Embibe Experts Solutions for Chapter: Chemical Kinetics, Exercise 1: JEE Main - 10th April 2015

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 $0.9$.

For conversion of compound $\mathrm{A}\to \mathrm{B}$, the rate constant of the reaction was found to be $4.6\times {10}^{-5} \mathrm{Lmol}{}^{-1} {\mathrm{s}}^{-1}$. The order of the reaction is _____ .

If compound $\mathrm{A}$ reacts with $\mathrm{B}$ following first order kinetics with rate constant $2.011\times {10}^{-3} {\mathrm{s}}^{-1}$. The time taken by A (in seconds) to reduce from $7 \mathrm{g}$ to $2 \mathrm{g}$ will be _____ . (Nearest Integer) $\left[\log 5=0.698,\log 7=0.845,\log 2=0.301\right]$

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 $10=2.3$

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

$\log 5=0.70$

$\log 3=0.48$

$\log 2=0.30$

The rate constant for a first order reaction is $20 {\min }^{-1}$. The time required for the initial concentration of the reactant to reduce to its $\frac{1}{32}$ level is $\_\_\_\_\_\_\times {10}^{-2} \min$. (Nearest integer)

A and B are two substances undergoing radioactive decay in a container. The half life of A is $15 \min$ and that of B is $5 \min$. If the initial concentration of B is $4$ times that of A and they both start decaying at the same time, how much time will it take for the concentration of both of them to be same? ________min.

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

The above reaction is of zero order. Half life of this reaction is $50 \min$. The time taken for the concentration of $\mathrm{A}$ to reduce to one-fourth of its initial value is min . (Nearest integer)