Chemical kinetics practice · Mixed difficulty

The half life of a first order reaction is 2000
years. If the concentration after 8000 years is
0.02 M, then the initial concentration was:

Rate constant of a reaction depends upon

Consider the given reaction

$\mathrm{N}_2 \mathrm{O}_4 \rightarrow 2 \mathrm{NO}_2$

Initial conc. of $\mathrm{N}_2 \mathrm{O}_4=3 \mathrm{M}$

Concentration of $\mathrm{N}_2 \mathrm{O}_4$ is $2.75 \mathrm{M}$

after $30 \mathrm{~sec}$., find out rate of formation of $\mathrm{NO}_2$ during this interval (in mol lit ${ }^{-1} \mathrm{~min}^{-1}$ ) (Nearest integer)

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?

$99 \%$ of a first order reaction was completed in $32 {~min}$. When will $99.9 \%$ of the reaction complete

The half-life period for a zero order reaction is equal to

For an elementary reaction $\mathrm{X}+2 \mathrm{Y} \xrightarrow{\mathrm{k}} \mathrm{Z}$
Rate law can be expressed as:

The reason for almost doubling the rate of reaction on increasing the temperature of the reaction system by $10^\circ C$ is

The energies of activation for forward and reverse reactions for ${A_2} + {B_2}\;\leftrightharpoons\;2AB$ are $180\;kJ\;\mathrm{mo}{\mathrm{l}^{ - 1}}$ and $200\;kJ\;\mathrm{mo}{\mathrm{l}^{ - 1}}$ respectively. The presence of a catalyst lowers the activation energy of both (forward and reverse) reactions by $100\;kJ\;\mathrm{mo}{\mathrm{l}^{ - 1}}$. The enthalpy change of the reaction (${A_2} + {B_2} \to 2AB$) in the presence of catalyst will be (in $kJ\;\mathrm{mo}{\mathrm{l}^{ - 1}}$)

For $A + B \to C + D,\;\Delta H = - 20\;\mathrm{kJ}\;\mathrm{mo}{\mathrm{l}^{ - 1}}$ the activation energy of the forward reaction is $85\;\mathrm{kJ}\;\mathrm{mo}{\mathrm{l}^{ - 1}}.$ The activation energy for backward reaction is …$\mathrm{kJ}\;\mathrm{mo}{\mathrm{l}^{ - 1}}$.

Naturally occurring potassium consists of $0.01 \%$ of $40 \mathrm{~K}$ which has a half-life of $1.28 \times 10^9 \mathrm{yr}$. Activity of $1.00 \mathrm{~g}$ sample of $\mathrm{KCl}$ is

The rate of a reaction A doubles on increasing the temperature from 300 to 310 K. By how much, the temperature of reaction B should be increased from 300 K so that rate doubles if activation energy of the reaction B is twice to that of reaction A.

The rate constant of a first order reaction is $4 \times {10^{ - 3\;}}{\sec ^{ - 1}}.$ At a reactant concentration of $0.02\;M$, the rate of reaction would be:

Assertion (A):All catalytic reactions show zero order for catalyst used.

Reason (R): The rate of reaction does not depend on concentration of catalyst.

The rate of a reaction double when its temperature changes from 300 K to 310 K. Activation energy of such a reaction will be $(R = 8.314\,\,\,\mathrm{J}{\mathrm{K}^{ - \mathrm{1}}}\mathrm{mo}{\mathrm{l}^{ - \mathrm{1}}}\,\,\,\,\mathrm{and}\,\,\,\log 2 = 0.301)$

By increase in temperature by $10\;K$, the rate of reaction becomes double. How many times the rate of reaction will be if the temperature is increased from $303\;K\;to\;353\;K$?

If rate constant for a first order reaction is $60 \mathrm{~s}^{-1}$, then how much time will take to reduce the initial concentration of the reactant to its $\frac{1}{16}$ th value?

Which expression is wrong for fist order reaction?

A first order reaction is formed to have a rate constant, $K = 5.5 \times {10^{ - 14}}{S^{ - 1}}$ , then the half life of the reactions is

As the initial concentration increases from $0.75$ to $1.55 \mathrm{~M}$ in a reaction, $t_{1 / 2}$ decreases from $60$ to $29 \mathrm{~s}.$ The order of the reaction is

Following mechanism has been proposed for a reaction,

$2A + B \to D + E$

$A + B \to C + D\;\;\;\;\;\;\;\;\;...(slow)$

$A + C \to E\;\;\;\;\;\;\;....(fast)$

The rate law expression for the reaction is:

A reaction is 50% complete in 2 hours and 75% complete in 4 hours. The order of reaction is

Rate constant $(k)$ of a reaction has least value at

The order of the reaction $\mathrm{A} \rightarrow \text{products}$ is $0.5 .$ The time for complete reaction $T$ and time for $50 \%$ reaction, $t_{1 / 2}$ will be related as

What is order with respect to A, B, C, respectively

$\begin{array}{cccccccccccccccccccc} {[{\text{A}}]}&{[{\text{B}}]}&{[{\text{C}}]}&{{\text{Rate(M/sec)}}} \\ {{\text{0}}{\text{.2}}}&{{\text{0}}{\text{.1}}}&{{\text{0}}{\text{.02}}}&{{\text{8}}.{\text{08}} \times {\text{1}}{{\text{0}}^{{\text{ - 3}}}}} \\ {{\text{0}}{\text{.1}}}&{{\text{0}}{\text{.2}}}&{{\text{0}}{\text{.02}}}&{{\text{2}}.{\text{01}} \times {\text{1}}{{\text{0}}^{{\text{ - 3}}}}} \\ {{\text{0}}{\text{.1}}}&{{\text{1}}{\text{.8}}}&{{\text{0}}{\text{.18}}}&{{\text{6}}.{\text{03}} \times {\text{1}}{{\text{0}}^{{\text{ - 3}}}}} \\ {{\text{0}}{\text{.2}}}&{{\text{0}}{\text{.1}}}&{{\text{0}}{\text{.08}}}&{{\text{6}}.{\text{464}} \times {\text{1}}{{\text{0}}^{{\text{ - 2}}}}} \end{array}$

The first order rate constant $\mathrm{k}$ is related to temperature as $\log \mathrm{k}=15.0-\left(10^6 / \mathrm{T}\right)$ Which of the following pair of value is correct?

If the half-time for a particular reaction is found to be constant and independent of the initial concentration of the reactants, then the ratio is of

Number of mole of a substance present in 1 litre volume is known as:

For an elementary reaction $2A + 3B2C$ . The rate of disappearance of B is

By increase in temperature by $10\;K$, the rate of reaction becomes double. How many times the rate of reaction will be if the temperature is increased from $303\;K\;to\;353\;K$?