Chemical kinetics practice · Mixed difficulty

Which statement is not correct?

The data for the reaction, $\mathrm{ }A + B \to C$
$\begin{array}{l} Ex\;\;\;\;\;\;\;\;\;\;\;{\left[ A \right]_0}\;\;\;\;\;\;\;\;\;{\left[ B \right]_0}\;\;\;\;\;\;\;\;\;Initial\;\mathrm{ }rate\\ \begin{array}{llllllllllllllllllll} {1\;\;\;\;\;\;\;\;\;\;\;\;\;\;0.012\;\;\;\;\;\;\;\;0.035\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;0.10}\\ {2\;\;\;\;\;\;\;\;\;\;\;\;\;0.024\;\;\;\;\;\;\;\;\;0.070\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;0.80}\\ {3\;\;\;\;\;\;\;\;\;\;\;\;\;0.024\;\;\;\;\;\;\;\;\;\;0.035\;\;\;\;\;\;\;\;\;\;\;\;\;0.10}\\ {4\;\;\;\;\;\;\;\;\;\;\;\;\;0.012\;\;\;\;\;\;\;\;\;0.070\;\;\;\;\;\;\;\;\;\;\;\;\;0.80} \end{array} \end{array}$
The rate law corresponds to the above data is

Slope and intercepts of the plots $\mathrm{ }lo{g_{10}}\;K\;\mathrm{vs}\;\frac{1}{T}$ are given respectively by :

In a reaction, the threshold energy is equal to:

In the given first-order sequential reactions $\mathrm{A}\xrightarrow{K_1} \mathrm{B} \xrightarrow{K_2} \mathrm{C} \xrightarrow{K_3} \mathrm{D},$ what is the ratio of number of atoms of $\mathrm{A}$ to the number of atoms of $\text{B}$ after long time interval starting with pure $\text{A}?$ $\left(K_1=\frac{\ln 2}{1200} \text{ and }K_2=\frac{\ln 2}{30}\right)$

Which of the following quantities changes on addition of a catalyst during a chemical reaction ?

The efficiency of an enzyme in catalyzing a reaction is due to its capacity

From the following data, the activation energy for the reaction (cal/mol):

${\mathrm{H}_2} + {\mathrm{I}_2} \to 2\mathrm{HI}$

$\begin{array}{l} T,K\;\;\;\;\;\;1T,{K^{ - 1}}\;\;\;\;\;\;{\log _{10}}K\\ 769\;\;\;\;\;1.3 \times {10^{ - 3}}\;\;\;\;\;\;\;\;2.9\\ 667\;\;\;\;\;1.5 \times {10^{ - 3}}\;\;\;\;\;\;\;\;1.1 \end{array}$

For a certain reaction a plot of $\frac{{\left[ {{c_0} - c} \right]}}{c}$ against time $t$, yields a straight line. ${{c_0}\;and\;c}$ are concentrations of reactant at $t = 0\;and\;t = t$ respectively. The rate of reaction is:

For the reaction ${aA}+{bB} \rightarrow {P}, r=K[{A}]^a \cdot [{B}]^b,$ if the concentration of ${A}$ is doubled, then the rate is doubled. If the concentration of ${B}$ is doubled, then the rate becomes four times. The correct relation is

Which plots will give the value of activation energy?

For a reaction $A \to products,$ rate law is -$- \frac{{d\left[ A \right]}}{{dt}} = K{\left[ A \right]_0}.$ The concentration of A left after time $t$ when $t = \frac{1}{K}$ is:

In a reaction $2A \to products$; the concentration of A decreases from $0.5\;\mathrm{mol}\;\mathrm{litr}{\mathrm{e}^{ - 1}}\;to\;0.4\;\mathrm{mol}\;\mathrm{litr}{\mathrm{e}^{ - 1}}$ in 10 minute. The rate of reaction during this interval is:

The slope of Arrhenius plot $\left( {\ln \,k\,\mathrm{v/s}\frac{1}{T}} \right)$ of first order reaction is $- 5 \times {10^3}K.$ The value of ${E_a}$ of the reaction is.
Choose the correct option for your answer.
[Given $R = 8.314\mathrm{ J}{\mathrm{K}^{ - 1}}\mathrm{ mo}{\mathrm{l}^{ - 1}}$]

${\mathrm{N}_2}\left( \mathrm{g} \right) + 3{\mathrm{H}_2}\left( \mathrm{g} \right)\;\leftrightharpoons\;2\mathrm{N}{\mathrm{H}_3}\left( \mathrm{g} \right) + 22\;\mathrm{kcal}$.

The activation energy for the forward reaction is $50\mathrm{ }\;kcal.$ What is the activation energy for the backward reaction?

For a fist order reaction, the concentration changes from $0.8\mathrm{ }\;to\;\mathrm{ }0.4\mathrm{ }\;in\mathrm{ }\;15\;\mathrm{ }min.$. The time taken for the concentration to change from $0.1\mathrm{ }\;M\;\mathrm{ }to\;\mathrm{ }0.025\mathrm{ }\;M\;\mathrm{ }is$

Consider the two hypothetical reactions given below:

I $a A \rightarrow$ Products, $k=x \mathrm{~mol}^{-1} \mathrm{~L} \mathrm{~min}^{-1}$
II $b B \rightarrow$ Products, $k=y \mathrm{~min}^{-1}$

The half-lives of both the reactions are the same, equal to $1 \mathrm{hr}$ when molar concentration of the reactant is $1.0 \mathrm{M}$ in each case. If these reactions are started at the same time taking $1 \mathrm{M}$ of the reactant in each case, the ratio $[A]/[B]$ after $3 \mathrm{hr}$ will be:

The rate constant ${K_1}$ of a reaction is found to be double that of rate constant ${K_2}$ of another reaction. The relationship between corresponding activation energies of the two reactions at same temperature $({E_1}\;and\;{E_2})$ can be represented as:

The decomposition of ${N_2}{O_5}$ occur as $2{N_2}{O_5}\, \to \,\,4N{O_2} + {O_2},$ and follows Ist order kinetics, hance

Choose correct option based on following statements. Here T stands for true statement and F for false statement.

(i) Molecularity is defined as the number of reacting species taking part in a complex reaction,

(ii) Molecularity helps in understanding the mechanism of reaction.

(iii) Reactions with the molecularity three are very rare and slow to proceed.

(iv) Complex reactions involving more than three molecules take place in more than one step.

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:

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 a certain reaction involving a single reactant, it is found that $C_0 \sqrt{T}$ is constant, where $C_0$ is the initial concentration of the reactant and $T$ is the half-life. What is the order of the reaction?

For a chemical reaction $X \to P$, the rate of reaction doubles when the concentration of X is increased 4 times. The order of reaction with respect to X is

Select the correct statements out of I, II and III for zero order reaction.

(I) Quantity of the products formed is directly proportional to time.

(II) Larger the initial concentration of the reactant, greater the half-life period.

(III) If $50 \%$ reaction takes place in $100 \mathrm{~min}, 75 \%$ reaction takes place in $150 \mathrm{~min}$.

With increase in temperature, rate of reaction

For a reaction between A and B, the initial rate of reaction is measured for various initial concentrations A and B. the data provided are

$\begin{array}{l} \,\,\,\,\,\,\,\,\,\,\,\,\left[ A \right]\,\,\,\,\,\,\,\,\,\,\,\left[ B \right]\;\;\;\;\;\;\;Initial\mathrm{ }reaction\mathrm{ }rate\\ 1\,\,\,\,\,\,\,0.20M\,\,\,\,\,0.30M\,\,\,\,\,\,5 \times {10^{ - 5}}\\ 2\,\,\,\,\,0.20\mathrm{ }M\,\,\,\,0.10\mathrm{ }M\,\,\,\,\,\,5 \times {10^{ - 5}}\\ 3\,\,\,\,\,0.40\mathrm{ }M\,\,\,\,0.05\mathrm{ }M\,\,\,\,\,\,1 \times {10^{ - 5}} \end{array}$

The overall order of the reaction is

Which of the following statement is not correct for the reaction: $4A + B \to 2C + 2D$

The rate of the reaction $A \to products$, at the initial concentration of $3.24 \times {10^{ - 2}}\;M$ is nine times its rate at another initial concentration of $1.2 \times {10^{ - 3}}\;M$. The order of the reaction is

For a gaseous reaction $\mathrm{A}(\mathrm{g}) \rightarrow \text{Products (order} = n),$ the rate may be expressed as

(i) $-\frac{\mathrm{d} P_{\mathrm{A}}}{\mathrm{d} t}=K_1 \cdot P_{\mathrm{A}}^n$

(ii) $-\frac{1}{V} \frac{\mathrm{d} n_{\mathrm{A}}}{\mathrm{d} t}=K_2 \cdot C_{\mathrm{A}}^n$

The rate constants, $K_1$ and $K_2$ are related as $\left(P_{\mathrm{A}}\right.$ and $C_{\mathrm{A}}$ are the partial pressures and molar concentration of $\text{A}$ at time '$t$', respectively)