Chemical kinetics practice · Easy

Which one of the following is a second order reaction?

For a first order reaction $k = 100\;{\mathrm{s}^{ - 1}}\mathrm{.}$ The time for completion of 50% reaction is

The rate of reaction increases with temperature due to

Half-life period of second order reaction is

Rate of reaction depends upon

Which of the following statements are correct?

1. Order of a reaction can be known from experimental result and not from the stoichiometry of reaction

2. Overall molecularity of a reaction may be determined in a manner similar to overall order of reaction

3. Overall order of reaction,

${A^m} + {B^n} \to A{B_x}\;is\;\left( {m + n} \right)$

4. Molecularity of a reaction refers to

(i) Molecularity of each of the elementary steps (slow steps) in a multistep reaction

(ii) Molecularity of that particular step in a single step reaction

Select the correct answer by using the codes given below

For zero order reaction the integrated rate equation is

An increase in the concentration of reactants of a reaction leads to change in

The rate constant for a reaction is $10.8 \times {10^{ - 5}}\,\,mol.{L^{ - 1}}.{S^{ - 1}}$ the reaction obeys

A zero order reaction is one:

Rate constant of a reaction depends upon

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

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 …$\mathrm{kJ}\;\mathrm{mo}{\mathrm{l}^{ - 1}}$.

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:

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 $303\;K\;to\;353\;K$?

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

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:

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:

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 $303\;K\;to\;353\;K$?

The integrated rate equations can be determined for

The concentration of R in the reaction $R \to P$ was measured as a function of time and the following data is obtained
$\begin{array}{llllllllllllllllllll} {\left[ R \right]\left( {molar} \right)\;\;\;1.00\;\;\;\;\;\;0.75\;\;\;\;\;0.40\;\;\;\;\;0.10}\\ {t\;\left( {min} \right)\;\;\;\;\;\;\;\;\;0.00\;\;\;\;\;0.05\;\;\;\;\;0.12\;\;\;\;\;0.18} \end{array}\;$
The order of the reaction is

For the reaction $2A + B \to 3\,C + D$, which of the following does not express the reaction rate

Assertion (A):The instantaneous rate of reaction can be studied in chemical kinetics.

Reason (R): Ionic reactions occur instantaneously.

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

Which of the following expression is correct for second order reaction. (${C_0}$ refers to initial concentration of reactant)?

The rate of a chemical reaction doubled for every $10^\circ C$ rise in temperature. If the temperature is increased by $60^\circ C$ the rate of reaction increase by