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Objective Chemistry for NEET Vol II

Pearson Education

Chapter 4

Chemical Kinetics - all with Video Answers

Educators

Chapter Questions

00:49

Problem 1

The unit of specific reaction rate constant for a firstorder (if the concentration is expressed in molarity) would be:
(a) $\mathrm{s}^{-1}$
(b) mole $\mathrm{s}^{-1}$
(c) mole $\mathrm{L}^{-1} \mathrm{~s}^{-1}$
(d) mole $\mathrm{L}^{-1}$

Alkendra Singh
Alkendra Singh
Numerade Educator
01:07

Problem 2

The temperature coefficient of most of the reactions lies between:
(a) 1 and 3
(b) 2 and 3
(c) 1 and 2
(d) 2 and 4

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:11

Problem 3

The activation energy for a simple chemical reaction $\mathrm{A} \longrightarrow \mathrm{B}$ is $\mathrm{E}$ in forward direction. The activation energy for reverse reaction:
(a) Can be less than or more than $\mathrm{E}_{\mathrm{a}}$
(b) Is always double of $E_{a}$
(c) Is negative of $\mathrm{E}_{\mathrm{a}}$
(d) Is always less than $\mathrm{E}_{\mathrm{a}}$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:09

Problem 4

For a reaction $\mathrm{A}+2 \mathrm{~B} \longrightarrow \mathrm{C}$, rate is given by $+\mathrm{d}[\mathrm{C}] / \mathrm{dt}=k[\mathrm{~A}][\mathrm{B}]$, hence the order of the reaction is:
(a) 3
(b) 2
(c) 1
(d) 0

Hunza Gilgit
Hunza Gilgit
Numerade Educator
00:48

Problem 5

The rate of reaction depends upon:
(a) Molar concentration
(b) Atomic mass
(c) Equivalent mass
(d) None of these

Alkendra Singh
Alkendra Singh
Numerade Educator
00:54

Problem 6

For a first-order reaction, the half-life period is independent of:
(a) Initial concentration
(b) Cube root of initial concentration
(c) First power of final concentration
(d) Square root of final concentration

Alkendra Singh
Alkendra Singh
Numerade Educator
00:19

Problem 7

Which of these graphs best describes the rate at which $\mathrm{N}_{2} \mathrm{O}_{4}$ decomposes to $\mathrm{NO}_{2}$ if the reaction is of firstorder?
(a)
(b)
(c)
(d)

Mishal Gul
Mishal Gul
Numerade Educator
01:21

Problem 8

Activation energy of a chemical reaction can be determined by:
(a) Evaluating rate constant at standard temperature.
(b) Evaluating velocities of reaction at two different temperatures.
(c) Evaluating rate constants at two different temperatures.
(d) Changing concentration of reactants.

Ramesh Singh
Ramesh Singh
Numerade Educator
01:30

Problem 9

The first-order rate constant for the decomposition of $\mathrm{N}_{2} \mathrm{O}_{5}$ is $6.2 \times 10^{-4} \mathrm{~s}^{-1} .$ The half-life for this decomposition is:
(a) $1177.7 \mathrm{~s}$
(b) $1117.7 \mathrm{~s}$
(c) $6.077 \mathrm{~s}$
(d) $110.77 \mathrm{~s}$

Alkendra Singh
Alkendra Singh
Numerade Educator
00:52

Problem 10

The given reaction, $2 \mathrm{FeCl}_{3}+\mathrm{SnCl}_{2} \longrightarrow 2 \mathrm{FeCl}_{2}+\mathrm{SnCl}_{4}$
is an example of:
(a) First-order reaction
(b) Second-order reaction
(c) Third-order reaction
(d) None of these

Alkendra Singh
Alkendra Singh
Numerade Educator
01:07

Problem 11

If the rate of the reaction is equal to the rate constant, the order of the reaction is:
(a) 3
(b) 0
(c) 1
(d) 2

Alkendra Singh
Alkendra Singh
Numerade Educator
01:10

Problem 12

Which of the following best explains the effects of a catalyst on the rate of a reversible reaction?
(a) It decreases the rate of the reverse reaction
(b) It increases the kinetic energy of the reacting mol ecules
(c) It moves the equilibrium position to the right
(d) It provides a new reaction path with a lower activation energy

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:07

Problem 13

Units of rate constant for the first and zero-order reactions in terms of molarity $\mathrm{M}$, units are respectively:
(a) $\mathrm{s}^{-1}, \mathrm{Ms}^{-1}$
(b) $\mathrm{s}^{-1}, \mathrm{M}$
(c) $\mathrm{M} s^{-1}, \mathrm{~s}^{-1}$
(d) $\mathrm{M}, \mathrm{s}^{-1}$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:03

Problem 14

For a chemical reaction $\mathrm{A} \longrightarrow \mathrm{B}$, the rate of reaction doubles when the concentration of $\mathrm{A}$ is increased four times. The order of reaction for $\mathrm{A}$ is:
(a) Zero
(b) One
(c) Two
(d) Half

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:20

Problem 15

The unit of second-order reaction rate constant is:
(a) $\mathrm{L}^{-1} \cdot \mathrm{mol}^{-1} \mathrm{~d} \mathrm{~s}^{-1}$
(b) $\mathrm{L}^{2} \mathrm{~mol}^{-2} \mathrm{~s}^{-1}$
(c) L. $\mathrm{mol}^{-1} \mathrm{~s}^{-1}$
(d) $\mathrm{s}^{-1}$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
02:18

Problem 16

What is the time required for a first-order reaction to be $99 \%$ complete, compared to the time taken for the reaction to be $90 \%$ complete?
(a) There is no change
(b) Time taken is double
(c) Time taken is triple
(d) The reaction is instantaneous

Mahendra Kumar
Mahendra Kumar
Numerade Educator
01:26

Problem 17

The accompanying figure depicts the change in con centrations of species $\mathrm{X}$ and $\mathrm{Y}$ for the reaction $\mathrm{X} \longrightarrow \mathrm{Y}$, as a function of time. The point of intersection of the two curves represents:(a) $\mathrm{t}_{1 / 2}$
(b) $\mathrm{t}_{3 / 4}$
(c) $\mathrm{t}_{1 / 2}$
(d) Unpredictable

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:14

Problem 18

Among the following factors, the specific reaction rate of a first-order reaction depends on:
(a) Temperature
(b) Concentration of reactant
(c) Pressure
(d) Volume

Hunza Gilgit
Hunza Gilgit
Numerade Educator
04:51

Problem 19

The molecularity of a reaction is:
(a) Always two
(b) Same as its order
(c) Different than the other
(d) May be same or different as compared to order

Himanshu Kushwaha
Himanshu Kushwaha
Numerade Educator
04:00

Problem 20

For the reaction, $\mathrm{A}+\mathrm{B} \longrightarrow \mathrm{C}+\mathrm{D}$. The variation of the concentration of the products is given by the curve:
(a) $\mathrm{w}$
(b) $x$
(c) $\mathrm{y}$
(d) $z$

Himanshu Kushwaha
Himanshu Kushwaha
Numerade Educator
03:53

Problem 21

Which of the following is incorrect about order of reaction?
(a) It is calculated experimentally
(b) It is sum of powers of concentration in rate law expression
(c) The order of reaction cannot be fractional
(d) There is not necessarily a connection between order and stoichiometry of a reaction.

Himanshu Kushwaha
Himanshu Kushwaha
Numerade Educator
03:31

Problem 22

Which curve corresponds to the temperature dependence of the rate $\mathrm{R}$ of a simple one-step reaction?

Himanshu Kushwaha
Himanshu Kushwaha
Numerade Educator
01:10

Problem 23

If $\mathrm{T}$ is the intensity of absorbed light and ' $\mathrm{C}$ is the concentration of $\mathrm{AB}$ for the photochemical process $\mathrm{AB}+\mathrm{hv} \longrightarrow \mathrm{AB}^{*}$, the rate of formation of $\mathrm{AB}^{\prime}$ is
directly proportional to:
(a) $\mathrm{C}$
(b) I
(c) $\mathrm{I}^{2}$
(d) C.I

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:14

Problem 24

For a first-order reaction,
(a) The degree of dissociation is equal to $\left(1-\mathrm{e}^{-\mathrm{kt}}\right)$
(b) The pre-exponential factor in the Arrhenius equation has the dimensions of time $\mathrm{t}^{-1}$.
(c) The time taken for the completion of $75 \%$ reation is thrice the t $1 / 2$ of the reaction.
(d) Both (a) and (b)

Hunza Gilgit
Hunza Gilgit
Numerade Educator
02:58

Problem 25

The rate law for the reaction:
$\mathrm{RCl}+\mathrm{NaOH}(\mathrm{aq}) \longrightarrow \mathrm{ROH}+\mathrm{NaCl}$
is given by Rate $=k[\mathrm{RCl}]$. The rate of the reaction will be
(a) Doubled on doubling the concentration of sodium hydroxide.
(b) Halved on reducing the concentration of alkyl halide to one half.
(c) Decreased on increasing the temperature of reaction.
(d) Unaffected by increasing the temperature of the reaction.

Himanshu Kushwaha
Himanshu Kushwaha
Numerade Educator
01:14

Problem 26

The equation for the rate constant is $k=\mathrm{Ae}^{-\mathrm{E}_{2} / \mathrm{RT}} . \mathrm{A}$ chemical reaction will proceed more rapidly if there is a decrease in:
(a) $k$
(b) A
(c) $\mathrm{E}$
(d) $\mathrm{T}$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:12

Problem 27

The rate law has the form; rate $=k[\mathrm{~A}][\mathrm{B}]^{3 / 2}$, can the reaction be an elementary process?
(a) Yes
(b) No
(c) May be yes or no
(d) Cannot be predicted

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:17

Problem 28

For a second-order reaction, $2 \mathrm{~A} \longrightarrow$ Product, a straight line is obtained if we plot:
(a) Concentration vs time
(b) Log (conc.) vs time
(c) Log (conc.) vs time $^{1}$
(d) (Conc.) vs time $^{1}$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:01

Problem 29

For an endothermic reaction, where $\Delta \mathrm{H}$ represents the enthalpy of the reaction in $\mathrm{kJ} /$ mole, the minimum value for the energy of activation will be:
(a) Less than $\Delta \mathrm{H}$
(b) Zero
(c) More than $\Delta \mathrm{H}$
(d) Equal to $\Delta \mathrm{H}$

Narayan Hari
Narayan Hari
Numerade Educator
01:18

Problem 30

The rate constant $k$, of a second-order reaction, $\mathrm{A} \longrightarrow$ Products, is given by $\mathrm{k}=1 / \mathrm{t}\{\mathrm{x} / \mathrm{a}(\mathrm{a}-\mathrm{x})\}$ the
ratio $\mathrm{t}_{3 / 4} \mathrm{t}_{1 / 2}$ is equal to:

Hunza Gilgit
Hunza Gilgit
Numerade Educator
02:41

Problem 31

The rate constant of a reaction depends on:
(a) Extent of reaction
(b) Time of reaction
(c) Temperature
(d) Initial concentration of the reactants

Himanshu Kushwaha
Himanshu Kushwaha
Numerade Educator
03:04

Problem 32

The function of catalyst in chemical reaction is to:
(a) Increase the product
(b) Decrease the product
(c) Accelerate the rate of reaction
(d) Increase the reactants

Himanshu Kushwaha
Himanshu Kushwaha
Numerade Educator
01:11

Problem 33

For a particular gaseous reaction, a graph was plotted as shown below. It shows that the reaction of $\mathrm{A}$ is:
(a) Zero-order w.r.t. A
(b) First-order w.r.t. A
(c) Second-order w.r.t. A
(d) A non-integer order w.r.t. A

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:10

Problem 34

According to the collision theory of reaction rates, an increase of the temperature at which the reaction occurs will inturn increase the rate of the reaction. This is caused due to:
(a) Greater number of molecules are having the activation energy (threshold energy)
(b) Greater velocity of reaction molecules
(c) Greater number of collisions
(d) None of these

Hunza Gilgit
Hunza Gilgit
Numerade Educator
03:30

Problem 35

For a chemical reaction, which can never be a fractional number?
(a) Order
(b) Half-life
(c) Molecularity
(d) Rate constant

Himanshu Kushwaha
Himanshu Kushwaha
Numerade Educator
01:22

Problem 36

Which of the following is correct for a first order reaction? ( $k=$ rate constant $t_{1 / 2}=$ half-life :
(a) $\mathrm{t}_{1 / 2}=0.693 \times \mathrm{k}$
(b) $k \cdot t_{1 / 2}=1 / 0.693$
(c) $\mathrm{k.t}_{1 / 2}=0.693$
(d) $6.93 \times k \times t_{1 / 2}=1$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
02:57

Problem 37

Which of the following relation is correct for a first order reaction? $(k=$ rate constant; $\mathrm{r}=$ rate of reaction; $\mathrm{C}=$ conc. of reactant)
(a) $k=\mathrm{r} \times \mathrm{C}^{2}$
(b) $k=\mathrm{r} \mathrm{x}$
(c) $k=\mathrm{C} / r$
(d) $k=\mathrm{r} / \mathrm{C}$

Himanshu Kushwaha
Himanshu Kushwaha
Numerade Educator
01:08

Problem 38

If the rate law of a reaction $\mathrm{nA} \longrightarrow \mathrm{B}$ is expressed as:
Rate $=-\frac{1}{\mathrm{n}} \frac{\mathrm{d}[\mathrm{A}]}{\mathrm{dt}}=+\frac{\mathrm{d}[\mathrm{B}]}{\mathrm{dt}}=k[\mathrm{~A}]^{\mathrm{x}}$
The unit of the rate constant will be
(a) $\mathrm{mol}^{\mathrm{x}} / \mathrm{L}^{\mathrm{x}} / \mathrm{s}$
(b) $\mathrm{L}^{\mathrm{x}} / \mathrm{mol}^{\mathrm{x}} \mathrm{s}$
(c) $\mathrm{mol}^{(1-\mathrm{x})} / \mathrm{L}^{(\mathrm{x}-1)} \cdot \mathrm{S}^{-1}$
(d) $\mathrm{mol}^{(\mathrm{x}-\mathrm{l})} / \mathrm{L}^{(1-\mathrm{x})} \cdot \mathrm{S}^{-1}$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:10

Problem 39

For an endothermic reaction:
(a) $\mathrm{E}_{\mathrm{a}}>\mathrm{E}^{\prime}$
(b) $\mathrm{E}_{\mathrm{a}}=\mathrm{E}^{\prime \mathrm{a}}$
(c) There is no relation between $\mathrm{E}_{\mathrm{a}}$ and $\mathrm{E}_{\text {a }}^{\prime}$
(d) $\mathrm{E}_{\mathrm{a}}<\mathrm{E}^{\prime}$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
04:04

Problem 40

Rate constant of a reaction $(k)$ is $175 \mathrm{~L}^{2} \mathrm{~mol}^{-2} \mathrm{sec}^{-1}$. What is the order of reaction?
(a) First
(b) Second
(c) Third
(d) Zero

Himanshu Kushwaha
Himanshu Kushwaha
Numerade Educator
03:33

Problem 41

A catalyst is a substance which:
(a) Supplies energy to the reaction
(b) Increases the equilibrium concentration of the product
(c) Changes the equilibrium constant of the reaction
(d) Shortens the time to each equilibrium

Himanshu Kushwaha
Himanshu Kushwaha
Numerade Educator
03:20

Problem 42

The rate of reaction was found to be equal to its rate constant at any concentration of the reactant. The order of the reaction is:
(a) Zero-order
(b) First-order
(c) Second-order
(d) Third-order

Himanshu Kushwaha
Himanshu Kushwaha
Numerade Educator
01:33

Problem 43

For the reaction:
$\mathrm{H}_{2}+\mathrm{Cl}_{2} \stackrel{\text { sunlight }}{\longrightarrow} 2 \mathrm{HCl}$
taking place on water, the order of reaction is:
(a) 0
(b) 1
(c) 2
(d) 3

Himanshu Kushwaha
Himanshu Kushwaha
Numerade Educator
01:16

Problem 44

$\mathrm{T}_{\mathrm{av}}$ (average life), $\mathrm{T}_{50}$ and $\mathrm{T}_{75}$ in the increasing order are:
(a) $\mathrm{T}_{50}<\mathrm{T}_{\mathrm{av}}<\mathrm{T}_{75}$
(b) $\mathrm{T}_{50}<\mathrm{T}_{75}<\mathrm{T}_{\mathrm{av}}$
(c) $\mathrm{T}_{\mathrm{gv}}=\mathrm{T}_{50}<\mathrm{T}_{75}$
(d) $\mathrm{T}_{\mathrm{av}}=\mathrm{T}_{50}<\mathrm{T}_{75}$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
03:16

Problem 45

A catalyst increases rate of reaction by:
(a) Decreasing enthalpy
(b) Decreasing activation energy
(c) Decreasing internal energy
(d) Increasing activation energy

Himanshu Kushwaha
Himanshu Kushwaha
Numerade Educator
00:18

Problem 46

For an exothermic chemical process occurring in two steps as:
(1) $\mathrm{A}+\mathrm{B} \longrightarrow \mathrm{X}(\mathrm{slow})$
(2) $\mathrm{X} \longrightarrow \mathrm{AB}$ (fast)
The progress of the reaction can be best described by:

Mishal Gul
Mishal Gul
Numerade Educator
01:16

Problem 47

The rate constant is given by the equation $=\mathrm{P} \mathrm{Ze}^{\mathrm{E} / \mathrm{RT}}$. Which factor should register a decrease for the reaction to proceed more rapidly?
(a) $\mathrm{T}$
(b) $\mathrm{Z}$
(c) $\mathrm{E}$
(d) $\mathrm{P}$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:21

Problem 48

For the reaction $\mathrm{H}_{2}+\mathrm{Br}_{2} \rightleftharpoons 2 \mathrm{HBr}$
The reaction rate $=\mathrm{k}\left[\mathrm{H}_{2}\right]^{1}\left[\mathrm{Br}_{2}\right]^{3 / 2}$ which is correct about it?
(a) Molecularity $=2$
(b) Order $=2$
(c) Order $=3 / 2$
(d) Both (a) and (c)

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:18

Problem 49

$2 \mathrm{O}_{3} \rightleftharpoons 3 \mathrm{O}_{2} .$ The mechanism is $\mathrm{O}_{3} \rightleftharpoons \mathrm{O}_{2}+\mathrm{O}$
$\mathrm{O}_{3}+\mathrm{O} \rightleftharpoons 2 \mathrm{O}_{2}$. The rate law is:
(a) $\mathrm{r}=k\left[\mathrm{O}_{3}\right]^{2}\left[\mathrm{O}_{2}\right]^{-1}$
(b) $\mathrm{r}=k\left[\mathrm{O}_{3}\right]^{2}\left[\mathrm{O}_{2}\right]$
(c) $\mathrm{r}=k\left[\mathrm{O}_{3}\right]\left[\mathrm{O}_{2}\right]$
(d) $\mathrm{r}=k\left[\mathrm{O}_{3}\right]^{2}$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:16

Problem 50

Which of the following statement is correct?
(a) A plot of $\log k_{\mathrm{p}}$ vs $1 / \mathrm{t}$ is linear
(b) A plot of $\log [\mathrm{X}]$ vs time is linear for a first-order reaction, $\mathrm{X} \longrightarrow \mathrm{P}$
(c) A plot of log $\mathrm{P}$ vs $1 / \mathrm{t}$ is linear at constant volume
(d) A plot of $\mathrm{P}$ vs $1 / \mathrm{V}$ is linear at constant pressure

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:14

Problem 51

For a zero-order reaction, the plot of concentration vs time is linear with:
(a) +ve slope and zero intercept
(b) - ve slope and zero intercept
(c) +ve slope and non-zero intercept
(d) - ve slope and non-zero intercept

Hunza Gilgit
Hunza Gilgit
Numerade Educator
00:09

Problem 52

Which curve represents zero-order reaction?

Mishal Gul
Mishal Gul
Numerade Educator
00:38

Problem 53

Consider the following two reactions:
$\mathrm{A} \longrightarrow$ Product $-\mathrm{d}[\mathrm{A}] / \mathrm{dt}=k_{1}[\mathrm{~A}]^{0}$
$\mathrm{B} \longrightarrow$ Product $-\mathrm{d}[\mathrm{B}] / \mathrm{dt}=\mathrm{k}_{2}[\mathrm{~B}]$
$k_{1}$, and $k_{2}$ are expressed in terms of molarity $\left(\mathrm{mol} \mathrm{L}^{-1}\right)$ and time $\left(\mathrm{s}^{-1}\right)$ as
(a) $\mathrm{s}^{-1}, \mathrm{M} \mathrm{s}^{-1} \mathrm{~L}^{-1}$
(b) $\mathrm{Ms}^{-1}, \mathrm{M} \mathrm{s}^{-1}$
(c) $\mathrm{s}^{-1} \mathrm{M}^{-1} \mathrm{~s}^{-1}$
(d) $\mathrm{M} \mathrm{s}^{-1}, \mathrm{~L}^{-1} \mathrm{~s}^{-1}$

Mishal Gul
Mishal Gul
Numerade Educator
01:26

Problem 54

A reaction rate is given by, $k=1.5 \times 10^{15} \exp (-25000 / \mathrm{RT}) \mathrm{s}^{-1}$
it means that:
(a) Half-life period of the reaction will be smaller at high temperature
(b) Log vs T will give a straight
(c) Half-life of the reaction will be smaller at lower temperature
(d) Log vs $1 / \mathrm{T}$ will give a straight line having a slope of $-25000$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:17

Problem 55

With respect to the figure given below which of the following statement is correct?(a) $\Delta \mathrm{E}$ for the forward reaction is $\mathrm{C}-\mathrm{B}$
(b) $\Delta \mathrm{E}$ for the forward reaction is $\mathrm{B}-\mathrm{A}$
(c) $\mathrm{E}$ (for reverse reaction) $=\mathrm{C}-\mathrm{A}$
(d) $\mathrm{E}_{\text {(Forward) }}>\mathrm{E}_{\text {(Backuad) }}$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
00:29

Problem 56

A substance undergoes first-order decomposition, it follows two parallel reactions:
$k_{1}=1.26 \times 10^{-4} \mathrm{~s}^{-1}$
and $k_{2}=3.8 \times 10^{-5} \mathrm{~s}^{-1}$
The percentage distribution of $\mathrm{Y}$ and $\mathrm{Z}$ are
(a) $80 \% \mathrm{Y}$ and $20 \% \mathrm{Z}$
(b) $72.83 \% \mathrm{Y}$ and $32.71 \% \mathrm{Z}$
(c) $76.83 \% \mathrm{Y}$ and $23.17 \% \mathrm{Z}$
(d) $62.4 \% \mathrm{Y}$ and $90.5 \% \mathrm{Z}$

Mishal Gul
Mishal Gul
Numerade Educator
00:26

Problem 57

A substance undergoes first-order decomposition, it follows two parallel reactions:
$k_{1}=1.26 \times 10^{-4} \mathrm{~s}^{-1}$
and $k_{2}=3.8 \times 10^{-5} \mathrm{~s}^{-1}$
The percentage distribution of $\mathrm{Y}$ and $\mathrm{Z}$ are
(a) $80 \% \mathrm{Y}$ and $20 \% \mathrm{Z}$
(b) $72.83 \% \mathrm{Y}$ and $32.71 \% \mathrm{Z}$
(c) $76.83 \% \mathrm{Y}$ and $23.17 \% \mathrm{Z}$
(d) $62.4 \% \mathrm{Y}$ and $90.5 \% \mathrm{Z}$

Mishal Gul
Mishal Gul
Numerade Educator
01:16

Problem 58

$k$ for a zero-order reaction is $2 \times 10^{-2} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1} .$ If the concentration of the reactant after $25 \mathrm{~s}$ is $0.5 \mathrm{M}$, the initial concentration must have been:
(a) $0.5 \mathrm{M}$
(b) $1.25 \mathrm{M}$
(c) $12.5 \mathrm{M}$
(d) $1.0 \mathrm{M}$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
03:06

Problem 59

$75 \%$ of a first-order reaction was completed in $32 \mathrm{~min}$. When was $50 \%$ of the reaction completed?
(a) $24 \mathrm{~min}$
(b) $16 \mathrm{~min}$
(c) $8 \mathrm{~min}$
(d) $64 \mathrm{~min}$

Himanshu Kushwaha
Himanshu Kushwaha
Numerade Educator
01:17

Problem 60

For a first-order reaction, $t_{0.75}$ is $138.6$ seconds. Its specific reaction rate constant (in $\mathrm{sec} .^{-1}$ ) is:
(a) $10^{-2}$
(b) $10^{-4}$
(c) $10^{-5}$
(d) $10^{-6}$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:09

Problem 61

Rate constant of the first-order reaction when initial concentration $C_{0}$ and concentration $C_{t}$ at time $t$ is given by equation:
$k_{t}=\log C_{0}-\log C_{t}$
Graph is a straight line if we plot
(a) $\mathrm{t} \operatorname{vs} \log \mathrm{C}_{\mathrm{o}}$
(b) $\mathrm{t} \mathrm{vs} \log \mathrm{C}_{\mathrm{t}}$
(c) $\mathrm{t}^{-1} \operatorname{vs} \log \mathrm{C}_{\mathrm{t}}$
(d) $\log C_{o} \operatorname{vs} \log C_{t}$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:08

Problem 62

For the first-order reaction half-life is $14 \mathrm{~s}$. The time required for the initial concentration to reduce to $1 / 8$ th of its value is:
(a) $21 \mathrm{~s}$
(b) $32 \mathrm{~s}$
(c) $42 \mathrm{~s}$
(d) $142 \mathrm{~s}$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:07

Problem 63

The potential energy diagram for a reaction $\mathrm{R} \longrightarrow \mathrm{P}$ is given below:
$\Delta \mathrm{H}^{\circ}$ of the reaction corresponds to the energy
(a) $\mathrm{x}$
(b) y
(c) $\mathrm{z}$
(d) $(\mathrm{x}+\mathrm{y})$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:10

Problem 64

For the reaction:
$$
2 \mathrm{~N}_{2} \mathrm{O}_{5}(\mathrm{~g}) \longrightarrow 4 \mathrm{NO}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g})
$$
which of the following graph will yield a straight line?
(a) $\log \mathrm{P}_{\mathrm{N}_{2} \mathrm{O}_{5}}$ vs time with a +ve slope
(b) $\log \mathrm{P}_{\mathrm{N}_{2} \mathrm{O}_{5}}$ vs time with a -ve slope
(c) $\left(\mathrm{PN}_{2} \mathrm{o}_{5}\right)^{-1}$ vs time
(d) $\log \mathrm{P}_{\mathrm{N} \gamma}$. vs time

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:19

Problem 65

The temperature dependence of rate constant (A) of a chemical reaction is written in terms of Arrhenius equation, $=\mathrm{A} \cdot \mathrm{e}^{-\mathrm{E} / \mathrm{RT}}$, Activation energy $\mathrm{E}_{3}$ of the reaction can be calculated by ploting:
(a) $\log \mathrm{k} \operatorname{vs} \mathrm{T}^{-1}$
(b) $\log \mathrm{k} \mathrm{vs} \frac{1}{\log \mathrm{T}}$
(c) $k \operatorname{vs} \mathrm{T}$
(d) $\mathrm{k} \mathrm{vs} \frac{1}{\log \mathrm{T}}$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:23

Problem 66

The half-life of a substance in a first-order reaction is 15 minutes. The rate constant is:
(a) $2.46 \times 10^{2} \mathrm{~min}^{-1}$
(b) $4.62 \times 10^{-2} \mathrm{~min}^{-1}$
(c) $3 \times 10^{-5} \mathrm{~min}^{-1}$
(d) $3 \times 10^{-9} \mathrm{~min}^{-1}$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
03:59

Problem 67

In a second-order reaction, if first-order is observed for both the reactants $\mathrm{A}$ and $\mathrm{B}$, then which one of the following reactant mixtures will provide the highest initial rate?
(a) $0.1$ mol of $A$ and $0.1$ mol of in $0.2$ litre solvent
(b) $1.0 \mathrm{~mol}$ of $\mathrm{A}$ and $1.0 \mathrm{~mol}$ of in one litre solvent
(c) $0.2$ mol of $A$ and $0.2$ mol of in $0.1$ litre solvent
(d) $0.1$ mol of $\mathrm{A}$ and $0.1$ mol of in $0.1$ litre solvent

Himanshu Kushwaha
Himanshu Kushwaha
Numerade Educator
01:13

Problem 68

The activation energy of a reaction is $9 \mathrm{kcal} /$ mole. The increase in the rate constant when its temperature is raised from 295 to 300 is:
(a) $14.9 \%$
(b) $28.9 \%$
(c) $78.9 \%$
(d) $82.9 \%$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
02:39

Problem 69

The rate constant of first-order reaction is $3 \times 10^{-6}$ per second. The initial concentration is $0.10 \mathrm{M}$. The initial rate is:
(a) $3 \times 10^{-7} \mathrm{Ms}^{-1}$
(b) $3 \times 10^{-4} \mathrm{Ms}^{-1}$
(c) $3 \times 10^{-5} \mathrm{Ms}^{-1}$
(d) $3 \times 10^{-6} \mathrm{Ms}^{-1}$

Himanshu Kushwaha
Himanshu Kushwaha
Numerade Educator
00:32

Problem 70

Consider the following statements:
(1) Rate of a process is directly proportional to its free energy change
(2) The order of an elementary reaction step can be determined by examining the stoichiometry
(3) The first-order reaction describe exponential time course. Of the statements:
(a) 1 and 2 are correct
(b) 1 and 3 are correct
(c) 2 and 3 are correct
(d) 1,2 and 3 are correct

Mishal Gul
Mishal Gul
Numerade Educator
01:22

Problem 71

In a first-order reaction $\mathrm{A} \longrightarrow \mathrm{P}$, the ratio of $\mathrm{a} /(\mathrm{a}-\mathrm{x})$ was found to be 8 after 60 minutes. If the concentration is $0.1 \mathrm{M}$ then the rate of reaction in moles of A reacted per minutes is:
(a) $2.226 \times 10^{-3}$ mol litre $^{-1} \min ^{-1}$
(b) $3.466 \times 10^{-3}$ mol litre $^{-1} \min ^{-1}$
(c) $4.455 \times 10^{-3}$ mol litre $^{-1} \min ^{-1}$
(d) $5.532 \times 10^{-3}$ mol litre $^{-1} \mathrm{~min}^{-1}$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:09

Problem 72

The rate law for a reaction between the substances $\mathrm{A}$ and is given by Rate $=[\mathrm{A}]^{\mathrm{n}}[\mathrm{B}]^{\mathrm{m}}$ :
On doubling the concentration of $\mathrm{A}$ and halving theconcentration of $\mathrm{B}$, the ratio of the new rate to the earlier rate of the reaction will be as
(a) $1 / 2^{(\mathrm{m}+\mathrm{m})}$
(b) $(\mathrm{m}+\mathrm{n})$
(c) $(\mathrm{n}-\mathrm{m})$
(d) $2^{(n-m)}$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:09

Problem 73

For the reaction,
$$
2 \mathrm{NO}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{~g}) \longrightarrow 2 \mathrm{NO}_{2}(\mathrm{~g})
$$
system volume is suddenly reduced to half its value by increasing the pressure on it. If the reaction is of first order with respect to $\mathrm{O}_{2}$ and second order with respect to $\mathrm{NO}_{2}$, the rate of reaction will:
(a) Diminish to one fourth of its initial value
(b) Diminish to one eighth of its initial value
(c) Increase to eight times of its initial value
(d) Increase to four times of its initial value

Hunza Gilgit
Hunza Gilgit
Numerade Educator
00:57

Problem 74

The energies of activation for forward and reverse reactions for $\mathrm{A}_{2}+\mathrm{B}_{2} \rightleftharpoons 2 \mathrm{AB}$ are $180 \mathrm{~kJ} \mathrm{~mol}^{-1}$
and $200 \mathrm{~kJ} \mathrm{~mol}^{-1}$ respectively. The presence of a catalyst lowers the activation energy of both (forward and reverse) reactions by $100 \mathrm{~kJ} \mathrm{~mol}^{-1}$. The enthalpy change of the reaction $\left(\mathrm{A}_{2}+\mathrm{B}_{2} \longrightarrow 2 \mathrm{AB}\right.$ ) in the presence of catalyst will be (in $\mathrm{kJ} \mathrm{mol}^{-1}$ ):
(a) 120
(b) 280
(c) 20
(d) 300

Mishal Gul
Mishal Gul
Numerade Educator
01:14

Problem 75

Rate of a reaction can be expressed by Arrhenius equation as, $k=\mathrm{Ae}^{-\mathrm{E} / \mathrm{RT}}$ :
In this equation, $\mathrm{E}$ represents
(a) The energy above which all the colliding molecules will react
(b) The energy below which colliding molecules wil not react
(c) The total energy of the reacting molecules at a tem perature, $T$
(d) The fraction of molecules with energy greater than the activation energy of the reaction

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:06

Problem 76

Which of the following are the examples of pseudounimolecular reactions?
(1) Acid catalyzed hydrolysis of an ester
(2) Inversion of cane sugar
(3) Decomposition of ozone
(4) Decomposition of $\mathrm{N}_{2} \mathrm{O}_{5}$ Select the correct answers using the codes given below:
(a) 1 and 2
(b) 1 and 3
(c) 2,3 and 4
(d) 1,2 and 4

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:07

Problem 77

A reaction was found to be second-order with respect to the concentration of carbon monoxide. If the concentration of carbon monoxide is doubled, with eveverything else kept the same, the rate of reaction will
(a) Remain unchanged
(b) Triple
(c) Increase by a factor of 4
(d) Double

Hunza Gilgit
Hunza Gilgit
Numerade Educator
00:34

Problem 78

The following mechanism has been proposed for the reaction of $\mathrm{NO}$ with $\mathrm{Br}_{2}$ to form $\mathrm{NO} \mathrm{Br}$
$$
\begin{aligned}
&\mathrm{NO}(\mathrm{g})+\mathrm{Br}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{NOBr}_{2}(\mathrm{~g}) \\
&\mathrm{NOBr}_{2}(\mathrm{~g})+\mathrm{NO}(\mathrm{g}) \longrightarrow 2 \mathrm{NOBr}(\mathrm{g})
\end{aligned}
$$
If the second step is the rate determining step, the order of the reaction with respect to $\mathrm{NO}(\mathrm{g})$ is:
(a) 1
(b) 0
(c) 3
(d) 2

Mishal Gul
Mishal Gul
Numerade Educator
02:54

Problem 79

A substance reacts according to first-order kinetics. The rate constant for the reaction is $1 \times 10^{-2} \mathrm{sec}^{1} .$ Its initial concentration is IM. Its initial rate is:
(a) $2 \times 10^{2} \mathrm{Ms}^{-1}$
(b) $1 \times 10^{2} \mathrm{Ms}^{-1}$
(c) $1 \times 10^{-2} \mathrm{Ms}^{-1}$
(d) $2 \times 10^{-2} \mathrm{Ms}^{-1}$

Himanshu Kushwaha
Himanshu Kushwaha
Numerade Educator
01:10

Problem 80

What will be the initial rate of a reaction if its constant is $10^{-3} \mathrm{~min}^{-1}$ and the concentration of reactant is $0.2 \mathrm{~mol} \mathrm{dm}^{3} ?$
(a) $0.02 \mathrm{~mol} \mathrm{dm}^{-3} \mathrm{~min}^{-1}$
(b) $0.002 \mathrm{~mol} \mathrm{dm}^{-3} \mathrm{~min}^{-1}$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:01

Problem 81

The rate of a certain hypothetical reaction $\mathrm{A}+\mathrm{B}+\mathrm{C} \longrightarrow$ Products
is given by:
$$
\mathrm{r}=-\frac{\mathrm{d}[\mathrm{A}]}{\mathrm{dt}}=k[\mathrm{~A}]^{1 / 2}[\mathrm{~B}]^{1 / 3}[\mathrm{C}]^{1 / 4}
$$
The order of the reaction is
(a) $13 / 12$
(b) $13 / 14$
(c) $12 / 13$
(d) $13 / 11$

Narayan Hari
Narayan Hari
Numerade Educator
01:14

Problem 82

The decay constant of ${ }_{6} \mathrm{C}^{14}$ is $2.31 \times 10^{-4}$ year $^{-1}$. Its half life is:
(a) $2 \times 10^{3}$ yrs
(b) $2.5 \times 10^{3}$ yrs
(c) $3 \times 10^{3}$ yrs
(d) $3.5 \times 10^{3} \mathrm{yrs}$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:16

Problem 83

A first-order reaction is $50 \%$ completed in 30 minutes at $27^{\circ} \mathrm{C}$. Its rate constant is:
(a) $2.31 \times 10^{-2} \mathrm{~min}^{-1}$
(b) $3.21 \times 10^{-3} \mathrm{~min}^{-1}$
(c) $4.75 \times 10^{-2} \mathrm{~min}^{4}$
(d) $1.33 \times 10^{-3} \mathrm{~min}^{-1}$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:09

Problem 84

The rate constant of a first-order reaction is $6 \times 10^{-3} \mathrm{~s}^{-1}$. If the initial concentration is $0.10 \mathrm{M}$, the initial rate of reaction is:
(a) $6 \times 10^{-3} \mathrm{Ms}^{-1}$
(b) $6 \times 10^{-1} \mathrm{Ms}^{-1}$
(c) $6 \times 10^{-6} \mathrm{Ms}^{-1}$
(d) $6 \times 10^{-8} \mathrm{Ms}^{-1}$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:00

Problem 85

A graph plotted between concentration of reactant, consumed at any time ( $\mathrm{x}$ ) and time ' $\mathrm{t}$ ' is found to be a straight line passing through the origin. The reaction is of:
(a) First-order
(b) Zero-order
(c) Third-order
(d) Second-order

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:02

Problem 86

From the following data for the reaction between $\mathrm{A}$ and $\mathrm{B}$,Calculate the rate equation:
(a) $\mathrm{r}=k[\mathrm{~B}]^{1}$
(b) $\mathrm{r}=k[\mathrm{~A}]^{2}$
(c) $\mathrm{r}=k[\mathrm{~A}]^{2}[\mathrm{~B}]^{1}$
(d) $\mathrm{r}=\mathrm{A}[\mathrm{A}][\mathrm{B}]$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:24

Problem 87

The rate constant, the activation energy and the Arrhenius parameter of a chemical reaction at $25^{\circ} \mathrm{C}$ are $3.0 \times 10^{-4} \mathrm{~s}^{-1}, 104.4 \mathrm{~kJ} \mathrm{~mol}^{-1}$ and $6 \times 10^{14} \mathrm{~s}^{-1}$
respectively:

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:14

Problem 88

The experimental rate law for a reaction:
$2 \mathrm{~A}+3 \mathrm{~B} \longrightarrow$ Product, is $\mathrm{V} \propto \mathrm{C}_{\Lambda} \mathrm{C}_{\mathrm{B}}^{1 / 2} .$ If
the concentration of both $\mathrm{A}$ and are doubled the rate of reaction increases by a factor of
(a) $\sqrt{2}$
(b) 2
(c) $2 . \sqrt{2}$
(d) 4

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:19

Problem 89

In a zero-order reaction, $47.5 \%$ of the reactant remains at the end of $2.5$ hours. The amount of reactant consumed in one hour is:
(a) $11.0 \%$
(b) $33.0 \%$
(c) $42.0 \%$
(d) $21.0 \%$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:15

Problem 90

In a zero-order reaction, $47.5 \%$ of the reactant remains at the end of $2.5$ hours. The amount of reactant consumed in one hour is:
(a) $11.0 \%$
(b) $33.0 \%$
(c) $42.0 \%$
(d) $21.0 \%$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:18

Problem 91

During the decomposition of $\mathrm{H}_{2} \mathrm{O}_{2}$ to give oxygen, $48 \mathrm{~g} \mathrm{O}_{2}$ is formed per minute at a certain point of time. The rate of formation of water at this point is:
(a) $0.75 \mathrm{~mol} \mathrm{~min}^{1}$
(b) $1.5 \mathrm{~mol} \mathrm{~min}^{-1}$
(c) $2.25 \mathrm{~mol} \mathrm{~min}^{-1}$
(d) $3.0 \mathrm{~mol} \mathrm{~min}^{-1}$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:23

Problem 92

The rate constant of a first-order reaction:
$\mathrm{A} \longrightarrow$ products, is $60 \times 10^{-4} \mathrm{~s}^{-1} .$ Its rate at $[\mathrm{A}]=$
$0.01 \mathrm{~mol} \mathrm{~L}^{-1}$ would be
(a) $60 \times 10^{-6} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~min}^{-1}$
(b) $36 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~min}^{-1}$
(c) $60 \times 10^{-2} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~min}^{-1}$
(d) $36 \times 10^{-1} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~min}^{-1}$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
02:04

Problem 93

In a first-order reaction, the concentration of reactant decreases from $800 \mathrm{~mol} / \mathrm{dm}^{3}$ to $50 \mathrm{~mol} / \mathrm{dm}^{3}$ in $2 \times 10^{4}$
sec. The rate constant of reaction in sec. ${ }^{-1}$ is:
(a) $2 \times 10^{4}$
(b) $3.45 \times 10^{-5}$
(c) $1.386 \times 10^{-4}$
(d) $2 \times 10^{-4}$

Deepanshu Kumar
Deepanshu Kumar
Numerade Educator
01:14

Problem 94

The activation energies of two reactions with rate constants $k_{1}$, and $k_{2}$, are $\mathrm{E}_{\mathrm{a}_{1}}$ and $\mathrm{E}_{\mathrm{a} 2}$ respectively. If $\mathrm{E}_{\mathrm{a}_{1}}<\mathrm{E}_{\mathrm{a} 2}$, when the temperature is increased from$\mathrm{T}$, to $\mathrm{T}_{2}$ the rate constants are $k_{1}^{\prime}$ and $k_{2}^{\prime} .$ Which one of the following statements is correct?
(a) $k_{1}=k_{2}^{\prime}$
(b) $\frac{k_{1}}{k_{1}}<\frac{k_{2}}{k_{2}}$
(c) $\frac{k_{1}}{k_{1}}>\frac{k_{2}}{k_{2}}$
(d) $\frac{k_{1}}{k_{1}}=\frac{k_{2}}{k_{2}}$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:05

Problem 95

In a chemical reaction, two reactants take part. The rate of reaction is directly proportional to the concentration of one of them and inversely proportional to the concentration of the other. The order of reaction is:
(a) 0
(b) 1
(c) 2
(d) 4

Hunza Gilgit
Hunza Gilgit
Numerade Educator
00:36

Problem 96

Which of the following statements is correct?
(1) Order of a reaction can be known from experimental results and not from the stoichiometry of a reaction.
(2) Molecularity a reaction refers to (i) each of the elementary steps in (an overall mechanism of) a complex reaction or (ii) a single step reaction.
(3) Overall molecularity of a reaction may be determined in a manner similar to overall order of reaction.
(4) Overall order of a reaction $\mathrm{A}^{\mathrm{m}}+\mathrm{B}^{\mathrm{n}} \longrightarrow \mathrm{AB}_{\mathrm{x}}$ is
$\mathrm{m}+\mathrm{n}$
Select the correct answer using the following codes:
(a) 2 and 3
(b) 1,3 and 4
(c) 2,3 and 4
(d) 1,2 and 3

Mishal Gul
Mishal Gul
Numerade Educator
01:07

Problem 97

The half-life of a chemical reaction at a particular concentration is $50 \mathrm{~min}$, when the concentration of reactants is doubled, the half-life becomes $100 \mathrm{~min}$. Find the order:
(a) Zero
(b) First
(c) Second
(d) Third

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:20

Problem 98

The rate constant of first-order reaction is $10^{-2} \min ^{-1}$. The half-life period of reaction is:
(a) $693 \mathrm{~min}$
(b) $69.3 \mathrm{~min}$
(c) $6.93 \mathrm{~min}$
(d) $0.693 \mathrm{~min}$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:23

Problem 99

When the reactants are and at one mole per litre each the rate equation is, rate $=[\mathrm{A}]^{\mathrm{x}}[\mathrm{B}]^{1 / \mathrm{Y}}[\mathrm{C}]^{\mathrm{X} / \mathrm{Y}}$. The order
of the reaction is:
(a) $\mathrm{x}+\frac{(1+\mathrm{X})}{\mathrm{Y}}$
(b) $\mathrm{X}-\mathrm{Y}+\frac{\mathrm{X}}{\mathrm{Y}}$
(c) $\mathrm{X}+\mathrm{Y}+\frac{\mathrm{X}}{\mathrm{Y}}$
(d) $2(\mathrm{X}+\mathrm{Y})$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:09

Problem 100

If the half-life period of a radioactive isotope is $10 \mathrm{~s}$, then its average life will be:
(a) $14.4 \mathrm{~s}$
(b) $1.44 \mathrm{~s}$
(c) $0.144 \mathrm{~s}$
(d) $2.44 \mathrm{~s}$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:16

Problem 101

In the first-order reaction, half of the reaction is completed in 100 seconds. The time for $99 \%$ reaction to occur will be:
(a) $664.64 \mathrm{~s}$
(b) $646.6 \mathrm{~s}$
(c) $660.9 \mathrm{~s}$
(d) $654.5 \mathrm{~s}$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:25

Problem 103

When the temperature of a reaction increases from $27^{\circ} \mathrm{C}$ to $37^{\circ} \mathrm{C}$, the rate increases by $2.5$ times, the activation energy in the temperature range is:
(a) $70.8 \mathrm{~kJ}$
(b) $7.08 \mathrm{~kJ}$
(c) $35.8 \mathrm{~kJ}$
(d) $14.85 \mathrm{~kJ}$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:16

Problem 104

The rate of the reaction for $\mathrm{A} \longrightarrow$ Products is 10 mol $\mathrm{L}^{-1} \mathrm{~min}^{-1}$ at time $\mathrm{t}_{1}=2$ minutes. What will be the rate (in $\operatorname{mol} \mathrm{L}^{-1} \mathrm{~min}^{-1}$ ) at time $\mathrm{t}_{2}=12$
minutes?
(a) More than 10
(b) Less than 10
(c) 10
(d) 20

Hunza Gilgit
Hunza Gilgit
Numerade Educator
01:22

Problem 105

Consider the following reaction:
$\mathrm{A} \longrightarrow$ products
This reaction is completed in 100 minutes. The rate constant of this reaction at $t_{1}=10$ min is $10^{-2} \mathrm{~min}^{-1}$. What is the rate constant (in $\mathrm{min}^{-1}$ ) at $\mathrm{t}_{2}=20 \mathrm{~min} ?$
(a) $2 \times 10^{-2}$
(b) $10^{-2}$
(c) $5 \times 10^{-3}$
(d) $0.1$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
00:59

Problem 106

Consider the chemical reaction:
$$
\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \longrightarrow 2 \mathrm{NH}_{3}(\mathrm{~g})
$$
The rate of this reaction can be expressed in terms of time derivatives of concentration of $\mathrm{N}_{2}(\mathrm{~g}), \mathrm{H}_{2}(\mathrm{~g})$ or $\mathrm{NH}_{3}(\mathrm{~g}) .$ Identify the correct relationship amongst the rate expressions:
(a) rate $=-\mathrm{d}\left[\mathrm{N}_{2}\right] / \mathrm{dt}=-1 / 3 \mathrm{~d}\left[\mathrm{H}_{2}\right] / \mathrm{dt}=V_{2} \mathrm{~d}\left[\mathrm{NH}_{3}\right] / \mathrm{dt}$
(b) rate $=-\mathrm{d}\left[\mathrm{N}_{2}\right] / \mathrm{dt}=-3 \mathrm{~d}\left[\mathrm{H}_{2}\right] / \mathrm{dt}=2 \mathrm{~d}\left[\mathrm{NH}_{3}\right] / \mathrm{dt}$
(c) rate $=-\mathrm{d}\left[\mathrm{N}_{2}\right] / \mathrm{dt}=-1 / 3 \mathrm{~d}\left[\mathrm{H}_{2}\right] / \mathrm{dt}=2 \mathrm{~d}\left[\mathrm{NH}_{3}\right] / \mathrm{dt}$
(d) rate $=-\mathrm{d}\left[\mathrm{N}_{2}\right] / \mathrm{dt}=-\mathrm{d}\left[\mathrm{H}_{2}\right] / \mathrm{dt}=\mathrm{d}\left[\mathrm{NH}_{3}\right] / \mathrm{dt}$

Mishal Gul
Mishal Gul
Numerade Educator
01:12

Problem 107

The rate constant for the reaction,
$$
2 \mathrm{~N}_{2} \mathrm{O}_{5} \longrightarrow 4 \mathrm{NO}_{2}+\mathrm{O}_{2}
$$
is $3.0 \times 10^{-5} \mathrm{~s}^{1} .$ If the rate is $2.40 \times 10^{-5} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{1}$,
then the concentration of $\mathrm{N}_{2} \mathrm{O}_{5}$ (in mol $\mathrm{L}^{4}$ ) is:
(a) $1.4$
(b) $1.2$
(c) $0.04$
(d) $0.8$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
00:49

Problem 108

Consider the following reaction:
$\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \longrightarrow 2 \mathrm{NH}_{3}(\mathrm{~g})$
The rate of this reaction in terms of $\mathrm{N}_{2}$ at $\mathrm{T}$ is $-\mathrm{d}\left[\mathrm{N}_{2}\right] / \mathrm{dt}=0.02 \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}$
What is the value of $\mathrm{d}\left[\mathrm{H}_{2}\right] / \mathrm{dt}$ (in units of $\mathrm{mol} \mathrm{L}^{-1} \mathrm{~s}^{-1}$ )
at the same temperature?
(a) $0.02$
(b) 50
(c) $0.06$
(d) $0.04$

Mishal Gul
Mishal Gul
Numerade Educator
01:20

Problem 109

The rate constant of a reaction at temperature 200 is 10 times less than the rate constant at $400 \mathrm{~K}$. What is the activation energy $\left(\mathrm{E}_{2}\right)$ of the reaction? $(\mathrm{R}=$ gas constant):
(a) $1842.4 \mathrm{R}$
(b) $921.2 \mathrm{R}$
(c) $460.0 \mathrm{R}$
(d) $230.3 \mathrm{R}$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
00:28

Problem 110

Which one of the following equations is correct for the reaction:
$\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \longrightarrow 2 \mathrm{NH}_{3}(\mathrm{~g}) ?$
(a) $\frac{1}{3} \frac{\mathrm{d}\left[\mathrm{NH}_{3}\right]}{\mathrm{dt}}=\frac{1}{2} \frac{\mathrm{d}\left[\mathrm{H}_{2}\right]}{\mathrm{dt}}$
(b) $\frac{1}{2} \frac{\mathrm{d}\left[\mathrm{NH}_{3}\right]}{\mathrm{dt}}=\frac{1}{-3} \frac{\mathrm{d}\left[\mathrm{H}_{2}\right]}{\mathrm{dt}}$
(c) $\frac{1}{2} \frac{d\left[\mathrm{NH}_{3}\right]}{\mathrm{dt}}=\frac{1}{3} \frac{\mathrm{d}\left[\mathrm{H}_{2}\right]}{\mathrm{dt}}$
(d) $\frac{1}{3} \frac{\mathrm{d}\left[\mathrm{NH}_{3}\right]}{\mathrm{dt}}=\frac{1}{-2} \frac{\mathrm{d}\left[\mathrm{H}_{2}\right]}{\mathrm{dt}}$

Mishal Gul
Mishal Gul
Numerade Educator
01:11

Problem 111

The time taken for the completion of $90 \%$ of a firstorder reaction is 't' min. What is the time (in seconds) taken for the completion of $99 \%$ of the reaction?
(a) $2 \mathrm{t}$
(b) $\mathrm{t} / 30$
(c) $120 \mathrm{t}$
(d) $60 \mathrm{t}$

Hunza Gilgit
Hunza Gilgit
Numerade Educator
00:53

Problem 112

Observe the following reaction.
$$
2 \mathrm{~A}+\mathrm{B} \longrightarrow \mathrm{C}
$$
The rate of formation of is $2.2 \times 10^{-3} \mathrm{~mol} . \mathrm{L}^{-1} .$ What is the value of ${ }^{-} \mathrm{d}[\mathrm{A}] / \mathrm{dt}\left(\mathrm{in} \mathrm{mol} \mathrm{L}^{-1} \mathrm{~min}^{-1}\right)$ ?
(a) $2.2 \times 10^{-3}$
(b) $1.1 \times 10^{-3}$
(c) $4.4 \times 10^{-3}$
(d) $5.5 \times 10^{-3}$

Mishal Gul
Mishal Gul
Numerade Educator
00:42

Problem 113

For a reaction $\frac{1}{2} \mathrm{~A} \longrightarrow 2 \mathrm{~B}$, rate of disappearance of ' $\mathrm{A}$ ' is related to the rate of appearance of ' $\mathrm{B}$ ' by the expression:
(a) $-\frac{\mathrm{d}[\mathrm{A}]}{\mathrm{dt}}=\frac{1}{2} \frac{\mathrm{d}[\mathrm{B}]}{\mathrm{dt}}$
(b) $-\frac{\mathrm{d}[\mathrm{A}]}{\mathrm{dt}}=\frac{1}{4} \frac{\mathrm{d}[\mathrm{B}]}{\mathrm{dt}}$
(c) $-\frac{\mathrm{d}[\mathrm{A}]}{\mathrm{dt}}=\frac{\mathrm{d}[\mathrm{B}]}{\mathrm{dt}}$
(d) $-\frac{\mathrm{d}[\mathrm{A}]}{\mathrm{dt}}=4 \frac{\mathrm{d}[\mathrm{B}]}{\mathrm{dt}}$

Mishal Gul
Mishal Gul
Numerade Educator
00:50

Problem 114

For a reaction $\mathrm{A}+\mathrm{B} \longrightarrow \mathrm{C}+\mathrm{D}$ if the concentration of A is doubled without altering the concentration of $\mathrm{B}$, the rate gets doubled. If the concentration of is increased by nine times without altering the concentration of $\mathrm{A}$, the rate gets tripled. The order of the reaction is:
(a) 2
(b) 1
(c) $3 / 2$
(d) $4 / 3$

Mishal Gul
Mishal Gul
Numerade Educator
00:39

Problem 115

For the reaction $\mathrm{A} \longrightarrow$ Products, it is found that the rate of reaction increases by a factor of $6.25$, when the concentration of $\mathrm{A}$ is increased by a factor of $2.5$. The order of reaction with respect to $\mathrm{A}$ is:
(a) $0.5$
(b) 1
(c) 2
(d) 3

Mishal Gul
Mishal Gul
Numerade Educator
00:54

Problem 116

For a gaseous reaction
$$
2 \mathrm{~A}+\mathrm{B} \longrightarrow 2 \mathrm{AB}
$$
The following rate data were obtained at $300 \mathrm{~K}$.What is the rate law?
(a) $\mathrm{r}=k[\mathrm{~A}]\left[\mathrm{B}_{2}\right]$
(b) $r=[\mathrm{A}]^{2}\left[\mathrm{~B}_{2}\right]^{1}$
(c) $\mathrm{r}=k[\mathrm{~A}]\left[\mathrm{B}_{2}\right]^{2}$
(d) $\mathrm{r}=k\left[\mathrm{~B}_{2}\right]$

Mishal Gul
Mishal Gul
Numerade Educator
00:41

Problem 117

The basic theory of Arrhenius equation is that:
(1) Activation energy and pre-exponential factors are always temperature independent
(2) The number of effective collisions is proportional to the number of molecule above a certain threshold energy.
(3) As the temperature increases, the number of molecules with energies exceeding the threshold energy increases.
(4) The rate constant is a function of temperature
(a) 2,3 and 4
(b) 1,2 and 3
(c) 2 and 3
(d) 1 and 3

Mishal Gul
Mishal Gul
Numerade Educator
00:43

Problem 118

The slope of the line for the graph of $\log k$ vs $1 / \mathrm{T}$ for the reaction,
$$
\mathrm{N}_{2} \mathrm{O}_{5} \longrightarrow 2 \mathrm{NO}_{2}+\frac{1}{2} \mathrm{O}_{2}
$$
is $-5000 .$ Calculate the energy of activation of the reaction:
(a) $95.7 \mathrm{~kJ} \mathrm{~mol}^{-1}$
(b) $9.57 \mathrm{~kJ} \mathrm{~mol}^{-1}$
(c) $957 \mathrm{~kJ} \mathrm{~mol}^{-1}$
(d) $0.957 \mathrm{~kJ} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$

Mishal Gul
Mishal Gul
Numerade Educator
00:51

Problem 119

For the reaction a $\mathrm{A} \longrightarrow \mathrm{xP}$ when $[\mathrm{A}]=2.2 \mathrm{mM}$
the rate was found to be $2.4 \mathrm{mM} \mathrm{s}^{-1}$. On reducingconcentration of $\mathrm{A}$ to half, the rate changes to $0.6 \mathrm{~m} \mathrm{M} s^{-1}$ The order of reaction with respect to $\mathrm{A}$ is:
(a) $1.5$
(b) $2.0$
(c) $2.5$
(d) $3.0$

Mishal Gul
Mishal Gul
Numerade Educator
00:34

Problem 120

If for a certain first-order reaction, the initial rate is $0.65 \%$ min" , the half-life in one hour is:
(a) $17.76$
(b) $27.14$
(c) $1.776$
(d) $11.66$

Mishal Gul
Mishal Gul
Numerade Educator
00:36

Problem 121

The reaction $\mathrm{X} \longrightarrow$ Product follows first-order kinetics, hi 40 minutes, the concentration of $X$ changes from $0.1 \mathrm{M}$ to $0.025 \mathrm{M}$, then the rate of reaction when concentration of $\mathrm{X}$ is $0.01 \mathrm{M}$ is:
(a) $3.47 \times 10^{-5} \mathrm{M} / \mathrm{min}$
(b) $1.73 \times 10^{-4} \mathrm{M} / \mathrm{min}$
(c) $1.73 \times 10^{-5} \mathrm{M} / \mathrm{min}$
(d) $3.47 \times 10^{-4} \mathrm{M} / \mathrm{min}$

Mishal Gul
Mishal Gul
Numerade Educator
00:39

Problem 122

The following data are obtained from the decomposition of a gaseous compound:
Initial pressure in arm $1.6$
$0.8$ $0.4$
Time for $50 \%$ reaction in $\min 80$ 113 160
The order of the reaction is:
(a) $0.5$
(b) $1.0$
(c) $1.5$
(d) $2.0$

Mishal Gul
Mishal Gul
Numerade Educator
00:32

Problem 123

The following data pertains to the reaction between $\mathrm{A}$ and $\mathrm{B}:$Which of the following inferences are drawn from the above data?
(1) Rate constant of the reaction is $10^{-4}$
(2) Rate law of the reaction is $[\mathrm{A}][\mathrm{B}]$

Mishal Gul
Mishal Gul
Numerade Educator
00:36

Problem 124

The rate constant for an isomerization reaction:
$\mathrm{A} \longrightarrow \mathrm{B}$, is $4.5 \times 10^{-3} \mathrm{~min}^{-1} .$ If the initial concen-
tration of $\mathrm{A}$ is $1 \mathrm{M}$, calculate the rate of reaction after I hour:
(a) $0.34354 \mathrm{Mmin}^{-1}$
(b) $0.034354 \mathrm{M} \mathrm{min}^{-1}$
(c) $0.0034354 \mathrm{M} \mathrm{min}^{-1}$
(d) $0.0003454 \mathrm{M} \mathrm{min}^{-1}$

Mishal Gul
Mishal Gul
Numerade Educator
01:31

Problem 125

In the above equation, what is the value of Arrhenius factor?
(a) $3 \times 10^{6}$
(b) $6.3 \times 10^{9}$
(c) $5.42 \times 10^{13}$
(d) $5.42 \times 10^{10}$

Narayan Hari
Narayan Hari
Numerade Educator
00:33

Problem 126

The rate constant of a reaction is $1.5 \times 10^{7} \mathrm{~s}^{-1}$ at $50^{\circ} \mathrm{C}$ and $4.5 \times 10^{7} \mathrm{~s}^{-1}$ at $100^{\circ} \mathrm{C}$. What is the value of
activation energy?
(a) $2.2 \times 10^{3} \mathrm{~J} \mathrm{~mol}^{-1}$
(b) $2300 \mathrm{~J} \mathrm{~mol}^{-1}$
(c) $2.2 \times 10^{4} \mathrm{~J} \mathrm{~mol}^{-4}$
(d) $220 \mathrm{~J} \mathrm{~mol}^{-1}$

Mishal Gul
Mishal Gul
Numerade Educator
00:40

Problem 127

The activation energies of two reactions are $18 \mathrm{~kJ} \mathrm{~mol}^{-1}$ and $4.0 \mathrm{~kJ} \mathrm{~mol}^{-4}$ respectively. Assuming
the pre-exponential factor to be the same for both reactions, the ratio of their rate constants at $27^{\circ} \mathrm{C}$ is:
(a) $3.656 \times 10^{-3}$
(b) $3.624 \times 10^{-6}$
(c) $36.52 \times 10^{-8}$
(d) $4.656 \times 10^{-4}$

Mishal Gul
Mishal Gul
Numerade Educator
00:49

Problem 128

The rate constant of a reaction is given in $k\left(\mathrm{sec} .^{-1}\right)=$ $\left.14.34-0.25 \times 10^{4}\right) / \mathrm{T}$
What will be the energy of activation?
(a) $24.83 \mathrm{kcal} \mathrm{mol}^{1}$
(b) $49.66 \mathrm{kcal} \mathrm{mol}^{1}$
(c) $12.42 \mathrm{kcal} / \mathrm{mol}$
(d) None of these

Mishal Gul
Mishal Gul
Numerade Educator
00:56

Problem 129

At $380^{\circ} \mathrm{C}$, half-life period for the first-order decomposition of $\mathrm{H}_{2} \mathrm{O}_{2}$ is $360 \mathrm{~min} .$ The energy of activation of the reaction is $200 \mathrm{~kJ}$ mol $^{1}$. Calculate the time required for $75 \%$ decomposition at $450^{\circ} \mathrm{C}$ if half-life for decomposition of $\mathrm{H}_{2} \mathrm{O}_{2}$ is $10.17$ min at $450^{\circ} \mathrm{C}:$
(a) $20.4 \mathrm{~min}$
(b) $408 \mathrm{~min}$
(c) $10.2 \mathrm{~min}$
(d) None of these

Mishal Gul
Mishal Gul
Numerade Educator
00:38

Problem 130

A gaseous compound decomposes on heating as per the following equation:
$\mathrm{A}(\mathrm{g}) \longrightarrow \mathrm{B}(\mathrm{g})+2 \mathrm{C}(\mathrm{g}) .$ After 5 minutes and
20 seconds, the pressure increases by $96 \mathrm{~mm} \mathrm{Hg}$.

Mishal Gul
Mishal Gul
Numerade Educator
00:37

Problem 131

The data given below is for the reaction of $\mathrm{NO}$ and $\mathrm{Cl}_{2}$ to form $\mathrm{NOCl}$ at 295 :What is the rate law?
(a) $\mathrm{r}=k[\mathrm{NO}]\left[\mathrm{Cl}_{2}\right]$
(b) $\mathrm{r}=k\left[\mathrm{Cl}_{2}\right]^{1}[\mathrm{NO}]^{2}$
(c) $\mathrm{r}=k\left[\mathrm{Cl}_{2}\right]^{2}[\mathrm{NO}]$
(d) $\mathrm{r}=k\left[\mathrm{Cl}_{2}\right]^{1}$

Mishal Gul
Mishal Gul
Numerade Educator
01:03

Problem 132

For the reaction, $\mathrm{C}_{2} \mathrm{H}_{4}+\mathrm{H}_{2} \longrightarrow \mathrm{C}_{2} \mathrm{H}_{6}, \Delta \mathrm{E}^{\circ}=$
$-30 \mathrm{kcal} .$ If the reaction is reversible and if the activation energy for the forward reaction is $28.0 \mathrm{kcal}$ and its drops to $10.5 \mathrm{kcal}$ in the presence of a catalyst, the activation energies for the uncatalysed and catalysed reverse reaction are respectively (in kcal):
(a) $58,40.5$
(b) $-58,-40.5$
(c) $40.5,58$
(d) $58.0,-58.0$

Mishal Gul
Mishal Gul
Numerade Educator
00:43

Problem 133

For the thermal rearrangement of vinyl allyl ether (g) to allyl acetaldehyde (g) at $175^{\circ} \mathrm{C}, \mathrm{A}=5 \times 10^{11} \exp$
$(-128000 / \mathrm{RT})$, where $\mathrm{K}$ is in $\mathrm{s}^{-1}$ and activation energy in $\mathrm{J} \mathrm{mol}^{-1}$. The enthalpy of activation in $\mathrm{kJ} \mathrm{mol}^{-1}$ is:
(a) $224.3$
(b) $142.3$
(c) $12.43$
(d) $124.3$

Mishal Gul
Mishal Gul
Numerade Educator
00:26

Problem 134

Which of the following statements are correct about half-life period?
(1) Time required for $99.9 \%$ completion of a reaction is 100 times the half-life period
(2) Time required for $75 \%$ completion of a first-order reaction is double the half-life of the reaction
(3) Average life $=1.44$ times the half-life for firstorder reaction
(4) It is proportional to initial concentration for zeroth-order
(a) 1,2 and 3
(b) 2,3 and 4
(c) 2 and 3
(d) 3 and 4

Mishal Gul
Mishal Gul
Numerade Educator
00:45

Problem 135

When concentrations of the reactants is increased sixteen times, the rate becomes two times. The reaction is of:
(a) $1 / 4$ order
(b) Fourth-order
(c) Third-order
(d) $1 / 8$ order

Mishal Gul
Mishal Gul
Numerade Educator
00:22

Problem 136

For the first order reaction, $3 \mathrm{X} \longrightarrow \mathrm{Y}$ concentration varies with time as shown in the following graph. The half-life of the reaction would be:(a) 4 minutes
(b) 2 minutes
(c) 12 minutes
(d) 6 minutes

Mishal Gul
Mishal Gul
Numerade Educator
00:42

Problem 137

For the reaction a $\mathrm{A} \longrightarrow \mathrm{xP}$ when $[\mathrm{A}]=2.2 \mathrm{mM}$
the rate was found to be $2.4 \mathrm{~m} \mathrm{M} \mathrm{s}^{-1}$ On reducing concentration of $\mathrm{A}$ to half, the rate changes to $0.6 \mathrm{~m} \mathrm{M} \mathrm{s}^{-1} .$ The order of reaction with respect to $\mathrm{A}$ is:
(a) $1.5$
(b) $2.0$
(c) $2.5$
(d) $3.0$

Mishal Gul
Mishal Gul
Numerade Educator
00:39

Problem 138

In a first-order reaction, the concentration of the reactant, decreases from $0.8 \mathrm{M}$ to $0.4 \mathrm{M}$ in 15 minutes. The time taken for the concentration to change from $0.1 \mathrm{M}$ to $0.025 \mathrm{M}$ is:
(a) 30 minutes
(b) 60 minutes
(c) $7.5$ minutes
(d) 15 minutes

Mishal Gul
Mishal Gul
Numerade Educator
00:45

Problem 139

NO react with oxygen to produce $\mathrm{NO}_{2}$ $2 \mathrm{NO}+\mathrm{O}_{2}+\longrightarrow_{\mathrm{g}^{\prime}}{\longrightarrow} 2 \mathrm{NO}_{2}$
If the mechanism of the reaction is as follows:
$\mathrm{NO}+\mathrm{O}_{2} \rightleftharpoons \mathrm{NO}_{3}$ (Fast)
$\mathrm{NO}_{3}+\mathrm{NO}_{2} \stackrel{\mathrm{K}_{1}}{\longrightarrow} \mathrm{NO}_{2}+\mathrm{NO}_{2}$ (Slow)
Rate law can be given as:
(a) Rate $=\mathrm{K}^{\prime}[\mathrm{NO}]\left[\mathrm{O}_{2}\right]$
(b) Rate $=\mathrm{K}^{\prime}[\mathrm{NO}]^{2}\left[\mathrm{O}_{2}\right]$
(c) Rate $=\mathrm{K}^{\prime}[\mathrm{NO}]^{3}\left[\mathrm{O}_{2}\right]$
(d) Rate $=\mathrm{K}[\mathrm{NO}]\left[\mathrm{O}_{2}\right]^{2}$

Mishal Gul
Mishal Gul
Numerade Educator
00:42

Problem 140

For a homogenous gaseous reaction:
$\mathrm{P} \longrightarrow \mathrm{Q}+\mathrm{R}+\mathrm{S}$, the initial pressure was $\mathrm{P}_{0}$ while
pressure after time ' $\mathrm{t}$ ' was $\mathrm{P}$ if ( $\mathrm{P}$ is more than $\mathrm{P}_{\mathrm{o}}$ ), the expression for the rate constant $(\mathrm{K})$ is:
(a) $\mathrm{K}=\frac{2.303}{\mathrm{t}} \log _{10}\left(\frac{\mathrm{P}_{\mathrm{o}}}{\mathrm{P}_{\mathrm{o}}-\mathrm{P}}\right)$
(b) $K=\frac{2.303}{t} \log _{10}\left(\frac{3 P_{o}}{2 P_{0}-P}\right)$
(c) $K=\frac{2.303}{t} \log _{10}\left(\frac{2 P_{o}}{3 P_{0}-P}\right)$
(d) $K=\frac{2.303}{t} \log _{10}\left(\frac{2 P_{0}}{4 P_{e}-P}\right)$

Mishal Gul
Mishal Gul
Numerade Educator