The number of correct statement/s from the following is _____ .

A.Larger the activation energy, smaller is the value of the rate constant.

B. The higher is the activation energy, higher is the value of the temperature coefficient.

C. At lower temperatures, increase in temperature causes more change in the value of $\mathrm{k}$ than at higher temperature.

D. A plot of $\ln \mathrm{k}$ vs $\frac{1}{ \mathrm{T}}$ is a straight line with slope equal to $-\frac{\mathrm{Ea}}{\mathrm{R}}$

A student has studied the decomposition of a gas $A{B}_3$ at $25°C$. He obtained the following data

The order of the reaction is

For the first order reaction $\mathrm{A}\to \mathrm{B}$  the half life is $30 \min$. The time taken for $75\%$ completion of the reaction is mm. (Nearest integer)

Given : $\log 2=0.3010$

$\log 3=0.4771$

$\log 5=0.6989$

A first order reaction has the rate constant,  $\mathrm{k}=4.6\times {10}^{-3} {\mathrm{s}}^{-1}$. The number of correct statement/s from the following is/are Given: $\log 3=0.48$.

A. Reaction completes in $1000 \mathrm{s}$.
B. The reaction has a half-life of $500 \mathrm{s}$.
C. The time required for $10\%$ completion is 25 times the time required for 90% completion.
D. The degree of dissociation is equal to $\left(1-{\mathrm{e}}^{-\mathrm{kt}}\right)$.
E. The rate and the rate constant have the same unit.

For certain chemical reaction $\mathrm{X}\to \mathrm{Y}$, the rate of formation of product is plotted against the time as shown in the figure. The number of Correct statement/s from the following is _____ 

(A) Over all order of this reaction is one
(B) Order of this reaction can't be determined
(C) In region-I and III, the reaction is of first and zero order respectively
(D) In region-II, the reaction is of first order
(E) In region-II, the order of reaction is in the range of $0.1$ to $0.9$.

An organic compound undergoes first order decomposition. If the time taken for the $60\%$ decomposition is $540 \mathrm{s}$, then the time required for $90\%$ decomposition will be is _____ s. (Nearest integer).

Given : $\ln 10=2.3;\log 2=0.3$

$\mathrm{A}\to \mathrm{B}$

The rate constants of the above reaction at $200 \mathrm{K}$ and $300 \mathrm{K}$ are $0.03 {\min }^{-1}$ and $0.05 {\min }^{-1}$ respectively. The activation energy for the reaction is $\mathrm{J}$ (Nearest integer)

(Given : In $10=2.3$

$\mathrm{R}=8.3 \mathrm{J} {\mathrm{K}}^{-1} {\mathrm{mol}}^{-1}$

$\log 5=0.70$

$\log 3=0.48$

$\log 2=0.30$