{2} \mathrm{O}(g) \rightleftharpoons 2 \mathrm{CO}_{2}(g)+2 \mathrm{H}_{2}(g)$; Eqm. Constant $=K_{1}$
(ii) $\mathrm{CH}_{4}(g)+\mathrm{H}_{2} \mathrm{O}(g) \rightleftharpoons \mathrm{CO}(g)+3 \mathrm{H}_{2}(g) ;$ Eqm. Constant $=K_{2}$
(iii) $\mathrm{CH}_{4}(g)+2 \mathrm{H}_{2} \mathrm{O}(g) \rightleftharpoons \mathrm{CO}_{2}(g)+4 \mathrm{H}_{2}(g) ;$ Eqm. Constant $=K_{3}$
Which of the following relation is correct?
(a) $K_{3}=\frac{K_{1}}{K_{2}}$
(b) $K_{3}=\frac{K_{1}^{2}}{K_{2}^{2}}$
(c) $K_{3}=K_{1} K_{2}$
(d) $K_{3}=\sqrt{K_{1}} \cdot K_{2}$

Shahina -
Shahina -
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02:32

Problem 28

For the reaction $2 \mathrm{NO}_{2}(g)+\frac{1}{2} \mathrm{O}_{2}(g) \rightleftharpoons \mathrm{N}_{2} \mathrm{O}_{5}(\dot{g})$, if the equilibrium constant is $K_{p}$, then the
equilibrium constant for the reaction $2 \mathrm{~N}_{2} \mathrm{O}_{5}(g) \rightleftharpoons 4 \mathrm{NO}_{2}(g)+\mathrm{O}_{2}(g)$ would be :
(a) $K_{p}^{2}$
(b) $\frac{2}{K_{p}}$
(c) $\frac{1}{K_{p}^{2}}$
(d) $\frac{1}{\sqrt{K_{p}}}$

Shahina -
Shahina -
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01:55

Problem 29

The equilibrium constant $\left(K_{c}\right)$ for the reaction
$$
2 \mathrm{HCl}(g) \rightleftharpoons \mathrm{H}_{2}(g)+\mathrm{Cl}_{2}(g)
$$
is $4 \times 10^{-34}$ at $25^{\circ} \mathrm{C}$. What is the equilibrium constant for the reaction?
$$
\frac{1}{2} \mathrm{H}_{2}(g)+\frac{1}{2} \mathrm{Cl}_{2}(g) \rightleftharpoons \mathrm{HCl}(g)
$$
(a) $2 \times 10^{-17}$
(b) $2.5 \times 10^{33}$
(c) $5 \times 10^{6}$
(d) None of these

Shahina -
Shahina -
Numerade Educator
06:18

Problem 30

At a certain temperature, the following reactions have the equilibrium constants as shown below:
$$
\begin{aligned}
\mathrm{S}(s)+\mathrm{O}_{2}(g) & \rightleftharpoons \mathrm{SO}_{2}(g) ; \quad K_{c}=5 \times 10^{52} \\
2 \mathrm{~S}(s)+3 \mathrm{O}_{2}(g) & \rightleftharpoons 2 \mathrm{SO}_{3}(g) ; K_{c}=10^{29}
\end{aligned}
$$
What is the equilibrium constant $K_{c}$ for the reaction at the same temperature?
$$
2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{SO}_{3}(g)
$$
(a) $2.5 \times 10^{76}$
(b) $4 \times 10^{23}$
(c) $4 \times 10^{-77}$
(d) None of these

Shalini Tyagi
Shalini Tyagi
Numerade Educator
05:47

Problem 31

Consider the following gaseous equilibria given below :
(I) $\mathrm{N}_{2}+3 \mathrm{H}_{2} \rightleftharpoons 2 \mathrm{NH}_{3}$; Eqm. Constant $=K_{1}$
(II) $\mathrm{N}_{2}+\mathrm{O}_{2} \rightleftharpoons 2 \mathrm{NO} ; \quad$ Eqm. Constant $=K_{2}$
(III) $\mathrm{H}_{2}+\frac{1}{2} \mathrm{O}_{2} \rightleftharpoons \mathrm{H}_{2} \mathrm{O} ;$ Eqm. Constant $=K_{3}$
The equilibrium constant for the reaction, $2 \mathrm{NH}_{3}+\frac{5}{2} \mathrm{O}_{2} \rightleftharpoons 2 \mathrm{NO}+3 \mathrm{H}_{2} \mathrm{O}$ in terms of $K_{1}, K_{2}$
and $K_{3}$ will be :
$\begin{array}{llll}\text { (a) } K_{1} K_{2} K_{3} & \text { (b) } \frac{K_{1} K_{2}}{K_{3}} & \text { (c) } \frac{K_{1} K_{3}^{2}}{K_{2}} & \text { (d) } \frac{K_{2} K_{3}^{3}}{K_{1}}\end{array}$

Shalini Tyagi
Shalini Tyagi
Numerade Educator
03:54

Problem 32

In the reaction $X(g)+Y(g) \rightleftharpoons 2 Z(g), 2$ mole of $X, 1$ mole of $Y$ and 1 mole of $Z$ are placed in a 10 litre vessel and allowed to reach equilibrium. If final concentration of $Z$ is $0.2 M$, then. $K_{c}$ for the given reaction is :
(a) $1.60$
(b) $\frac{80}{3}$
(c) $\frac{16}{3}$
(d) None of these

Shalini Tyagi
Shalini Tyagi
Numerade Educator
02:22

Problem 33

An equilibrium mixture of the reaction $2 \mathrm{H}_{2} \mathrm{~S}(g) \rightleftharpoons 2 \mathrm{H}_{2}(g)+\mathrm{S}_{2}(g)$ had $0.5$ mole $\mathrm{H}_{2} \mathrm{~S}, 0.10$
mole $\mathrm{H}_{2}$ and $0.4$ mole $\mathrm{S}_{2}$ in one litre vessel. The value of equilibrium constant $(\mathrm{K})$ in $\mathrm{mol}$ litre $^{-1}$ is :
(a) $0.004$
(b) $0.008$
(c) $0.016$
(d) $0.160$

Shalini Tyagi
Shalini Tyagi
Numerade Educator
02:48

Problem 34

Given $\left[\mathrm{CS}_{2}\right]=0.120 \mathrm{M},\left[\mathrm{H}_{2}\right]=0.10,\left[\mathrm{H}_{2} \mathrm{~S}\right]=0.20$ and $\left[\mathrm{CH}_{4}\right]=8.40 \times 10^{-5} M$ for the
following reaction at $900^{\circ} \mathrm{C}$, at eq. Calculate the equilibrium constant $\left(K_{c}\right)$.
$$
\mathrm{CS}_{2}(g)+4 \mathrm{H}_{2}(g) \rightleftharpoons \mathrm{CH}_{4}(g)+2 \mathrm{H}_{2} \mathrm{~S}(g)
$$
(a) $0.0120$
(b) $0.0980$
(c) $0.280$
(d) $0.120$

Shalini Tyagi
Shalini Tyagi
Numerade Educator
03:24

Problem 35

The equilibrium constant for the following reaction is $10.5$ at $500 \mathrm{~K}$. A system at equilibrium has $[\mathrm{CO}]=0.250 \mathrm{M}$ and $\left[\mathrm{H}_{2}\right]=0.120 \mathrm{M}$. What is the $\left[\mathrm{CH}_{3} \mathrm{OH}\right]$ ?
$$
\mathrm{CO}(g)+2 \mathrm{H}_{2}(g) \rightleftharpoons \mathrm{CH}_{3} \mathrm{OH}(g)
$$
(a) $0.0378$
(b) $0.0435$
(c) $0.546$
(d) $0.0499$

Shalini Tyagi
Shalini Tyagi
Numerade Educator
01:01

Problem 36

When sulphur (in the form of $S_{8}$ ) is heated at temperature $T$, at equilibrium, the pressure of $S_{8}$ falls by $30 \%$ from $1.0 \mathrm{~atm}$, because $\mathrm{S}_{8}(g)$ is partially converted into $\mathrm{S}_{2}(g)$. Find the value of $K_{p}$ for this reaction.
(a) $2.96$
(b) $6.14$
(c) $204.8$
(d) None of these

Narayan Hari
Narayan Hari
Numerade Educator
08:04

Problem 37

$9.2$ grams of $\mathrm{N}_{2} \mathrm{O}_{4}(g)$ is taken in a closed one litre vessel and heated till the following equilibrium is reached $\mathrm{N}_{2} \mathrm{O}_{4}(g) \rightleftharpoons 2 \mathrm{NO}_{2}(g)$
At equilibrium, $50 \% \mathrm{~N}_{2} \mathrm{O}_{4}(g)$ is dissociated. What is the equilibrium constant (in mol litre $^{-1}$ ) (molecular weight of $\mathrm{N}_{2} \mathrm{O}_{4}=92$ )
(a) $0.1$
(b) $0.4$
(c) $0.2$
(d) 2

Shalini Tyagi
Shalini Tyagi
Numerade Educator
05:26

Problem 38

Two moles of $\mathrm{NH}_{3}$ when put into a previously evacuated vessel (one litre), partially dissociated into $\mathrm{N}_{2}$ and $\mathrm{H}_{2}$. If at equilibrium one mole of $\mathrm{NH}_{3}$ is present, the equilibrium constant is :
(a) $3 / 4 \mathrm{~mol}^{2}$ litre $^{-2}$
(b) $27 / 64 \mathrm{~mol}^{2}$ litre $^{-2}$
(c) $27 / 32 \mathrm{~mol}^{2}$ litre $^{-2}$
(d) $27 / 16 \mathrm{~mol}^{2}$ litre $^{-2}$

Shalini Tyagi
Shalini Tyagi
Numerade Educator
01:03

Problem 39

In the presence of excess of anhydrous $\mathrm{SrCl}_{2}$, the amount of water taken up is governed by $K_{p}=10^{12} \mathrm{~atm}^{-4}$ for the following reaction at $273 \mathrm{~K}$
$$
\mathrm{SrCl}_{2} \cdot 2 \mathrm{H}_{2} \mathrm{O}(s)+4 \mathrm{H}_{2} \mathrm{O}(g) \rightleftharpoons \mathrm{SrCl}_{2} \cdot 6 \mathrm{H}_{2} \mathrm{O}(s)
$$
What is equilibrium vapour pressure (in torr) of water in a closed vessel that contains $\mathrm{SrCl}_{2} \cdot 2 \mathrm{H}_{2} \mathrm{O}(s) ?$
(a) $0.001$ torr
(b) $10^{3}$ torr
(c) $0.76$ torr
(d) $1.31$ torr

Narayan Hari
Narayan Hari
Numerade Educator
01:01

Problem 40

$\mathrm{CuSO}_{4} \cdot 5 \mathrm{H}_{2} \mathrm{O}(s) \rightleftharpoons \mathrm{CuSO}_{4} \cdot 3 \mathrm{H}_{2} \mathrm{O}(s)+2 \mathrm{H}_{2} \mathrm{O}(g) ; K_{p}=4 \times 10^{-4} \mathrm{~atm}^{2}$. If the vapour pressure
of water is 38 torr then percentage of relative humidity is : (Assume all data at constant temperature)
(a) 4
(b) 10
(c) 40
(d) None of these

Narayan Hari
Narayan Hari
Numerade Educator
05:27

Problem 41

$\mathrm{NH}_{4} \mathrm{HS}(s) \rightleftharpoons \mathrm{NH}_{3}(g)+\mathrm{H}_{2} \mathrm{~S}(g)$
The equilibrium pressure at $25^{\circ} \mathrm{C}$ is $0.660 \mathrm{~atm}$. What is $K_{p}$ for the reaction?
(a) $0.109$
(b) $0.218$
(c) $1.89$
(d) $2.18$

Shalini Tyagi
Shalini Tyagi
Numerade Educator
01:01

Problem 42

For the reaction $2 A(g) \rightleftharpoons B(g)+3 C(g)$, at a given temperature, $K_{c}=16 .$ What must be the volume of the flask, if a mixture of 2 mole each of $A, B$ and $C$ exist in equilibrium?
(a) $\frac{1}{4}$
(b) $\frac{1}{2}$
(c) 1
(d) None of these

Narayan Hari
Narayan Hari
Numerade Educator
03:13

Problem 43

One mole of pure ethyl alcohol was treated with one mole of pure acetic acid at $25^{\circ} \mathrm{C}$. One-third of the acid changes into ester at equilibrium. The equilibrium constant for the reaction will be :
(a) $\frac{1}{4}$
(b) 2
(c) 3
(d) 4

Shalini Tyagi
Shalini Tyagi
Numerade Educator
09:32

Problem 44

$\mathrm{I}_{2}(a q)+\mathrm{I}^{-}(a q) \rightleftharpoons \mathrm{I}_{3}^{-}(a q) .$ We started with 1 mole of $\mathrm{I}_{2}$ and $0.5$ mole of $\mathrm{I}^{-}$ in one litre flask. After equilibrium is reached, excess of $\mathrm{AgNO}_{3}$ gave $0.25$ mole of yellow precipitate. Equilibrium constant is :
(a) $1.33$
(b) $2.66$
(c) $2.0$
(d) $3.0$

Shalini Tyagi
Shalini Tyagi
Numerade Educator
01:01

Problem 45

At $87^{\circ} \mathrm{C}$, the following equilibrium is established.
$$
\mathrm{H}_{2}(g)+\mathrm{S}(s) \rightleftharpoons \mathrm{H}_{2} \mathrm{~S}(g) ; K_{c}=0.08
$$
If $0.3$ mole hydrogen and 2 mole sulphur are heated to $87^{\circ} \mathrm{C}$ in a $2 \mathrm{~L}$ vessel, what will be the concentration of $\mathrm{H}_{2} \mathrm{~S}$ at equilibrium?
(a) $0.011 \mathrm{M}$
(b) $0.022 \mathrm{M}$
(c) $0.044 \mathrm{M}$
(d) $0.08 \mathrm{M}$

Narayan Hari
Narayan Hari
Numerade Educator
05:00

Problem 46

In the equilibrium $2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{SO}_{3}(g)$, the partial pressure of $\mathrm{SO}_{2}, \mathrm{O}_{2}$ and $\mathrm{SO}_{3}$
are $0.662,0.10$ and $0.331$ atm respectively. What should be the partial pressure of oxygen so that the equilibrium concentrations of $\mathrm{SO}_{2}$ and $\mathrm{SO}_{3}$ are equal?
(a) $0.4 \mathrm{~atm}$
(b) $1.0 \mathrm{~atm}$
(c) $0.8$ atm
(d) $0.25$ atm

Shalini Tyagi
Shalini Tyagi
Numerade Educator
01:01

Problem 47

When heated, ammonium carbamate decomposes as follows:
$\because$
$$
\mathrm{NH}_{4} \mathrm{COONH}_{2}(s) \rightleftharpoons 2 \mathrm{NH}_{3}(g)+\mathrm{CO}_{2}(g)
$$
At a certain temperature, the equilibrium pressure of the system is $0.318$ atm. $K_{p}$ for the reaction is :
(a) $0.128$
(b) $0.426$
(c) $4.76 \times 10^{-3}$
(d) None of these

Narayan Hari
Narayan Hari
Numerade Educator
07:10

Problem 48

In a system $A(s) \rightleftharpoons 2 B(g)+3 C(g)$, if the concentration of $C$ at equilibrium is increased by a factor of 2 , it will cause the equilibrium concentration of $B$ to change to :
(a) two times the original value
(b) one half of its original value
(c) $2 \sqrt{2}$ times to the original value
(d) $\frac{1}{2 \sqrt{2}}$ times the original value

Shalini Tyagi
Shalini Tyagi
Numerade Educator
04:50

Problem 49

$A+B \rightleftharpoons C+D$. If finally the concentration of $A$ and $B$ are both equal but at equilibrium concentration of $D$ will be twice of that of $A$ then what will be the equilibrium constant of reaction ?
(a) $\frac{4}{0}$
(b) $\frac{9}{4}$
(c) $\frac{1}{9}$
(d) 4

Shalini Tyagi
Shalini Tyagi
Numerade Educator
06:12

Problem 50

The equilibrium constant $K_{c}$ for the reaction $\mathrm{SO}_{2}(g)+\mathrm{NO}_{2}(g) \rightleftharpoons \mathrm{SO}_{3}(g)+\mathrm{NO}(g)$ is $16 .$ If 1 mole of each of all the four gases is taken in $1 \mathrm{dm}^{3}$ vessel, the equilibrium concentration of NO would be :
(a) $0.4 \mathrm{M}$
(b) $0.6 \mathrm{M}$
(c) $1.4 \mathrm{M}$
(d) $1.6 \mathrm{M}$

Shalini Tyagi
Shalini Tyagi
Numerade Educator
01:33

Problem 51

On increasing the temperature, the rate of a reaction :
(a) always increases
(b) always decreases
(c) first increases and then decreases
(d) may increase or decrease depending upon the nature of the reaction

Shahina -
Shahina -
Numerade Educator
01:39

Problem 52

A catalyst increases the rate of a reaction by:
(a) increasing the activation energy of the reaction
(b) increasing the value of rate constants $\left(k_{f}\right.$ and $k_{b}$ )
(c) increasing the enthalpy change of the reaction
(d) decreasing the enthalpy change of the reaction

Shahina -
Shahina -
Numerade Educator
01:17

Problem 53

At a certain temperature, only $50 \% \mathrm{HI}$ is dissociated at equilibrium in the following reaction:
$$
2 \mathrm{HI}(g) \rightleftharpoons \mathrm{H}_{2}(g)+\mathrm{I}_{2}(g)
$$
The equilibrium constant for this reaction is :
(a) $0.25$
(b) $1.0$
(c) $3.0$
(d) $0.5$

Shahina -
Shahina -
Numerade Educator
01:54

Problem 54

The equilibrium constant $K_{p}$ for the reaction
$$
\mathrm{H}_{2}(g)+\mathrm{CO}_{2}(g) \rightleftharpoons \mathrm{H}_{2} \mathrm{O}(g)+\mathrm{CO}(g)
$$
$4.0$ at $1660^{\circ} \mathrm{C}$. Initially $0.80$ mole $\mathrm{H}_{2}$ and $0.80$ mole $\mathrm{CO}_{2}$ are injected into a $5.0$ litre flask. What is the equilibrium concentration of $\mathrm{CO}_{2}(g) ?$
(a) $0.533 \mathrm{M}$
(b) $0.0534 \mathrm{M}$
(c) $0.535 \mathrm{M}$
(d) None of these

Narayan Hari
Narayan Hari
Numerade Educator
01:05

Problem 55

At $273 \mathrm{~K}$ and 1 atm, 10 litre of $\mathrm{N}_{2} \mathrm{O}_{4}$ decomposes to $\mathrm{NO}_{2}$ according to equation
$$
\mathrm{N}_{2} \mathrm{O}_{4}(g) \rightleftharpoons 2 \mathrm{NO}_{2}(g)
$$
What is degree of dissociation $(\alpha)$ when the original volume is $25 \%$ less than that of existing volume?
(a) $0.25$
(b) $0.33$
(c) $0.66$
(d) $0.5$

Narayan Hari
Narayan Hari
Numerade Educator
01:02

Problem 56

The equilibrium constant for the reaction $\mathrm{CO}(g)+\mathrm{H}_{2} \mathrm{O}(g) \rightleftharpoons \mathrm{CO}_{2}(g)+\mathrm{H}_{2}(g)$ is $5 .$ How
many moles of $\mathrm{CO}_{2}$ must be added to 1 litre container already containing 3 moles each of $\mathrm{CO}$ and $\mathrm{H}_{2} \mathrm{O}$ to make $2 \mathrm{M}$ equilibrium concentration of $\mathrm{CO}$ ?
(a) 15
(b) 19
(c) 5
(d) 20

Narayan Hari
Narayan Hari
Numerade Educator
04:25

Problem 57

A nitrogen-hydrogen mixture initially in the molar ratio of $1: 3$ reached equilibrium to form ammonia when $25 \%$ of the $\mathrm{N}_{2}$ and $\mathrm{H}_{2}$ had reacted. If the total pressure of the system was 21 atm, the partial pressure of ammonia at the equilibrium was:
(a) $4.5$ atm
(b) $3.0 \mathrm{~atm}$
(c) $2.0 \mathrm{~atm}$
(d) $1.5 \mathrm{~atm}$

Shahina -
Shahina -
Numerade Educator
05:37

Problem 58

Ammonia under a pressure of $15 \mathrm{~atm}$ at $27^{\circ} \mathrm{C}$ is heated to $347^{\circ} \mathrm{C}$ in a closed vessel in the presence of a catalyst. Under the conditions, $\mathrm{NH}_{3}$ is partially decomposed according to the equation, $2 \mathrm{NH}_{3} \rightleftharpoons \mathrm{N}_{2}+3 \mathrm{H}_{2}$ the vessel is such that the volume remains effectively constant where as pressure increases to $50 \mathrm{~atm} .$ Calculate the percentage of $\mathrm{NH}_{3}$ actually decomposed :
(a) $65 \%$
(b) $61.3 \%$
(c) $62.5 \%$
(d) $64 \%$

Shahina -
Shahina -
Numerade Educator
01:40

Problem 59

$0.1$ mole of $\mathrm{N}_{2} \mathrm{O}_{4}(g)$ was sealed in a tube under one atmospheric conditions at $25^{\circ} \mathrm{C} .$ Calculate the number of moles of $\mathrm{NO}_{2}(g)$ present, if the equilibrium $\mathrm{N}_{2} \mathrm{O}_{4}(g) \rightleftharpoons 2 \mathrm{NO}_{2}(g)$ $\left(K_{p}=0.14\right)$ is reached after some time :
(a) $1.8 \times 10^{2}$
(b) $2.8 \times 10^{2}$
(c) $0.034$
(d) $28 \times 10^{-2}$

Shahina -
Shahina -
Numerade Educator
02:29

Problem 60

5 moles of $\mathrm{SO}_{2}$ and 5 moles of $\mathrm{O}_{2}$ are allowed to react. At equilibrium, it was found that $60 \%$ of $\mathrm{SO}_{2}$ is used up. If the pressure of the equilibrium mixture is one atmosphere, the partial pressure of $\mathrm{O}_{2}$ is:
(a) $0.52 \mathrm{~atm}$
(b) $0.21 \mathrm{~atm}$
(c) $0.41 \mathrm{~atm}$
(d) $0.82$ atm

Shahina -
Shahina -
Numerade Educator
03:04

Problem 61

$\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \rightleftharpoons 2 \mathrm{NH}_{3}(g)$
For the reaction initially the mole ratio was $1: 3$ of $\mathrm{N}_{2}: \mathrm{H}_{2} .$ At equilibrium $50 \%$ of each has reacted. If the equilibrium pressure is $p$, the partial pressure of $\mathrm{NH}_{3}$ at equilibrium is :
(a) $\frac{P}{3}$
(b) $\frac{P}{4}$
(c) $\frac{P}{6}$
(d) $\frac{P}{8}$
$\therefore$

Shahina -
Shahina -
Numerade Educator
04:10

Problem 62

$2.0$ mole of $\mathrm{PCl}_{5}$ were introduced in a vessel of $5.0 \mathrm{~L}$ capacity of a particular temperature. At equilibrium, $\mathrm{PCl}_{5}$ was found to be $35 \%$ dissociated into $\mathrm{PCl}_{3}$ and $\mathrm{Cl}_{2}$. The value of $K_{c}$ for the reaction
$$
\mathrm{PCl}_{3}(g)+\mathrm{Cl}_{2}(g) \rightleftharpoons \mathrm{PCl}_{5}(g)
$$
(a) $1.89$
(b) $0.377$
(c) $1.33$
(d) $13.3$

Shahina -
Shahina -
Numerade Educator
04:33

Problem 63

At certain temperature compound $A B_{2}(g)$ dissociates according to the reaction
$$
2 A B_{2}(g) \rightleftharpoons 2 A B(g)+B_{2}(g)
$$
With degree of dissociation $\alpha$, which is small compared with unity. The expression of $K_{p}$, in terms of $\alpha$ and initial pressure $P$ is :
(a) $P \frac{\alpha^{3}}{2}$
(b) $\frac{P \alpha^{2}}{3}$
(c) $P \frac{\alpha^{3}}{3}$
(d) $\frac{P \alpha^{2}}{2}$

Shalini Tyagi
Shalini Tyagi
Numerade Educator
04:27

Problem 64

For the reaction $\mathrm{H}_{2}(g)+\mathrm{CO}_{2}(g) \rightleftharpoons \mathrm{CO}(g)+\mathrm{H}_{2} \mathrm{O}(g)$. If the initial concentration of $\left[\mathrm{H}_{2}\right]=\left[\mathrm{CO}_{2}\right]$ and $x$
moles/litre of hydrogen is consumed at equilibrium, the correct expression of $K_{p}$ is :
(a) $\frac{x^{2}}{(1-x)^{2}}$
(b) $\frac{(1+x)^{2}}{(1-x)^{2}}$
(c) $\frac{x^{2}}{(2+x)^{2}}$
(d) $\frac{x^{2}}{1-x^{2}}$

Shalini Tyagi
Shalini Tyagi
Numerade Educator
02:42

Problem 65

If $D_{T}$ and $D_{O}$ are the theoretical and observed vapour densities at a definite temperature and $\alpha$ be the degree of dissociation of a substance. Then, $\alpha$ in the terms of $D_{O}, D_{T}$ and $n$ (number of moles of products formed from 1 mole reactant) is calculated by the formula :
(a) $\alpha=\frac{D_{O}-D_{T}}{(1-n) D_{T}}$
(b) $\alpha=\frac{D_{T}-D_{O}}{(n-1) D_{T}}$
(c) $\alpha=\frac{D_{T}-D_{O}}{(n-1) D_{O}}$
(d) $\alpha=\frac{D-D_{T}}{(n-1) D_{T}}$

Rajesh Singh
Rajesh Singh
Numerade Educator
01:01

Problem 66

For the dissociation of $\mathrm{PCl}_{5}$ into $\mathrm{PCl}_{5}$ and $\mathrm{Cl}_{2}$ in gaseous phase reaction, if $d$ is the observed vapour density and $D$ the theoretical vapour density with ' $\alpha$ ' as degree of dissociation. Variation of $D / d$ with ' $\alpha$ ' is given by which graph?

Narayan Hari
Narayan Hari
Numerade Educator
01:01

Problem 67

At $27^{\circ} \mathrm{C}$ and 1 atm pressure, $\mathrm{N}_{2} \mathrm{O}_{4}$ is $20 \%$ dissociation into $\mathrm{NO}_{2} .$ What is the density of equilibrium mixture of $\mathrm{N}_{2} \mathrm{O}_{4}$ and $\mathrm{NO}_{2}$ at $27^{\circ} \mathrm{C}$ and $1 \mathrm{~atm}$ ?
(a) $3.11 \mathrm{~g} /$ litre
(b) $2.11 \mathrm{~g} /$ litre
(c) $4.5 \mathrm{~g} /$ litre
(d) None of these

Narayan Hari
Narayan Hari
Numerade Educator
01:01

Problem 68

$\mathrm{COCl}_{2}$ gas dissociates according to the equation, $\mathrm{COCl}_{2}(g) \rightleftharpoons \mathrm{CO}(g)+\mathrm{Cl}_{2}(g)$. When
heated to $700 \mathrm{~K}$ the density of the gas mixture at $1.16 \mathrm{~atm}$ and at equilibrium is $1.16 \mathrm{~g} /$ litre. The degree of dissociation of $\mathrm{CO}_{2}$ at $700 \mathrm{~K}$ is :
(a) $0.28$
(b) $0.50$
(c) $0.72$
(d) $0.42$

Narayan Hari
Narayan Hari
Numerade Educator
07:46

Problem 69

The degree of dissociation of $\mathrm{I}_{2}$ molecule of $1000^{\circ} \mathrm{C}$ and under atmospheric pressure is $40 \%$ by volume. If the dissociation is reduced to $20 \%$ at the same temp. total equilibrium pressure on the gas is :
(a) $1.57 \mathrm{~atm}$
(b) $2.57$ atm
(c) $3.57$ atm
(d) $4.57 \mathrm{~atm}$

Shalini Tyagi
Shalini Tyagi
Numerade Educator
01:05

Problem 70

Determine the value of equilibrium constant $\left(K_{c}\right)$ for the reaction
$$
A_{2}(g)+B_{2}(g) \rightleftharpoons 2 A B(g)
$$
If 10 moles of $A_{2} ; 15$ moles of $B_{2}$ and 5 moles of $A B$ are placed in a 2 litre vessel and allowed to come to equilibrium. The final concentration of $A B$ is $7.5 M$ :
(a) $4.5$
(b) $1.5$
(c) $0.6$
(d) None of these

Narayan Hari
Narayan Hari
Numerade Educator
01:19

Problem 71

At $87^{\circ} \mathrm{C}$, the following equilibrium is established
$$
\mathrm{H}_{2}(g)+\mathrm{S}(s) \rightleftharpoons \mathrm{H}_{2} \mathrm{~S}(g) ; \quad K_{p}=7 \times 10^{-2}
$$
If $0.50$ mole of hydrogen and $1.0$ mole of sulphur are heated to $87^{\circ} \mathrm{C}$ in $1.0 \mathrm{~L}$ vessel, what will be the partial pressure of $\mathrm{H}_{2} \mathrm{~S}$ at equilibrium?
(a) $0.966 \mathrm{~atm}$
(b) $1.38 \mathrm{~atm}$
(c) $0.0327$ atm
(d) 1 atm

Narayan Hari
Narayan Hari
Numerade Educator
01:03

Problem 72

Pure $\mathrm{PCl}_{5}$ is introduced into an evacuated chamber and comes to equilibrium at $247^{\circ} \mathrm{C}$ and $2.0$ atm. The equilibrium gaseous mixture contains $40 \%$ chlorine by volume. Calculate $K_{p}$ at $247^{\circ} \mathrm{C}$ for the reaction
$$
\mathrm{PCl}_{5}(g) \rightleftharpoons \mathrm{PCl}_{3}(\dot{g})+\mathrm{Cl}_{2}(g)
$$
(a) $0.625$ atm
(b) 4 atm
(c) $1.6$ atm
(d) None of these

Narayan Hari
Narayan Hari
Numerade Educator
01:01

Problem 73

For the reaction
$$
\mathrm{SnO}_{2}(s)+2 \mathrm{H}_{2}(g) \rightleftharpoons 2 \mathrm{H}_{2} \mathrm{O}(g)+\operatorname{Sn}(l)
$$
calculate $K_{p}$ at $900 \mathrm{~K}$, where the equilibrium steam-hydrogen mixture was $45 \% \mathrm{H}_{2}$ by volume :
(a) $1.49$
(b). $1.22$
(c) $0.67$
(d) None of these

Narayan Hari
Narayan Hari
Numerade Educator
01:06

Problem 74

For the reaction $\mathrm{XCO}_{3}(s) \rightleftharpoons \mathrm{XO}(s)+\mathrm{CO}_{2}(g), K_{p}=1.642 \mathrm{~atm}$ at $727^{\circ} \mathrm{C}$. If 4 moles of
$\mathrm{XCO}_{3}(s)$ was put into a 50 litre container and heated to $727^{\circ} \mathrm{C} .$ What mole percent of the $X \mathrm{CO}_{3}$ remains unreacted at equilibrium?
(a) 20
(b) 25
(c) 50
(d) None of these

Narayan Hari
Narayan Hari
Numerade Educator
01:21

Problem 75

$\mathrm{Fe}_{2} \mathrm{O}_{3}(s)$ may be converted to $\mathrm{Fe}$ by the reaction
$$
\mathrm{Fe}_{2} \mathrm{O}_{3}(s)+3 \mathrm{H}_{2}(g) \rightleftharpoons 2 \mathrm{Fe}(s)+3 \mathrm{H}_{2} \mathrm{O}(g)
$$
for which $K_{c}=8$ at temp. $720^{\circ} \mathrm{C}$. What percentage of the $\mathrm{H}_{2}$ remains unreacted after the reaction has come to equilibrium?
(a) $=22 \%$
(b) $=34 \%$
$(\mathrm{c})=66 \%$
$(\mathrm{d})=78 \%$

Narayan Hari
Narayan Hari
Numerade Educator
01:03

Problem 76

$A B_{3}(g)$ is dissociates as $A B_{3}(g) \rightleftharpoons A B_{2}(g)+\frac{1}{2} B_{2}(g)$
When the initial pressure of $A B_{2}$ is 800 torr and the total pressure developed at equilibrium is 900 torr. What fraction of $A B_{3}(g)$ is dissociated?
(a) $10 \%$
(b) $20 \%$
(c) $25 \%$
(d) $30 \%$

Narayan Hari
Narayan Hari
Numerade Educator
01:05

Problem 77

At $1000 \mathrm{~K}$, a sample of pure $\mathrm{NO}_{2}$ gas decomposes as:
$$
2 \mathrm{NO}_{2}(g) \rightleftharpoons 2 \mathrm{NO}(g)+\mathrm{O}_{2}(g)
$$
The equilibrium constant $K_{p}$ is $156.25$ atm. Analysis shows that the partial pressure of $\mathrm{O}_{2}$ is $0.25$ atm at equilibrium. The partial pressure of $\mathrm{NO}_{2}$ at equilibrium is :
(a) $0.01$
(b) $0.02$
(c) $0.04$
(d) None of these

Narayan Hari
Narayan Hari
Numerade Educator
01:06

Problem 78

Pure nitrosyl chloride (NOCl) gas was heated to $240^{\circ} \mathrm{C}$ in a $1.0 \mathrm{~L}$ container. At equilibrium the total pressure was $1.0 \mathrm{~atm}$ and the NOCl pressure was $0.64 \mathrm{~atm}$. What would be the value of $K_{p}$ ?
(a) $1.02 \mathrm{~atm}$
(b) $16.875 \times 10^{-3}$ atm
(c) $16 \times 10^{-2}$ atm
(d) None of these

Narayan Hari
Narayan Hari
Numerade Educator
01:30

Problem 79

At a certain temperature the equilibrium constant $K_{c}$ is $0.25$ for the reaction
$$
A_{2}(g)+B_{2}(g) \rightleftharpoons C_{2}(g)+D_{2}(g)
$$
If we take 1 mole of each of the four gases in a 10 litre container, what would be equilibrium concentration of $A_{2}(g) ?$
(a) $0.331 \mathrm{M}$
(b) $0.033 M$
(c) $0.133 \mathrm{M}$
(d) $1.33 \mathrm{M}$

Narayan Hari
Narayan Hari
Numerade Educator
02:17

Problem 80

At $200^{\circ} \mathrm{C} \mathrm{PCl}_{5}$ dissociates as follows :
$$
\mathrm{PCl}_{5}(g) \rightleftharpoons \mathrm{PCl}_{3}(g)+\mathrm{Cl}_{2}(g)
$$
It was found that the equilibrium vapours are 62 times as heavy as hydrogen. The degree of dissociation of $\mathrm{PCl}_{5}$ at $200^{\circ} \mathrm{C}$ is nearly :
(a) $10 \%$
(b) $42 \%$
(c) $50 \%$
(d) $68 \%$

Shalini Tyagi
Shalini Tyagi
Numerade Educator
06:27

Problem 81

For the dissociation reaction $\mathrm{N}_{2} \mathrm{O}_{4}(g) \rightleftharpoons 2 \mathrm{NO}_{2}(g)$, the degree of dissociation $(\alpha)$ in terms of $K_{p}$ and total equilibrium pressure $P$ is :
(a) $\alpha=\sqrt{\frac{4 P+K_{P}}{K_{P}}}$
(b) $\alpha=\sqrt{\frac{K_{p}}{4 P+K_{p}}}$
(c) $\alpha=\sqrt{\frac{K_{P}}{4 P}}$
(d) None of these

Shalini Tyagi
Shalini Tyagi
Numerade Educator
01:16

Problem 82

The graph which represents all the equilibrium concentrations for the reaction
$$
\mathrm{N}_{2} \mathrm{O}_{4}(g) \rightleftharpoons 2 \mathrm{NO}_{2}(g)
$$
Then the select the correct graph for concentrations of $\mathrm{NO}_{2}$ against concentrations of $\mathrm{NO}_{4}$ :

Deepanshu Kumar
Deepanshu Kumar
Numerade Educator
01:01

Problem 83

The vapour pressure of mercury is $0.002 \mathrm{~mm} \mathrm{Hg}$ at $27^{\circ} \mathrm{C} . K_{c}$ for the process $\mathrm{Hg}(l) \rightleftharpoons \mathrm{Hg}(g)$
is :
(a) $0.002$
(b) $8.12 \times 10^{-5}$
(c) $6.48 \times 10^{-5}$
(d) $1.068 \times 10^{-7}$

Narayan Hari
Narayan Hari
Numerade Educator
01:01

Problem 84

Calculate the equilibrium constant $\left(K_{c}\right)$ for the reaction below if they are present at equilibrium $5.0$ mole of $A_{2}, 3$ mole of $B_{2}$ and 2 mole of $A B_{2}$ at $8.21$ atm and $300 \mathrm{~K}$
$$
A_{2}(g)+2 B_{2}(g) \rightleftharpoons 2 A B_{2}(g)+\text { Heat }
$$
(a) $1.333$
(b) $2.66$
(c) 20
(d) None of these

Narayan Hari
Narayan Hari
Numerade Educator
05:48

Problem 85

For the reaction (1) and (2)
$$
\begin{aligned}
&A(g) \rightleftharpoons B(g)+C(g) \\
&X(g) \rightleftharpoons 2 Y(g)
\end{aligned}
$$
Given, $K_{R_{1}}: K_{P_{2}}=9: 1$
If the degree of dissociation of $A(g)$ and $X(g)$ be same then the total pressure at equilibrium
(1) and (2) are in the ratio :
(a) $3: 1$
(b) $36: 1$
(c) $1: 1$
(d) $0.5: 1$

Shalini Tyagi
Shalini Tyagi
Numerade Educator
06:49

Problem 86

Given the following reaction at equilibrium, $\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \rightleftharpoons 2 \mathrm{NH}_{3}(g) .$ Some inert gas at constant pressure is added to the system. Predict which of the following facts will be affected?
(a) More $\mathrm{NH}_{3}(g)$ is produced
(b) Less $\mathrm{NH}_{3}(g)$ is produced
(c) No affect on the equilibrium
(d) $K_{p}$ of the reaction is decreased

Shalini Tyagi
Shalini Tyagi
Numerade Educator
02:48

Problem 87

Change in volume of the system does not alter the number of moles in which of the following equilibrium :
(a) $\mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{NO}(g)$
(b) $\mathrm{PCl}_{5}(g) \rightleftharpoons \mathrm{PCl}_{3}(g)+\mathrm{Cl}_{2}(g)$
(c) $\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \rightleftharpoons 2 \mathrm{NH}_{3}(g)$
(d) $\mathrm{SO}_{2} \mathrm{Cl}_{2}(g) \rightleftharpoons \mathrm{SO}_{2}(g)+\mathrm{Cl}_{2}(g)$

Shalini Tyagi
Shalini Tyagi
Numerade Educator
05:08

Problem 88

For the reaction
$$
\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \rightleftharpoons 2 \mathrm{NH}_{3}(g) ; \quad \Delta H=-93.6 \mathrm{~kJ} \mathrm{~mol}^{-1}
$$
the number of moles of $\mathrm{H}_{2}$ at equilibrium will increase if :
(a) volume is increased
(b) volume is decreased
(c) argon gas is added at constant volume
(d) $\mathrm{NH}_{3}$ is removed

Aswathy M
Aswathy M
Numerade Educator
01:32

Problem 89

The volume of the reaction vessel containing an equilibrium mixture is increased in the following reaction
$$
\mathrm{SO}_{2} \mathrm{Cl}_{2}(g) \rightleftharpoons \mathrm{SO}_{2}(g)+\mathrm{Cl}_{2}(g)
$$
When equilibrium is re-established :
(a) the amount of $\mathrm{Cl}_{2}(g)$ remains unchanged
(b) the amount of $\mathrm{Cl}_{2}(g)$ increases
(c) the amount of $\mathrm{SO}_{2} \mathrm{Cl}_{2}(g)$ increases
(d) the amount of $\mathrm{SO}_{2}(g)$ decreases

Shahina -
Shahina -
Numerade Educator
01:49

Problem 90

Some inert gas is added at constant volume to the following reaction at equilibrium
$$
\mathrm{NH}_{4} \mathrm{HS}(s) \rightleftharpoons \mathrm{NH}_{3}(g)+\mathrm{H}_{2} \mathrm{~S}(g)
$$
Predict the effect of adding the inert gas:
(a) the equilibrium shifts in the forward direction
(b) the equilibrium shifts in the backward direction
(c) the equilibrium remains unaffected
(d) the value of $K_{p}$ is increased

Shahina -
Shahina -
Numerade Educator
02:17

Problem 91

Consider the reaction where $K_{p}=0.497$ at $500 \mathrm{~K}$
$$
\mathrm{PCl}_{5}(g) \rightleftharpoons \mathrm{PCl}_{3}(g)+\mathrm{Cl}_{2}(g)
$$
If the three gases are mixed in a rigid container so that the partial pressure of each gas in initially $1 \mathrm{~atm}$. Which is true ?
(a) More $\mathrm{PCl}_{5}$ will be produced
(b) More $\mathrm{PCl}_{3}$ will be produced
(c) Equilibrium will be established when $50 \%$ reaction is complete
(d) None of the above

Shahina -
Shahina -
Numerade Educator
02:14

Problem 92

The preparation of $\mathrm{SO}_{3}(g) \quad$ by reaction
$\mathrm{SO}_{2}(g)+\frac{1}{2} \mathrm{O}_{2}(g) \rightleftharpoons \mathrm{SO}_{3}(g)$ is an exothermic reaction. If the
preparation follows the following temperature-pressure relationship for its $\%$ yield, then for temperatures $T_{1}, T_{2}$ and $T_{3}$. The correct option is :
(a) $T_{3}>T_{2}>T_{1}$
(b) $T_{1}>T_{2}>T_{3}$
(c) $T_{1}=T_{2}=T_{3}$
(d) Nothing could be predicted about temperature through given

Shahina -
Shahina -
Numerade Educator
01:16

Problem 93

An equilibrium mixture at $700 \mathrm{~K}$ of $0.05 \mathrm{M} \mathrm{N}_{2}(g), 0.3 \mathrm{M} \mathrm{H}_{2}(g)$ and $0.2 \mathrm{M} \mathrm{NH}_{3}(g)$ is present in
a container. Now if this equilibrium is disturbed by adding $\mathrm{N}_{2}(\mathrm{~g})$ so that its concentration becomes $0.15 M$ just after addition then which of the following graphs represents the above situation more appropriately:

Deepanshu Kumar
Deepanshu Kumar
Numerade Educator
01:01

Problem 94

In a vessel containing $\mathrm{N}_{2}, \mathrm{H}_{2}$ and $\mathrm{NH}_{3}$ at equilibrium, some helium gas is introduced so that total pressure increase while temperature and volume remain constant. According to Le Chatelier's principle, the dissociation of $\mathrm{NH}_{3}$ :
(a) increases
(b) decreases
(c) remains unaltered
(d) changes unpredictably

Narayan Hari
Narayan Hari
Numerade Educator
01:02

Problem 95

Le-Chatelier principle is not applicable to :
(a) $\mathrm{H}_{2}(g)+\mathrm{I}_{2}(g) \rightleftharpoons 2 \mathrm{HI}(g)$
(b), $\mathrm{Fe}(s)+\mathrm{S}(s) \rightleftharpoons \mathrm{FeS}(s)$
(c) $\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \rightleftharpoons 2 \mathrm{NH}_{3}(g)$
(d) $\mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{NO}(g)$

Narayan Hari
Narayan Hari
Numerade Educator
02:05

Problem 96

Consider the following reactions. In which cases is the product formation favoured by decreased pressure?
(1) $\mathrm{CO}_{2}(g)+\mathrm{C}(s) \rightleftharpoons 2 \mathrm{CO}(g) ; \quad \Delta H^{\circ}=+172.5 \mathrm{~kJ}$
(2) $\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \rightleftharpoons 2 \mathrm{NH}_{3}(g) ; \quad \Delta H^{\circ}=-91.8 \mathrm{~kJ}$
(3) $\mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{NO}(g) ; \quad \Delta H^{\circ}=181 \mathrm{~kJ}$
(4) $2 \mathrm{H}_{2} \mathrm{O}(g) \rightleftharpoons 2 \mathrm{H}_{2}(g)+\mathrm{O}_{2}(g) ; \quad \Delta H^{\circ}=484.6 \mathrm{~kJ}$
(a) 2,3
(b) 3,4
(c) 2,4
(d) 1,4

Shahina -
Shahina -
Numerade Educator
05:05

Problem 97

Consider the following reactions. In which cases is product formation favoured by decreased temperature?
(1) $\mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{NO}(g) ; \quad \Delta H^{\circ}=181 \mathrm{~kJ}$
(2) $2 \mathrm{CO}_{2}(g) \rightleftharpoons 2 \mathrm{CO}(g)+\mathrm{O}_{2}(g) ; \quad \Delta H^{\circ}=566 \mathrm{~kJ}$
(3) $\mathrm{H}_{2}(g)+\mathrm{I}_{2}(g) \rightleftharpoons 2 \mathrm{HI}(g)$
$\Delta H^{\circ}=-9.4 \mathrm{~kJ}$
(4) $\mathrm{H}_{2}(g)+\mathrm{F}_{2}(g) \rightleftharpoons 2 \mathrm{HF}(g) ; \quad \Delta H^{\circ}=-541 \mathrm{~kJ}$
(a) 1,2
(b) 2 only
(c) $1,2,3$
(d) 3,4

Shalini Tyagi
Shalini Tyagi
Numerade Educator
03:23

Problem 98

For which of the following reactions is product formation favoured by low pressure and high temperature?
(a) $\mathrm{H}_{2}(g)+\mathrm{I}_{2}(g) \rightleftharpoons 2 \mathrm{HI}(g)$
$\Delta H^{\circ}=-9.4 \mathrm{~kJ}$
(b) $\mathrm{CO}_{2}(g)+\mathrm{C}(s) \rightleftharpoons 2 \mathrm{CO}(g)$
$\Delta H^{\circ}=172.5 \mathrm{~kJ}$
(c) $\mathrm{CO}(g)+2 \mathrm{H}_{2}(g) \rightleftharpoons \mathrm{CH}_{3} \mathrm{OH}$
$\Delta H^{\circ}=-21.7 \mathrm{~kJ}$
(d) $3 \mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{O}_{3}(g) ; \quad \Delta H^{\circ}=285 \mathrm{~kJ}$

Shahina -
Shahina -
Numerade Educator
03:23

Problem 99

For which of the following reaction is product formation favoured by low pressure and low temperature?
(a) $\mathrm{CO}_{2}(g)+\mathrm{C}(s) \rightleftharpoons 2 \mathrm{CO}(g) ; \quad \Delta H^{\circ}=172.5 \mathrm{~kJ}$
(b) $\mathrm{CO}(\mathrm{g})+2 \mathrm{H}_{2}(g) \rightleftharpoons \mathrm{CH}_{3} \mathrm{OH}$
$\Delta H^{\circ}=-21.7 \mathrm{~kJ}$
(c) $2 \mathrm{O}_{3}(g) \rightleftharpoons 3 \mathrm{O}_{2}(g)$
$\Delta H^{\circ}=-285 \mathrm{~kJ}$
(d) $\mathrm{H}_{2}(g)+\mathrm{F}_{2}(g) \rightleftharpoons 2 \mathrm{HF}(g)$
$\Delta H^{\circ}=-541 \mathrm{~kJ}$

Shahina -
Shahina -
Numerade Educator
07:12

Problem 100

Consider the following reactions at equilibrium and determine which of the indicated changes will cause the reaction to proceed to the right.
(1) $\mathrm{CO}(g)+3 \mathrm{H}_{2}(g) \rightleftharpoons \mathrm{CH}_{4}(g)+\mathrm{H}_{2} \mathrm{O}(g)\left(\right.$ add $\left.\mathrm{CH}_{4}\right)$
(2) $\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \rightleftharpoons 2 \mathrm{NH}_{3}(g)$
(remove $\mathrm{NH}_{3}$ )
(3) $\mathrm{H}_{2}(g)+\mathrm{F}_{2}(g) \rightleftharpoons 2 \mathrm{HF}(g)$
(add $\mathrm{F}_{2}$ )
(4) $\mathrm{BaO}(s)+\mathrm{SO}_{3}(g) \rightleftharpoons \mathrm{BaSO}_{4}(s)$
(add BaO)
(a) $2.3$
(b) $1.4$
(c) $2.4$
(d) $2,3,4$

Shalini Tyagi
Shalini Tyagi
Numerade Educator
03:50

Problem 101

If the pressure in a reaction vessel for the following reaction is increased by decreasing the volume, what will happen to the concentrations of $\mathrm{CO}$ and $\mathrm{CO}_{2}$ ?
$$
\mathrm{H}_{2} \mathrm{O}(g)+\mathrm{CO}(g) \rightleftharpoons \mathrm{H}_{2}(g)+\mathrm{CO}_{2}(g)+\text { Heat }
$$
(a) both the [CO] and [CO $\left._{2}\right]$ will decrease
(b) neither the [CO] nor the $\left[\mathrm{CO}_{2}\right]$ will change
(c) the [CO] will decrease and the [CO $_{2}$ ] will increase
(d) both the [CO] and [CO $\left._{2}\right]$ will increase

Shalini Tyagi
Shalini Tyagi
Numerade Educator
05:50

Problem 102

Consider the following reaction and determine which of the conditions will shift the equilibrium position to the right?
$$
4 \mathrm{NH}_{3}(g)+5 \mathrm{O}_{2}(g) \rightleftharpoons 4 \mathrm{NO}(g)+6 \mathrm{H}_{2} \mathrm{O}(g)+\text { Heat }
$$
(a) increasing the temperature
(b) increasing the pressure
(c) adding a catalyst
(d) none of the above is correct

Shalini Tyagi
Shalini Tyagi
Numerade Educator
04:53

Problem 103

The conversion of ozone into oxygen is exothermic. Under what conditions is ozone the most stable?
$$
2 \mathrm{O}_{3}(g) \rightleftharpoons 3 \mathrm{O}_{2}(g)
$$
(a) At low pressure and low temperature
(b) At high pressure and high temperature
(c) At high pressure and low temperature
(d) At low pressure and high temperature

Shalini Tyagi
Shalini Tyagi
Numerade Educator
01:09

Problem 104

A system at equilibrium is described by the equation of fixed temperature $T$.
$$
\mathrm{SO}_{2} \mathrm{Cl}_{2}(g) \rightleftharpoons \mathrm{SO}_{2}(g)+\mathrm{Cl}_{2}(g)
$$
What effect will an increases in the total pressure caused by a decrease in volume have on the equilibrium?

Narayan Hari
Narayan Hari
Numerade Educator
07:34

Problem 106

Densities of diamond and graphite are $3.5$ and $2.3 \mathrm{gm} / \mathrm{mL}$ $\mathrm{C}$ (diamond) $\rightleftharpoons \mathrm{C}$ (graphite); $\Delta_{r} H=-1.9 \mathrm{~kJ} / \mathrm{mol}$
favourable conditions for formation of graphite are :
(a) high pressure and low temperature
(b) low pressure and high temperature
(c) high pressure and high temperature
(d) low pressure and low temperature

Shalini Tyagi
Shalini Tyagi
Numerade Educator
04:28

Problem 107

For an equilibrium $\mathrm{H}_{2} \mathrm{O}(s) \rightleftharpoons \mathrm{H}_{2} \mathrm{O}(l)$, which of the following statements is true?
(a) The pressure changes do not affect the equilibrium
(b) More of ice melts if pressure on the system is increased
(c) More of liquid freezes if pressure on the system is increased
(d) The pressure changes may increase or decrease the degree of advancement of the process

Shalini Tyagi
Shalini Tyagi
Numerade Educator
04:10

Problem 108

A pressure cooker reduces cooking time for food because:
(a) the higher pressure inside the cooker crushes the food material
(b) cooking involves chemical changes helped by a rise in temperature
(c) heat is more evenly distributed in the cooking space
(d) boiling point of water involved in cooking is increased

Shalini Tyagi
Shalini Tyagi
Numerade Educator
05:41

Problem 109

The vapour pressure of a liquid in a closed container depends on :
(1) temperature of liquid
(2) quantity of liquid
(3) surface area of the liquid
(a) 1 only
(b) 2 only
(c) 1 and 3 only
(d) 1,2 and 3

Shalini Tyagi
Shalini Tyagi
Numerade Educator
01:03

Problem 110

The pressure on a sample of water at its triple point is reduced while the temperature is held constant. Which phases changes are favoured?
(I) melting of ice
(II) sublimation of ice
(III) vaporization of liquid water
(a) I only
(b) III only
(c) II only
(d) II and III

Ajay Singhal
Ajay Singhal
Numerade Educator
02:35

Problem 111

\text { An exothermic reaction is represented by the graph : }

Rashmi Gondi
Rashmi Gondi
Numerade Educator
02:35

Problem 112

\text { An endothermic reaction is represented by the graph : }

Rashmi Gondi
Rashmi Gondi
Numerade Educator
01:17

Problem 113

\text { A schematic plot of } \ln K_{e q} \text { versus inverse of temperature for a reaction is shown below }
the reaction must be :
(a) Exothermic
(b) Endothermic
(c) One with negligible enthalpy change
(d) Highly spontaneous at ordinam to

Mahipal Kumawat
Mahipal Kumawat
Numerade Educator
03:26

Problem 114

What is the correct relationship between free energy change and equilibrium constant of a reaction :
(a) $\Delta G^{\circ}=R T \ln K$
(b) $\Delta G^{\circ}=-R T \ln K$
(c) $\Lambda G=B T \ln K$
(d) $\Delta G=-R T \ln K$

Shalini Tyagi
Shalini Tyagi
Numerade Educator
04:58

Problem 115

For the chemical equilibrium $\mathrm{CaCO}_{3}(s) \rightleftharpoons \mathrm{CaO}(s)+\mathrm{CO}_{2}(g), \Delta H_{r}^{0}$ can be determined from
which one of the following plots ?

Kevin Zaborsky
Kevin Zaborsky
Numerade Educator
01:01

Problem 116

$K_{p}$ has the value of $10^{-6}$ atm $^{3}$ and $10^{-4} \mathrm{~atm}^{3}$ at $298 \mathrm{~K}$ and $323 \mathrm{~K}$ respectively for the reaction
$$
\mathrm{CuSO}_{4} \cdot 3 \mathrm{H}_{2} \mathrm{O}(s) \rightleftharpoons \mathrm{CuSO}_{4}(s)+3 \mathrm{H}_{2} \mathrm{O}(g)
$$
$\Delta_{\mathrm{r}} H^{\circ}$ for the reaction is :
(a). $7.7 \mathrm{~kJ} / \mathrm{mol}$
(b) $-147.41 \mathrm{~kJ} / \mathrm{mol}$
(c) $147.41 \mathrm{~kJ} / \mathrm{mol}$
(d) None of

Narayan Hari
Narayan Hari
Numerade Educator
04:37

Problem 117

van't Hoffs equation shows the effect of temperature on equilibrium constants $K_{c}$ and $K_{p} .$ The $K_{p}$ varies with temperature according to the relation :
(a) $\log \frac{K_{p_{2}}}{K_{p_{1}}}=\frac{\Delta H^{\circ}}{2.303 R}\left(\frac{T_{1}-T_{2}}{T_{1} T_{2}}\right)$
(b) $\log \frac{K_{p_{2}}}{K_{p_{1}}}=\frac{\Delta H^{\circ}}{2.303 R}\left(\frac{T_{2}-T_{1}}{T_{1} T_{2}}\right)$

Natalie Almond
Natalie Almond
Numerade Educator
05:14

Problem 118

For a reaction, the value of $K_{p}$ increases with increase in temperature. The $\Delta H$ for the reaction would be :
(a) positive
(b) negative
(c) zero
(d) cannot be predicted

Shalini Tyagi
Shalini Tyagi
Numerade Educator
04:07

Problem 119

The most stable oxides of nitrogen will be :
(a) $2 \mathrm{NO}_{2}(g) \rightleftharpoons \mathrm{N}_{2}(g)+2 \mathrm{O}_{2}(g) ; \quad K=6.7 \times 10^{16} \mathrm{~mol} \mathrm{~L}^{-1}$
(b) $2 \mathrm{~N}_{2} \mathrm{O}_{5}(g) \rightleftharpoons 2 \mathrm{~N}_{2}(g)+5 \mathrm{O}_{2}(g) ; \quad K=1.2 \times 10^{24} \mathrm{~mol}^{5} \mathrm{~L}^{-5}$
(c) $2 \mathrm{NO}(g) \rightleftharpoons \mathrm{N}_{2}(g)+\mathrm{O}_{2}(g)$
$K=2.2 \times 10^{30}$
(d) $2 \mathrm{~N}_{2} \mathrm{O}(g) \rightleftharpoons 2 \mathrm{~N}_{2}(g)+\mathrm{O}_{2}(g) ; \quad K=3.5 \times 10^{33} \mathrm{~mol} \mathrm{~L}^{-1}$

Shalini Tyagi
Shalini Tyagi
Numerade Educator
02:53

Problem 120

When 1 mole of pure ethyl alcohol $\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\right)$ is mixed with 1 mole of acetic acid at $25^{\circ} \mathrm{C}$, the equilibrium mixture contains $2 / 3$ mole each of ester and water
$$
\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(l)+\mathrm{CH}_{3} \mathrm{COOH}(l) \rightleftharpoons \mathrm{CH}_{3} \mathrm{COOC}_{2} \mathrm{H}_{5}(l)+\mathrm{H}_{2} \mathrm{O}
$$
The $\Delta G^{\circ}$ for the reaction at $298 \mathrm{~K}$ is :
(a) $3435 \mathrm{~J}$
(b) $4 \mathrm{~J}$
(c) $-3435 \mathrm{~J}$
(d) Zero

Shahina -
Shahina -
Numerade Educator
01:27

Problem 121

The value of $\Delta G^{\circ}$ for a reaction $^{\circ}$ in aqueous phase having $K_{c}=1$, would be :
(a) $-R T$
(b) $-1$
(c) 0
(d) $+R T$

Ishu Khandelwal
Ishu Khandelwal
Numerade Educator
02:48

Problem 122

A plot of Gibbs energy of a reaction mixture against the extent of the reaction is :
(a) minimum at equilibrium
(b) zero at equilibrium
(c) maximum at equilibrium
(d) None of these

Shahina -
Shahina -
Numerade Educator
03:30

Problem 123

For the reaction at $300 \mathrm{~K}$
$$
\begin{gathered}
A(g) \rightleftharpoons V(g)+S(g) \\
\Delta_{r} H^{\circ}=-30 \mathrm{~kJ} / \mathrm{mol}, \Delta_{r} S^{\circ}=-0.1 \mathrm{~kJ} \cdot \mathrm{K}^{-1} \cdot \mathrm{mol}^{-1}
\end{gathered}
$$
What is the value of equilibrium constant?
(a) 0
(b) 1
(c) 10
(d) None of these

Shahina -
Shahina -
Numerade Educator
01:17

Problem 124

Solid $\mathrm{Ca}\left(\mathrm{HCO}_{3}\right)_{2}$ decomposes as $\mathrm{Ca}\left(\mathrm{HCO}_{3}\right)_{2}(s) \rightleftharpoons \mathrm{CaCO}_{3}(s)+\mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)$
If the total pressure is $0.2$ bar at $420 \mathrm{~K}$, what is the standard free energy change for the given reaction $\left(\Delta_{r} G^{\circ}\right) ?$
(a) $840 \mathrm{~kJ} / \mathrm{mol}$
(b) $3.86 \mathrm{~kJ} / \mathrm{mol}$
(c) $6.98 \mathrm{~kJ} / \mathrm{mol}$
(d) $16.083 \mathrm{~kJ} / \mathrm{mol}$

Narayan Hari
Narayan Hari
Numerade Educator
03:11

Problem 125

The standard free energy change of a reaction is $\Delta G^{\circ}=-115 \mathrm{~kJ}$ at $298 \mathrm{~K}$. Calculate the value of $\log _{10} K_{p}\left(R=8.314 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}\right)$
(a) $20.16$
(b) $2.303$
(c) $2.016$
(d) $13.83$

Shahina -
Shahina -
Numerade Educator