Chemical kinetics practice · Mixed difficulty

A catalyst is used in a reaction to

The time taken for the completion of $3/4$ of a first order reaction is

The reaction $2S{O_2}\left( g \right) + {O_2}\left( g \right)\;\leftrightharpoons\;2S{O_3}\left( g \right)$ is carried out in a $1\;d{m^3}$ vessel and $2\;d{m^3}$ vessel separately. The ratio of the reaction velocities will be

If rate constant of a reaction is $1.155 \times {10^{ - 3}}{s^{ - 1}}$ then the half life period for the reaction will be

The following equilibrium constants are given
${N_2} + 3{H_2} \rightleftarrows 2N{H_3};{K_1}$
${N_2} + {O_2} \rightleftarrows 2NO;{K_2}$
${H_2} + \frac{1}{2}{O_2} \rightleftarrows {H_2}O;{K_3}$
The equilibrium constant for the oxidation of $2\,{\text{mol}}\,N{H_3}$ by oxygen to $NO$ is

The rate constant for a first order reaction which has half-life 231 s is

The rate constant is numerically the same for three reactions of first, second and third order respectively. Which one is true for rate of three reaction?

The rate of first order reaction, $A \to \;products$, is $7.5 \times {10^{ - 4}}\;\mathrm{mol}\;\mathrm{litr}{\mathrm{e}^{ - 1}}\;{\sec ^{ - 1}}.$ If the concentration of $A\;is\;0.5\;\mathrm{mol}\;\mathrm{litr}{\mathrm{e}^{ - 1}}$ the rate constant is:

Identify correct statements.

As the temperature increases.

A) Rate of reaction increases

B) Number of activated molecules increases

C) Collision frequency increases

In a first order reaction the $a/\left( {a - x} \right)$ was found to be 8 after 10 minute. The rate constant is:

The temperature coefficient of a reaction is:

In the respect of the equation $k = A{e^{ - {E_a}/RT}}$ in chemical kinetics, which one of the following statements is correct?

$\frac{{{K_{{{35}^0}}}}}{{{K_{{{34}^0}}}}} > 1$, this means that

The two reactions $\text{(I) } \mathrm{A} \rightarrow \text{Products},$ and $\text{(II) } \mathrm{B}\rightarrow \text{Products}$ follow first-order kinetics. The rate of reaction-I is doubled when temperature is raised from $300$ to $310 \mathrm{~K}.$ The half-life for this reaction at $310 \mathrm{~K}$ is 30 minutes. At the same temperature, B decomposes twice as fast as A. If the energy of activation for the reaction-II is half that of reaction-I, the rate constant of reaction-II at 300 K is

The activation energy of a reaction is zero. The rate constant for the reaction

During the kinetic study of the reaction $2A + B \to C + D$ following results were obtained.

$\begin{array}{l} Run\;\;\;\;[A]\;\;in\;M\;\;\;\;[B]\;in\;M\;\;\;\;Initial\;rate\;of\;formation\;of\;D\;in\;M\;{s^{ - 1}}\\ I\;\;\;\;\;\;\;\;\;\;\;\;0.1\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;0.1\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;6.0 \times {10^{ - 3}}\;\\ II\;\;\;\;\;\;\;\;\;\;\;0.3\;\;\;\;\;\;\;\;\;\;\;\;\;\;0.2\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;7.2 \times {10^{ - 2}}\;\;\\ III\;\;\;\;\;\;\;\;\;\;0.3\;\;\;\;\;\;\;\;\;\;\;\;\;\;0.4\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;2.88 \times {10^{ - 1}}\;\;\;\;\\ IV\;\;\;\;\;\;\;\;\;\;0.4\;\;\;\;\;\;\;\;\;\;\;\;\;\;0.1\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;2.40 \times {10^{ - 2}}\;\;\;\; \end{array}$

On the basis of above data which one is correct:

Consider the following statements

a) Increase in concentration of reactant increases the rate of zero order reaction

b) Rate constant K is equal to collision frequency A if ${E_a} = 0$

c) Rate constant K is equal to collision frequency A if ${E_a} = \, \propto$

d) ln K Vs T is a straight line

e) ln K Vs 1/T is a straight line

Correct statements are

A first order reaction is carried out with an initial concentration of 10 mole per litre and $80\%$ of the reactant changes into the product. Now if the same reaction is carried out with an initial concentration of 5 mol per litre the percentage of the reactant changing to the product is:

Two reactions $A \to products$ and $B \to products$ have rate constants ${K_A}$ and ${K_B}$ at temperature $T$ and activation energies ${E_A}$ and ${E_B}$ respectively. If ${K_A} > {K_B}$&nbsp; and ${E_A} < {E_B}$ and assuming that $A$ for both the reactions is same, then:

For the first order reaction with the rate constant $k$, which expression gives the rate half-life period? $(Initial\mathrm{ }conc.\mathrm{ } = a)$

$A + B \to products$
If concentration of $A$ is doubled, rate increases 4 times. If concentration of $A$ and $B$ are doubled, rate increases 8 times. The differential rate equation of the reaction will be

Which one is not correct, according to Arrhenius equation:

The correct difference between first and second – order reactions is that

For the reaction,

$2{N_2}{O_5}\left( g \right) \to 4N{O_2}\left( g \right) + {O_2}\left( g \right)$

If the concentration of $N{O_2}$ increase by $5.2 \times {10^{ - 3}}\;M$ in 100 s then the rate of the reactions

The rate equation for the reaction $2A + B \to C$ is found to be
$Rate = k\left[ A \right]\left[ B \right]$
The correct statement in relation to this reaction that the

For the reaction, $2A + B \to products$, the active mass of B is kept constant, and that of A is doubled. The rate of reaction will be then

Activation energy is given by

In the reaction,

$2{N_2}{O_5} \to 4N{O_2} + {O_2}$ initial pressure is $500\;atm$ and rate constant $k$ is
$3.38 \times {10^{ - 5}}\;{s^{ - 1}}$ after 10 min the final pressure of ${N_2}{O_5}$ is

A mixture of ${ }^{239} \mathrm{Pu}$ and ${ }^{240} \mathrm{Pu}$ has specific activity of $6 \times$ $10^9(\mathrm{dps}) \mathrm{gm}^{-1}$. The half-life of the isotopes are $2.44 \times 10^4$ years (for ${ }^{239} \mathrm{Pu}$ ) and $6.58 \times 10^3$ years (for ${ }^{240} \mathrm{Pu}$ ) respectively. Determine the isotropic composition of this sample in nearest possible integers.

For an elementary reaction $2 {A} \rightarrow {B},$ consider following statements:

(a) Rate law can be written as rate $={k}[{A}]^2$

(b) On increasing temperature, rate constant $k$ decreases.

(c) On doubling the volume, rate becomes one fourth.

(d) On doubling the concentration, rate becomes one fourth.

Choose the correct answer from the options given below: