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43 Years JEE ADVANCED (1978-2020) + JEE MAIN Chapterwise & Topicwise Solved Papers Chemistry

Disha Experts

Chapter 7

Equilibrium - all with Video Answers

Educators

TG

Section 1

Topic 1 : Chemical Equlibrium

01:05

Problem 1

For the reaction
$\mathrm{Fe}_{2} \mathrm{~N}(\mathrm{~s})+\frac{3}{2} \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{Fe}(\mathrm{s})+\mathrm{NH}_{3}(\mathrm{~g})$
(a) $K_{\mathrm{c}}=K_{\mathrm{p}}(\mathrm{RT})$
(b) $K_{\mathrm{c}}=K_{\mathrm{p}}(\mathrm{RT})^{\frac{-1}{2}}$
(c) $K_{\mathrm{c}}=K_{\mathrm{p}}(\mathrm{RT})^{\frac{1}{2}}$
(d) $K_{\mathrm{c}}=K_{\mathrm{p}}(\mathrm{RT})^{\frac{3}{2}}$

TG
Tanish Gupta
Numerade Educator
03:45

Problem 2

The variation of equilibrium constant with temperature is given below:
$$
\begin{array}{ll}
{\text { Temperature }} & {\text { Equilibrium Constant }} \\
\mathrm{T}_{1}=25^{\circ} \mathrm{C} & \mathrm{K}_{1}=10 \\
\mathrm{~T}_{2}=100{ }^{\circ} \mathrm{C} & \mathrm{K}_{2}=100
\end{array}
$$
The values of $\Delta \mathrm{H}^{\circ}, \Delta \mathrm{G}^{\circ}$ at $\mathrm{T}_{1}$ and $\Delta \mathrm{G}^{\circ}$ at $\mathrm{T}_{2}$ (in $\mathrm{kj} \mathrm{mol}^{-1}$ ) respectively, are close to
[use $\left.\mathrm{R}=8.314 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right]$
(a) $28.4,-7.14$ and $-5.71$
(b) $0.64,-7.14$ and $-5.71$
(c) $28.4,-5.71$ and $-14.29$
(d) $0.64,-5.71$ and $-14.29$

TG
Tanish Gupta
Numerade Educator
01:54

Problem 3

The value of $\mathrm{Kc}$ is 64 at $800 \mathrm{~K}$ for the reaction $\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_{3}(\mathrm{~g}) .$ The value of $K_{\mathrm{c}}$ for the following
reaction is :
$\mathrm{NH}_{3}(\mathrm{~g}) \rightleftharpoons \frac{1}{2} \mathrm{~N}_{2}(\mathrm{~g})+\frac{3}{2} \mathrm{H}_{2}(\mathrm{~g})$
(a) $1 / 64$
(b) 8
(c) $1 / 4$
(d) $1 / 8$

TG
Tanish Gupta
Numerade Educator
02:12

Problem 4

Consider the following reaction:
$\mathrm{N}_{2} \mathrm{O}_{4}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}_{2}(\mathrm{~g}) ; \mathrm{DH}^{0}=+58 \mathrm{~kJ}$
For each of the following cases ((i), (ii)), the direction in which the equilibrium shifts is :
(i) Temperature is decreases
(ii) Pressure is increased by adding $\mathrm{N}_{2}$ at constant $\mathrm{T}$.
(a) (i) towards product, (ii) towards product
(b) (i) towards reactant, (ii) towards product
(c) (i) towards reactant, (ii) no change
(d) (i) towards product, (ii) no change

TG
Tanish Gupta
Numerade Educator
01:53

Problem 5

For the equilibrium $\mathrm{A} \rightleftharpoons \mathrm{B}$, the variation of the rate of the forward (a) and reverse (b) reaction with time is given by:

TG
Tanish Gupta
Numerade Educator
01:35

Problem 6

If the equilibrium constant for $\mathrm{A} \rightleftharpoons \mathrm{B}+\mathrm{C}$ is $\mathrm{K}_{\mathrm{eq}}^{(1)}$ and that of $\mathrm{B}+\mathrm{C} \rightleftharpoons \mathrm{P}$ is $\mathrm{K}_{\mathrm{eq}}^{(2)}$, the equilibrium constant for $\mathrm{A} \rightleftharpoons \mathrm{P}$ is :
(a) $\mathrm{K}_{\mathrm{eq}}^{(1)} / \mathrm{K}_{\mathrm{eq}}^{(2)}$
(b) $\mathrm{K}_{\mathrm{eq}}^{(2)}-\mathrm{K}_{\mathrm{eq}}^{(1)}$
(c) $\mathrm{K}_{\mathrm{eq}}^{(1)}+\mathrm{K}_{\mathrm{eq}}^{(2)}$
(d) $\mathrm{K}_{\mathrm{eq}}^{(\mathrm{I})} \mathrm{K}_{\mathrm{eq}}^{(2)}$

TG
Tanish Gupta
Numerade Educator
01:12

Problem 7

In the figure shown below reactant $\mathrm{A}$ (represented by square) is in equilibrium with product B (represented by circle). The equilibrium constant is:
(a) 4
(b) 8
(c) 1
(d) 2

TG
Tanish Gupta
Numerade Educator
02:51

Problem 8

For the reaction, $2 \mathrm{SO}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{SO}_{3}(\mathrm{~g})$
$\mathrm{DH}=-57.2 \mathrm{~kJ} \mathrm{~mol}^{-1}$ and $\mathrm{K}_{\mathrm{c}}=1.7 \times 10^{16}$
Which of the following statement is INCORRECT? [Main April 10, 2019 (II)]
(a) The equilibrium constant is large suggestive of reaction going to completion and so no catalyst is required.
(b) The equilibrium will shift in forward direction as the pressure increases.
(c) The equilibrium constant decreases as the temperature increases.
(d) The addition of inert gas at constant volume will not affect the equilibrium constant.

TG
Tanish Gupta
Numerade Educator
02:06

Problem 9

In which one of the following equilibria, $\mathrm{K}_{\mathrm{p}} \neq \mathrm{K}_{\mathrm{c}}$ ?
(a) $2 \mathrm{C}(\mathrm{s})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{CO}(\mathrm{g})$
(b) $2 \mathrm{HI}(\mathrm{g}) \rightleftharpoons \mathrm{H}_{2}(\mathrm{~g})+\mathrm{I}_{2}(\mathrm{~g})$
(c) $\mathrm{NO}_{2}(\mathrm{~g})+\mathrm{SO}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{NO}(\mathrm{g})+\mathrm{SO}_{3}(\mathrm{~g})$
(d) $2 \mathrm{NO}(\mathrm{g}) \rightleftharpoons \mathrm{N}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g})$

TG
Tanish Gupta
Numerade Educator
02:41

Problem 10

For the equilibrium $2 \mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{H}_{3} \mathrm{O}^{+}+\mathrm{OH}^{-} ;$the value of $\square \mathrm{G}^{\circ}$ at
$298 \mathrm{~K}$ is approximately: [Main Jan. 11, 2019 (II)]
(a) $100 \mathrm{~kJ} \mathrm{~mol}^{-1}$
(b) $-80 \mathrm{~kJ} \mathrm{~mol}^{-1}$
(c) $80 \mathrm{~kJ} \mathrm{~mol}^{-1}$
(d) $-100 \mathrm{~kJ} \mathrm{~mol}^{-1}$

TG
Tanish Gupta
Numerade Educator
02:53

Problem 11

Consider the following reversible chemical reactions:
$\mathrm{A}_{2}(\mathrm{~g})+\mathrm{B}_{2}(\mathrm{~g}) \rightleftharpoons{\mathrm{K}_{\mathrm{I}}}{\rightleftharpoons} 2 \mathrm{AB}(\mathrm{g}) \ldots \ldots(1)$
$6 \mathrm{AB}(\mathrm{g}) \stackrel{\mathrm{K}_{2}}{\rightleftharpoons} 3 \mathrm{~A}_{2}(\mathrm{~g})+3 \mathrm{~B}_{2}(\mathrm{~g}) \ldots . .(2)$
The relation between $\mathrm{K}_{1}$ and $\mathrm{K}_{2}$ is:
(a) $\mathrm{K}_{1} \mathrm{~K}_{2}=\frac{1}{3}$
(b) $\mathrm{K}_{2}=\mathrm{K}_{1}$
(c) $\mathrm{K}_{2}=\mathrm{K}_{1}^{3}$
(d) $\mathrm{K}_{1} \mathrm{~K}_{2}=3$

TG
Tanish Gupta
Numerade Educator
03:05

Problem 12

In which of the following reactions, an increase in the volume of the container will favour the formation of products?
(a) $4 \mathrm{NH}_{3}(\mathrm{~g})+5 \mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 4 \mathrm{NO}(\mathrm{g})+6 \mathrm{H}_{2} \mathrm{O}$ (l)
(b) $2 \mathrm{NO}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{~g})$
(c) $3 \mathrm{O}_{2} \rightleftharpoons 2 \mathrm{O}_{3}(\mathrm{~g})$
(d) $\mathrm{H}_{2}(\mathrm{~g})+\mathrm{I}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{HI}(\mathrm{g})$

TG
Tanish Gupta
Numerade Educator
02:58

Problem 13

The following reaction occurs in the Blast Furnace where iron ore is reduced to iron metal :
$\mathrm{Fe}_{2} \mathrm{O}_{3}(\mathrm{~s})+3 \mathrm{CO}(\mathrm{g}) \rightleftharpoons 2 \mathrm{Fe}(1)+3 \mathrm{CO}_{2}(\mathrm{~g})$
Using the Le Chatelier's principle, predict which one of the following will not disturb the equilibrium?
(a) Removal of CO
(b) Removal of $\mathrm{CO}_{2}$
(c) Addition of $\mathrm{CO}_{2}$
(d) Addition of $\mathrm{Fe}_{2} \mathrm{O}_{3}$

TG
Tanish Gupta
Numerade Educator
02:51

Problem 14

The equilibrium constant at $298 \mathrm{~K}$ for a reaction $A+B \rightleftharpoons C+D$ is 100 . If the initial concentration of all the four species were $1 \mathrm{M}$ each, then equilibrium concentration of $D$ (in $\mathrm{mol} \mathrm{L}^{-1}$ ) will be :
(a) $1.818$
(b) $1.182$
(c) $0.182$
(d) $0.818$

TG
Tanish Gupta
Numerade Educator
01:28

Problem 15

A solid XY kept in an evacuated sealed container undergoes decomposition to form a mixture of gases $\mathrm{X}$ and $\mathrm{Y}$ at temperature $\mathrm{T}$. The equilibrium pressure is 10 bar in the vessel. $K_{\mathrm{p}}$ for this reaction is:
(a) 25
(b) 100
(c) 10
(d) 5

ra
Rajbala Aggarwal
Numerade Educator
01:36

Problem 16

The following reaction is performed at $298 \mathrm{~K}$. [Main 2015] $$2 \mathrm{NO}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}_{2}(\mathrm{~g})$$. The standard free energy of formation of $\mathrm{NO}(\mathrm{g})$ is $86.6 \mathrm{KJ} / \mathrm{mol}$ at $298 \mathrm{~K}$. What is the standard free energy of formation of $\mathrm{NO}_{2}(\mathrm{~g})$ at $298 \mathrm{~K} ?\left(K_{\mathrm{p}}\right.$ $\left.=1.6 \times 10^{12}\right)$.
(a) $86600-\frac{\ln \left(1.6 \times 10^{12}\right)}{\mathrm{R}(298)}$
(b) $\quad 0.5\left[2 \times 86,600-R(298) \ln \left(1.6 \times 10^{12}\right)\right]$
(c) $R(298) \ln \left(1.6 \times 10^{12}\right)-86600$
(d) $86600+R(298) \ln \left(1.6 \times 10^{12}\right)$

Rajesh Singh
Rajesh Singh
Numerade Educator
01:02

Problem 17

The increase of pressure on ice $\rightleftharpoons$ water system at constant temperature will lead to
(a) a decrease in the entropy of the system
(b) an increase in the Gibb's energy of the system
(c) no effect on the equilibrium
(d) a shift of the equilibrium in the forward direction

Dheeraj Sharma
Dheeraj Sharma
Numerade Educator
02:05

Problem 18

For the reaction $\mathrm{SO}_{2}(\mathrm{~g})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{SO}_{3}(\mathrm{~g})$, if $K_{\mathrm{p}}=K_{\mathrm{c}}(R T)^{x}$. where the symbols have usual meaning then the value of $x$ is (assuming ideality):
(a) $-1$
(b) $-\frac{1}{2}$
(c) $\frac{1}{2}$
(d) 1

Preeti Kumari
Preeti Kumari
Numerade Educator
01:49

Problem 19

What happens when an inert gas is added to an equilibrium keeping volume unchanged? [Main Online April 12, 2014]
(a) More product will form
(b) Less product will form
(c) More reactant will form
(d) Equilibrium will remain unchanged

Shahina -
Shahina -
Numerade Educator
03:38

Problem 20

In reaction $\mathrm{A}+2 \mathrm{~B} \rightleftharpoons 2 \mathrm{C}+\mathrm{D}$, initial concentration of $\mathrm{B}$ was $1.5$ times of $[\mathrm{A}]$, but at equilibrium the concentrations of $\mathrm{A}$ and $\mathrm{B}$ became equal. The equilibrium constant for the reaction is:
(a) 8
(b) 4
(c) 12
(d) 6

Rajesh Singh
Rajesh Singh
Numerade Educator
02:40

Problem 21

Solubility product constant $\left(K_{s p}\right)$ of salts of types $M X, M X_{2}$ and $M_{3} X$ at temperature $T$ are $4.0 \times 10^{-8}, 3.2 \times 10^{-14}$ and $2.7 \times 10^{-15}$, respectively. Solubilities (mol $\mathrm{dm}^{-3}$ ) of the salts at temperature ' $T$ are in the order
(a) $M X>M X_{2}>M_{3} X$
(b) $\mathrm{M}_{3} \mathrm{X}>\mathrm{MX}_{2}>\mathrm{MX}$
(c) $M X_{2}>M_{3} X>M X$
(d) $M X>M_{3} X>M X_{2}$

Gaurav Priyank
Gaurav Priyank
Numerade Educator
03:46

Problem 22

The Haber's process for the formation of $\mathrm{NH}_{3}$ at $298 \mathrm{~K}$ is
$\mathrm{N}_{2}+3 \mathrm{H}_{2} \rightleftharpoons 2 \mathrm{NH}_{3} ; \Delta H=-46.0 \mathrm{~kJ} ;$ Which of the following is the
correct statement
(a) The condition for equilibrium is
$$
G_{\mathrm{N}_{2}}+3 G_{\mathrm{H}_{2}}=2 G_{\mathrm{NH}_{3}}
$$
where $G$ is Gibb's free energy per mole of the gaseous species measured at that partial pressure.
(b) On adding $\mathrm{N}_{2}$, the equilibrium will shift to forward direction because according to $\mathrm{II}^{\text {nd }}$ law of thermodynamics, the entropy must increase in the direction of spontaneous reaction
(c) The catalyst will increase the rate of forward reaction by 2 times and that of backward reaction by $1.5$ times
(d) None of these

Deepanshu Kumar
Deepanshu Kumar
Numerade Educator
01:08

Problem 23

Consider the following equilibrium in a closed container
$$
\mathrm{N}_{2} \mathrm{O}_{4}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}_{2}(\mathrm{~g})
$$
At a fixed temperature, the volume of the reaction container is halved. For this change, which of the following statements holds true regarding the equilibrium constant $\left(K_{p}\right)$ and degree of dissociation $(\alpha)$ ?
(a) neither $K_{p}$ nor $\alpha$ changes
(b) both $K_{p}$ and $\alpha$ change
(c) $K_{p}$ changes, but $\alpha$ does not change
(d) $K_{p}$ does not change, but $\alpha$ changes

Akhil Choudhary
Akhil Choudhary
Numerade Educator
01:01

Problem 24

At constant temperature, the equilibrium constant $\left(K_{p}\right)$ for the decomposition reaction $\mathrm{N}_{2} \mathrm{O}_{4} \rightleftharpoons 2 \mathrm{NO}_{2}$ is expressed by $K_{p}=$ $\left(4 x^{2} P\right) /\left(1-x^{2}\right)$, where $P=$ pressure, $x=$ extent of decomposition. Which one of the following statements is true? [2001S]
(a) $K_{p}$ increases with increase of $P$
(b) $K_{p}$ increases with increase of $x$
(c) $K_{p}$ increases with decrease of $x$
(d) $K_{p}$ remains constant with change in $P$ and $x$

Narayan Hari
Narayan Hari
Numerade Educator
01:36

Problem 25

For a sparingly soluble salt $A_{p} B_{q}$, the relationship of its solubility product $\left(L_{S}\right)$ with its solubility $(S)$ is [2001S]
(a) $L_{S}=S^{p+q} \cdot p^{p} \cdot q^{q}$
(b) $L_{S}=S^{p+q} \cdot p^{q} \cdot q^{p}$
(c) $L_{S}=S^{p q} \cdot p^{p} \cdot q^{q}$
(d) $L_{S}=S^{p q} \cdot(p q)^{p+q}$

Hitendra Singh
Hitendra Singh
Numerade Educator
01:29

Problem 26

When two reactants, $A \& B$ are mixed to give products $C \& D$, the reaction quotient $Q$, at the initial stages of the reaction [2000S]
(a) is zero
(b) decreases with time
(c) is independent of time
(d) increases with time

ra
Rajbala Aggarwal
Numerade Educator
05:06

Problem 27

For the reversible reaction, $\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_{3}(\mathrm{~g})$ 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) $\frac{1.44 \times 10^{-5}}{(0.082 \times 500)^{-2}}$
(b) $\frac{1.44 \times 10^{-5}}{(8.314 \times 773)^{-2}}$
(c) $\frac{1.44 \times 10^{-5}}{(0.082 \times 773)^{2}}$
(d) $\frac{1.44 \times 10^{-5}}{(0.082 \times 773)^{-2}}$

Shalini Tyagi
Shalini Tyagi
Numerade Educator
01:02

Problem 28

For the chemical reaction $3 X(\mathrm{~g})+Y(\mathrm{~g}) \rightleftharpoons X_{3} Y(\mathrm{~g})$, the amount of $X_{3} Y$ at equilibrium is affected by [1999 - 2 Marks]
(a) temperature and pressure
(b) temperature only
(c) pressure only
(d) temperature, pressure and catalyst

Akhil Choudhary
Akhil Choudhary
Numerade Educator
03:11

Problem 29

Amongst the following hydroxides, the one which has the lowest value of $K_{s p}$ at ordinary temperature (about $25^{\circ} \mathrm{C}$ ) is [1990-1 Mark]
(a) $\mathrm{Mg}(\mathrm{OH})_{2}$
(b) $\mathrm{Ca}(\mathrm{OH})_{2}$
(c) $\mathrm{Ba}(\mathrm{OH})_{2}$
(d) $\mathrm{Be}(\mathrm{OH})_{2}$

Preeti Kumari
Preeti Kumari
Numerade Educator
00:29

Problem 30

When equal volumes of the following solutions are mixed, precipitation of $\mathrm{AgCl}\left(\mathrm{K}_{\mathrm{sp}}=1.8 \times 10^{-10}\right)$ will occur only with
(a) $10^{-4} \mathrm{M}\left(\mathrm{Ag}^{+}\right)$and $10^{-4} \mathrm{M}\left(\mathrm{Cl}^{-}\right)$
(b) $10^{-5} \mathrm{M}\left(\mathrm{Ag}^{+}\right)$and $10^{-5} \mathrm{M}\left(\mathrm{Cl}^{-}\right)$
(c) $10^{-6} \mathrm{M}\left(\mathrm{Ag}^{+}\right)$and $10^{-6} \mathrm{M}\left(\mathrm{Cl}^{-}\right)$
(d) $10^{-10} \mathrm{M}\left(\mathrm{Ag}^{+}\right)$and $10^{-10} \mathrm{M}\left(\mathrm{Cl}^{-}\right)$

Akhil Choudhary
Akhil Choudhary
Numerade Educator
01:01

Problem 31

An example of a reversible reaction is :
(a) $\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2} \mathrm{aq}+2 \mathrm{NaI}(\mathrm{aq}) \rightarrow \mathrm{PbI}_{2}(\mathrm{~s})+2 \mathrm{NaNO}_{3}(\mathrm{aq})$
(b) $\mathrm{AgNO}_{3}(\mathrm{aq})+\mathrm{HCl}(\mathrm{aq}) \rightarrow \mathrm{AgCl}(\mathrm{s})+\mathrm{NaNO}_{3}(\mathrm{aq})$
(c) $2 \mathrm{Na}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(1) \rightarrow 2 \mathrm{NaOH}(\mathrm{aq})+\mathrm{H}_{2}(\mathrm{~g})$
(d) $\mathrm{KNO}_{3}(\mathrm{aq})+\mathrm{NaCl}(\mathrm{aq}) \rightarrow \mathrm{KCl}(\mathrm{aq})+\mathrm{NaNO}_{3}(\mathrm{aq})$

Narayan Hari
Narayan Hari
Numerade Educator
01:26

Problem 32

Pure ammonia is placed in a vessel at a temperature where its dissociation constant $(\alpha)$ is appreciable. At equilibrium:
(a) $K_{p}$ does not change significantly with pressure.
(b) $\alpha$ does not change with pressure.
(c) concentration of $\mathrm{NH}_{3}$ does not change with pressure.
(d) concentration of hydrogen is less than that of nitrogen.

Hitendra Singh
Hitendra Singh
Numerade Educator
01:01

Problem 33

A liquid is in equilibrium with its vapour at its boiling point. On the average, the molecules in the two phases have equal :
(a) inter-molecular forces
(b) potential energy
(c) total energy
(d) kinetic energy

Narayan Hari
Narayan Hari
Numerade Educator
01:00

Problem 34

The precipitate of $$\mathrm{CaF}_{2}\left(K_{s p}=1.7 \times 10^{-10}\right)$$ is obtained when equal volumes of the following are mixed
(a) $10^{-4} \mathrm{M} \mathrm{Ca}^{2+}+10^{-4} \mathrm{M} \mathrm{F}^{-}$
(b) $10^{-2} \mathrm{M} \mathrm{Ca}^{2+}+10^{-3} \mathrm{M} \mathrm{F}^{-}$
(c) $10^{-5} \mathrm{M} \mathrm{Ca}^{2+}+10^{-3} \mathrm{M} \mathrm{F}^{-}$
(d) $10^{-3} \mathrm{M} \mathrm{Ca}^{2+}+10^{-5} \mathrm{M} \mathrm{F}^{-}$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:45

Problem 35

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

Ishu Khandelwal
Ishu Khandelwal
Numerade Educator
00:39

Problem 36

The oxidation of $\mathrm{SO}_{2}$ by $\mathrm{O}_{2}$ to $\mathrm{SO}_{3}$ is an exothermic reaction. The yield of $\mathrm{SO}_{3}$ will be maximum if [1981-1 Mark]
(a) temperature is increased and pressure is kept constant
(b) temperature is reduced and pressure is increased
(c) both temperature and pressure are increased
(d) both temperature and pressure are reduced

Akhil Choudhary
Akhil Choudhary
Numerade Educator
01:10

Problem 37

Molten sodium chloride conducts electricitry due to the presence of [1981-1 Mark]
(a) free electrons
(b) free ions
(c) free molecules
(d) atoms of sodium and chlorine

Narayan Hari
Narayan Hari
Numerade Educator
01:39

Problem 38

In 1 L saturated solution of $\mathrm{AgCl}\left[\mathrm{Ksp}(\mathrm{AgCl})=1.6 \times 10^{-10}\right], 0.1 \mathrm{~mol}$ of $\mathrm{CuCl}\left[K_{s p}(\mathrm{CuCl})=1.0 \times 10^{-6}\right]$ is added. The resultant concentration of $\mathrm{Ag}^{+}$in the solution is $1.6 \times 10^{-x}$. The value of " $x$ " is

David Collins
David Collins
Numerade Educator
02:01

Problem 39

For a reaction $\mathrm{X}+\mathrm{Y} \rightleftharpoons 2 \mathrm{Z}, 1.0 \mathrm{~mol}$ of $\mathrm{X}, 1.5 \mathrm{~mol}$ of $\mathrm{Y}$ and $0.5 \mathrm{~mol}$
of $Z$ were taken in a 1 L vessel and allowed to react. At equilibrium, the concentration of $Z$ was $1.0 \mathrm{~mol} \mathrm{~L}^{-1} .$ The equilibrium constant of
the reaction is $\frac{x}{15} .$ The value of $x$ is _________.

John Nicolle
John Nicolle
Numerade Educator
02:57

Problem 40

Consider the reaction $\mathbf{A} \rightleftharpoons \mathbf{B}$ at $1000 \mathrm{~K}$. At time $t^{\prime}$, the temperature of the system was increased to $2000 \mathrm{~K}$ and the system was allowed to reach equilibrium. Throughout this experiment the partial pressure of A was maintained at 1 bar. Given below is the plot of the partial pressure of $\mathbf{B}$ with time. What is the ratio of the standard Gibbs energy of the reaction at $1000 \mathrm{~K}$ to that at $2000 \mathrm{~K} ?$

Natalie Almond
Natalie Almond
Numerade Educator
01:50

Problem 41

For the following reaction, the equilibrium constant $K_{c}$ at $298 \mathrm{~K}$ is $1.6$ $\times 10^{17}$
$$
\mathrm{Fe}^{2+}(\mathrm{aq})+\mathrm{S}^{2-}(\mathrm{aq}) \rightleftharpoons \mathrm{FeS}(\mathrm{s})
$$
When equal volumes of $0.06 \mathrm{M} \mathrm{Fe}^{2+}$ (aq) and $0.2 \mathrm{M} \mathrm{S}^{2-}$ (aq) solutions are mixed, the equilibrium concentration of $\mathrm{Fe}^{2+}$ (aq) is found to be $Y \times$ $10^{-17} \mathrm{M}$. The value of $Y$ is

Stephen Ho
Stephen Ho
Numerade Educator
04:53

Problem 42

An aqueous solution of a metal bromide $M \mathrm{Br}_{2}(0.05 \mathrm{M})$ is saturated with $\mathrm{H}_{2} \mathrm{~S}$. What is the minimum $\mathrm{pH}$ at which $M \mathrm{~S}$ will precipitate? [1993 - 3 Marks] $K_{s p}$ for $M \mathrm{~S}=6.0 \times 10^{-21} ;$ concentration of saturated $\mathrm{H}_{2} \mathrm{~S}=0.1 \mathrm{M}$
$K_{1}=10^{-7}$ and $K_{2}=1.3 \times 10^{-13}$, for $\mathrm{H}_{2} \mathrm{~S}$.

SO
Stephanie Orozco
Numerade Educator
01:30

Problem 43

The equilibrium constant of the reaction $A_{2}(\mathrm{~g})+B_{2}(\mathrm{~g}) \rightleftharpoons 2 A B(\mathrm{~g})$ at $100^{\circ} \mathrm{C}$ is 50 . If a one litre flask, containing one mole of $A_{2}$ is connected to a two litre flask, containing two mole of $B_{2}$, how many mole of $A B$ will be formed at $373^{\circ} \mathrm{C}$ ?

Narayan Hari
Narayan Hari
Numerade Educator
02:58

Problem 44

A ten-fold increase in pressure on the reaction, $\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons$ $2 \mathrm{NH}_{3}(\mathrm{~g})$ at equilibrium results in $\ldots .$ in $K_{P}$

Ronald Prasad
Ronald Prasad
Numerade Educator
00:58

Problem 45

For a given reversible reaction at a fixed temperature, equilibrium constants $K_{p}$ and $K_{c}$ are related by........

Ronald Prasad
Ronald Prasad
Numerade Educator
00:49

Problem 46

Solubility of sodium hydroxide increases with increase in temperature.

Nicole Smina
Nicole Smina
Numerade Educator
02:29

Problem 47

When a liquid and its vapour are at equilibrium and the pressure is suddenly decreased, cooling occurs.

Theodore Donnell
Theodore Donnell
Numerade Educator
00:36

Problem 48

If equilibrium constant for the reaction $A_{2}+B_{2} \rightleftharpoons 2 A B$, is $K$, then for the backward reaction $A B \rightleftharpoons 1 / 2 A_{2}+1 / 2 B_{2}$, the equilibrium constant is $1 / K$.

Rory Naguib
Rory Naguib
Numerade Educator
02:44

Problem 49

The \%yield of ammonia as a function of time in the reaction $\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_{3}(\mathrm{~g}), \Delta H<0$ at $\left(P, T_{1}\right)$ is given below

Eileen Sullivan
Eileen Sullivan
Numerade Educator
01:07

Problem 50

The thermal dissociation equilibrium of $\mathrm{CaCO}_{3}$ (s) is studied under different conditions $\mathrm{CaCO}_{3}(\mathrm{~s}) \rightleftharpoons \mathrm{CaO}(\mathrm{s})+\mathrm{CO}_{2}(\mathrm{~g}) .$ For this equilibrium, the correct
statement(s) is (are)
(a) $\Delta H$ is dependent on $T$
(b) $K$ is independent of the initial amount of $\mathrm{CaCO}_{3}$
(c) $K$ is dependent on the pressure of $\mathrm{CO}_{2}$ at a given $T$
(d) $\Delta H$ is independent of catalyst, if any

Deepanshu Kumar
Deepanshu Kumar
Numerade Educator
03:52

Problem 51

The $K_{s p}$ of $\mathrm{Ag}_{2} \mathrm{CrO}_{4}$ is $1.1 \times 10^{-12}$ at $298 \mathrm{~K}$. The solubility (in $\mathrm{mol} / \mathrm{L}$ ) of $\mathrm{Ag}_{2} \mathrm{CrO}_{4}$ in a $0.1 \mathrm{M} \mathrm{AgNO}_{3}$ solution is
(a) $1.1 \times 10^{-11}$
(b) $1.1 \times 10^{-10}$
(c) $1.1 \times 10^{-12}$
(d) $1.1 \times 10^{-9}$

Adriano Chikande
Adriano Chikande
Numerade Educator
01:01

Problem 52

For the reaction $\mathrm{CO}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \rightleftharpoons \mathrm{CO}_{2}(\mathrm{~g})+\mathrm{H}_{2}(\mathrm{~g})$ at a given temperature, the equilibrium amount of $\mathrm{CO}_{2}(\mathrm{~g})$ can be increased by [1998 - 2 Marks]
(a) adding a suitable catalyst
(b) adding an inert gas
(c) decreasing the volume of the container
(d) increasing the amount of $\mathrm{CO}(\mathrm{g})$.

Narayan Hari
Narayan Hari
Numerade Educator
02:18

Problem 53

For the reaction :
$$
\mathrm{PCl}_{5}(\mathrm{~g}) \rightarrow \mathrm{PCl}_{3}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g})
$$
The forward reaction at constant temperature is favoured by
(a) introducing an inert gas at constant volume
(b) introducing chlorine gas at constant volume
(c) introducing an inert gas at constant pressure
(d) increasing the volume of the container
(e) introducing $\mathrm{PCl}_{5}$ at constant volume

Prachi Joshi
Prachi Joshi
Numerade Educator
02:07

Problem 54

The equilibrium :
$$
\begin{gathered}
\text { [1989-1 Mark] } \\
\mathrm{SO}_{2} \mathrm{Cl}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{SO}_{2}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g})
\end{gathered}
$$
is attained at $25^{\circ} \mathrm{C}$ in a closed container and an inert gas, helium is introduced. Which of the following statements are correct?
(a) Concentration of $\mathrm{SO}_{2}, \mathrm{Cl}_{2}$ and $\mathrm{SO}_{2} \mathrm{Cl}_{2}$ do not change
(b) More chlorine is formed
(c) Concentration of $\mathrm{SO}_{2}$ is reduced
(d) More $\mathrm{SO}_{2} \mathrm{Cl}_{2}$ is formed.

Prachi Joshi
Prachi Joshi
Numerade Educator
03:57

Problem 55

When $\mathrm{NaNO}_{3}$ is heated in a closed vessel, oxygen is liberated and $\mathrm{NaNO}_{2}$ is left behind. At equilibrium. [1986-1 Mark]
(a) addition of $\mathrm{NaNO}_{2}$ favours reverse reaction
(b) addition of $\mathrm{NaNO}_{3}$ favours forward reaction
(c) increasing temperature favours forward reaction
(d) increasing pressure favours reverse reaction

Deepanshu Kumar
Deepanshu Kumar
Numerade Educator
02:56

Problem 56

For the gas phase reaction :
$$\mathrm{C}_{2} \mathrm{H}_{4}+\mathrm{H}_{2} \rightleftharpoons \mathrm{C}_{2} \mathrm{H}_{6}(\Delta H=-32.7 \mathrm{kcal})$$
carried out in a vessel, the equilibrium concentration of $\mathrm{C}_{2} \mathrm{H}_{4}$ can be increased by :
(a) increasing the temperature
(b) decreasing the pressure
(c) removing some $\mathrm{H}_{2}$
(d) adding some $\mathrm{C}_{2} \mathrm{H}_{6}$

Deepanshu Kumar
Deepanshu Kumar
Numerade Educator
01:54

Problem 57

Each question contains STATEMENT-1 (Assertion) and STATEMENT-2 (Reason). Each question has 5 choices (a), (b), (c) and (d) out of which ONLY ONE is correct. Mark your answer as
Statement $-1$ For every chemical reaction at equilibrium, standard Gibbs energy of reaction is zero.
Statement $-2$ At constant temperature and pressure, chemical reactions are spontaneous in the direction of decreasing Gibbs energy.

Ramesh Singh
Ramesh Singh
Numerade Educator
02:49

Problem 58

Statement $-1$ The endothermic reactions are favoured at lower temperature and the exothermic reactions are favoured at higher temperature.
Statement $-2$ When a system in equilibrium is disturbed by changing the temperature, it will tend to adjust itself so as to overcome the effect of change.

Deepanshu Kumar
Deepanshu Kumar
Numerade Educator
01:12

Problem 59

When $3.06 \mathrm{~g}$ of solid $\mathrm{NH}_{4} \mathrm{HS}$ is introduced into a two litre evacuated flask at $27^{\circ} \mathrm{C}, 30 \%$ of the solid decomposes into gaseous ammonia and hydrogen sulphide. (i) Calculate $K_{c}$ and $K_{p}$ for the reaction at $27^{\circ} \mathrm{C}$. (ii) What would happen to the equilibrium when more solid $\mathrm{NH}_{4} \mathrm{HS}$ is introduced into the flask?

Eileen Sullivan
Eileen Sullivan
Numerade Educator
01:39

Problem 60

Given : $\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}^{+} \rightleftharpoons \mathrm{Ag}^{+}+2 \mathrm{NH}_{3}, K_{c}=6.2 \times 10^{-8}$ and $K_{s p}$ of
$\mathrm{AgCl}=1.8 \times 10^{-10}$ at $298 \mathrm{~K}$. If ammonia is added to a water solution containing excess of $\mathrm{AgCl}(\mathrm{s})$ only, calculate the concentration of the complex in $1.0 \mathrm{M}$ aqueous ammonia.

David Collins
David Collins
Numerade Educator
01:53

Problem 61

A sample of $\mathrm{AgCl}$ was treated with $5.00 \mathrm{~mL}$ of $1.5 \mathrm{M} \mathrm{Na}_{2} \mathrm{CO}_{3}$ solution to give $\mathrm{Ag}_{2} \mathrm{CO}_{3} .$ The remaining solution contained $0.0026 \mathrm{~g}$ of $\mathrm{Cl}^{-}$per litre. Calculate the solubility product of $\mathrm{AgCl}\left(K_{s p}\left(\mathrm{Ag}_{2} \mathrm{CO}_{3}\right)=8.2 \times\right.$ $\left(0^{-12}\right)$

David Collins
David Collins
Numerade Educator
01:13

Problem 62

62. For the reaction
$$
\left[\mathrm{Ag}(\mathrm{CN})_{2}\right]^{-} \rightleftharpoons \mathrm{Ag}^{+}+2 \mathrm{CN}^{-}
$$
the equilibrium costant, at $25^{\circ} \mathrm{C}$, is $4.0 \times 10^{-19} .$ Calculate the silver ion concentration in a solution which was originally $0.10$ molar in KCN and $0.03$ molar in $\mathrm{AgNO}_{3}$.

Akhil Choudhary
Akhil Choudhary
Numerade Educator
01:13

Problem 63

For the reaction
$$
\left[\mathrm{Ag}(\mathrm{CN})_{2}\right]^{-} \rightleftharpoons \mathrm{Ag}^{+}+2 \mathrm{CN}^{-}
$$
the equilibrium costant, at $25^{\circ} \mathrm{C}$, is $4.0 \times 10^{-19} .$ Calculate the silver ion concentration in a solution which was originally $0.10$ molar in KCN and $0.03$ molar in $\mathrm{AgNO}_{3}$.

Akhil Choudhary
Akhil Choudhary
Numerade Educator
09:57

Problem 64

$0.15$ mole of $\mathrm{CO}$ taken in a $2.5 \mathrm{~L}$ flask is maintained at $750 \mathrm{~K}$ along with a catalyst so that the following reaction can take place :
$$
\mathrm{CO}(\mathrm{g})+2 \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{CH}_{3} \mathrm{OH}(\mathrm{g})
$$
Hydrogen is introduced until the total pressure of the system is $8.5$ atmosphere at equilibrium and $0.08$ mole of methanol is formed. Calculate (i) $K_{p}$ and $K_{c}$ and (ii) the final pressure if the same amount of $\mathrm{CO}$ and $\mathrm{H}_{2}$ as before are used, but with no catalyst so that the reaction does not take place.

Shubham Kumar
Shubham Kumar
Numerade Educator
07:33

Problem 65

The solubility product $\left(K_{s p}\right)$ of $\mathrm{Ca}(\mathrm{OH})_{2}$ at $25^{\circ} \mathrm{C}$ is $4.42 \times 10^{-5}$. A 500 $\mathrm{mL}$. of saturated solution of $\mathrm{Ca}(\mathrm{OH})_{2}$ is mixed with equal volume of $0.4 \mathrm{M} \mathrm{NaOH}$. How much $\mathrm{Ca}(\mathrm{OH})_{2}$ in milligrams is precipitated?

Susan Hallstrom
Susan Hallstrom
Numerade Educator
02:12

Problem 66

The solubility product of $\mathrm{Ag}_{2} \mathrm{C}_{2} \mathrm{O}_{4}$ at $25^{\circ} \mathrm{C}$ is $1.29 \times 10^{-11} \mathrm{~mol}^{3} \mathrm{~L}^{-3}$. A
solution of $\mathrm{K}_{2} \mathrm{C}_{2} \mathrm{O}_{4}$ containing $0.1520$ mole in $500 \mathrm{~mL}$ water is shaken at $25^{\circ} \mathrm{C}$ with excess of $\mathrm{Ag}_{2} \mathrm{CO}_{3}$ till the following equilibrium is reached:
$$\mathrm{Ag}_{2} \mathrm{CO}_{3}+\mathrm{K}_{2} \mathrm{C}_{2} \mathrm{O}_{4} \rightleftharpoons \mathrm{Ag}_{2} \mathrm{C}_{2} \mathrm{O}_{4}+\mathrm{K}_{2} \mathrm{CO}_{3}$$
At equilibrium, the solution contains $0.0358$ mole of $\mathrm{K}_{2} \mathrm{CO}_{3}$. Assuming the degree of dissociation of $\mathrm{K}_{2} \mathrm{C}_{2} \mathrm{O}_{4}$ and $\mathrm{K}_{2} \mathrm{CO}_{3}$ to be equal, calculate the solubility product of $\mathrm{Ag}_{2} \mathrm{CO}_{3}$

Anand Jangid
Anand Jangid
Numerade Educator
03:37

Problem 67

For the reaction : $\mathrm{CO}(\mathrm{g})+2 \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{CH}_{3} \mathrm{OH}(\mathrm{g})$
hydrogen gas is introduced into a five litre flask at $327^{\circ} \mathrm{C}$, containing $0.2$ mole of $\mathrm{CO}(\mathrm{g})$ and a catalyst, until the pressure is $4.92 \mathrm{~atm}$. At this point $0.1$ mole of $\mathrm{CH}_{3} \mathrm{OH}(\mathrm{g})$ is formed. Calculate the equilibrium constant, $K_{p}$ and $K_{c}$.

Bailey Mccarthy Riley
Bailey Mccarthy Riley
Numerade Educator
02:15

Problem 68

Freshly precipitated aluminium and magnesium hydroxides are stirred vigorously in a buffer solution containing $0.25$ mole/L of ammonium chloride and $0.05$ mole/ $\mathrm{L}$ of ammonium hydroxide.
Calculate the concentration of aluminium and magnesium ions in solution:
$K_{b}\left[\mathrm{NH}_{4} \mathrm{OH}\right]=1.80 \times 10^{-5}$
$K_{s p}\left[\mathrm{Mg}(\mathrm{OH})_{2}\right]=6 \times 10^{-10}$
$K_{s n}\left[\mathrm{Al}(\mathrm{OH})_{3}\right]=6 \times 10^{-32}$

Lottie Adams
Lottie Adams
Numerade Educator
02:47

Problem 69

The equilibrium constant $K_{p}$ of the reaction:
$$
2 \mathrm{SO}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{SO}_{3}(\mathrm{~g})
$$
is 900 atm. at $800 \mathrm{~K}$. A mixture containing $\mathrm{SO}_{3}$ and $\mathrm{O}_{2}$ having initial partial pressure of 1 and 2 atm. respectively is heated at constant volume to equilibrate. Calculate the partial pressure of each gas at $800 \mathrm{~K}$.

Shubham Kumar
Shubham Kumar
Numerade Educator
10:07

Problem 70

$\mathrm{N}_{2} \mathrm{O}_{4}$ is $25 \%$ dissociated at $37^{\circ} \mathrm{C}$ and one atmosphere pressure. Calculate (i) $K_{o}$ and (ii) the percentage dissociation at $0.1$ atmosphere and

Prashant Bana
Prashant Bana
Numerade Educator
01:30

Problem 71

At a certain temperature equilibrium constant $(K)$ is 16 for the reaction.
$$
\begin{gathered}
{[1987-5 \text { Marks }]} \\
\mathrm{SO}_{2}(\mathrm{~g})+\mathrm{NO}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{SO}_{3}(\mathrm{~g})+\mathrm{NO}(\mathrm{g})
\end{gathered}
$$
If we take one mole each of all the four gases in a one litre container, what would be the equilibrium concentrations of $\mathrm{NO}(\mathrm{g})$ and $\mathrm{NO}_{2}(\mathrm{~g})$ ?

Narayan Hari
Narayan Hari
Numerade Educator
02:44

Problem 72

The solubility of $\mathrm{Mg}(\mathrm{OH})_{2}$ in pure water is $9.57 \times 10^{-3} \mathrm{~g} /$ litre. Calculate its solubility (in $\mathrm{g}$ /litre) in $0.02 \mathrm{M} \mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}$ solution.

Himanshu Kushwaha
Himanshu Kushwaha
Numerade Educator
02:18

Problem 73

One mole of $\mathrm{Cl}_{2}$ and 3 moles of $\mathrm{PCl}_{5}$ are placed in a 100 litre vessel heated to $227^{\circ} \mathrm{C}$. The equilibrium pressure is $2.05$ atmosphere. Assuming ideal behaviour, calculate the degree of dissociation for $\mathrm{PCl}_{5}$ and $K_{p}$ for the reaction:
$\mathrm{PCl}_{5}(\mathrm{~g}) \rightleftharpoons \mathrm{PCl}_{3}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g})$

ra
Rajbala Aggarwal
Numerade Educator
03:30

Problem 74

A solution contains a mixture of $\mathrm{Ag}(0.10 \mathrm{M})$ and $\mathrm{Hg}_{2}^{++}(0.10 \mathrm{M})$ which are to be separated by selective precipitation. Calculate the maximum concentration of iodide ion at which one of them gets precipitated almost completely. What percentage of that metal ion is precipitated? $\left[K_{s p}: \mathrm{AgI}=8.5 \times 10^{-17} ; \mathrm{Hg}_{2} \mathrm{I}_{2}=2.5 \times 10^{-26}\right]$

Lottie Adams
Lottie Adams
Numerade Educator
01:05

Problem 75

One mole of nitrogen is mixed with three moles of hydrogen in a 4 litre container. If $0.25$ per cent of nitrogen is converted to ammonia by the following reaction
$$
\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_{3}(\mathrm{~g})
$$
calculate the equilibrium constant $\left(K_{c}\right)$ in concentration units. What will be the value of $K_{c}$ for the following equilibrium?
$$
\frac{1}{2} \mathrm{~N}_{2}(\mathrm{~g})+\frac{3}{2} \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{NH}_{3}(\mathrm{ag})
$$

Ronald Prasad
Ronald Prasad
Numerade Educator