Chemical kinetics practice · Mixed difficulty

If the rate constant of the reaction, $X \rightarrow Y$ is $2.5 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}$ and initial concentration of $X$ is $3 \mathrm{~M}$ then the concentration of ${Y}$ after 100 minutes will be

The ${t_{\frac{1}{2}}}$ of a reaction is halved as the initial concentration of the reactant is doubled. What is order of reaction?

For the elementary step,

${\left( {\mathrm{C}{\mathrm{H}_3}} \right)_3} \cdot \mathrm{CBr}\left( {aq} \right) \to {\left( {\mathrm{C}{\mathrm{H}_3}} \right)_3}{\mathrm{C}^ + }\left( {aq} \right) + \mathrm{B}{\mathrm{r}^ - }\left( {aq} \right)$ the molecularity is:

After $20 \%$ completion, the rate of reaction $\mathrm{A} \rightarrow \text{products}$ is 10 unit and after $80 \%$ completion, the rate is 0.625 unit. The order of the reaction is

In the reaction $A + B \to products$, if B is taken in excess, then it is an example of

Which of the following statement is incorrect about the molecularity of a reaction?

The unit of rate constant for a zero order reaction is

Statement I: Rate constants determined from Arrhenius equation are fairly accurate for simple as well as complex molecules

Statement II: Reactant molecules undergo chemical change irrespective of their orientation during collision

Following reaction takes places by mechanism

$\mathrm{NO}_2+\mathrm{CO} \longrightarrow \mathrm{NO}+\mathrm{CO}_2$
Step I $\mathrm{NO}_2+\mathrm{NO}_2 \xrightarrow{k_1 \text {. Slow }} \mathrm{NO}_3+\mathrm{NO}$

Step II $\mathrm{NO}_3+\mathrm{CO} \xrightarrow{k_2 \text {. Fast }} \mathrm{NO}_2+\mathrm{CO}_2$

Hence, $\left(\frac{d x}{d t}\right)$ for the given reaction is

For the reaction $2 \mathrm{NH}_3 \rightarrow \mathrm{N}_2+3 \mathrm{H}_2$,

$-\frac{\mathrm{d}\left[\mathrm{NH}_3\right]}{\mathrm{d} t}=k_1\left[\mathrm{NH}_3\right],-\frac{\mathrm{d}\left[\mathrm{N}_2\right]}{\mathrm{d} t}=k_2\left[\mathrm{NH}_3\right], \frac{\mathrm{d}\left[\mathrm{H}_2\right]}{\mathrm{d} t}=k_3\left[\mathrm{NH}_3\right]$

Then relation between $k_1, k_2$ and $k_3$ is

The half-life for decay of radioactive ${ }^{14} {C}$ is 5730 years. An archaeological artefact containing wood has only $80 \%$ of the ${ }^{14} {C}$ activity as found in living trees. The age of the artefact would be [Given : $\log 1.25=0.0969$]

For a reaction of the type $A + B \to x$ products, it is observed that doubling the concentration of $A$ causes the reaction rate $({k_1})$ to be four times as great but doubling the amount of $B$ does not affect the rate $({k_2})$. The rate equation 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 …$\mathrm{kJ}\;\mathrm{mo}{\mathrm{l}^{ - 1}}$.

After how many second will the concentration of the reactant in a first order reaction be halved if the rate constant is $1.155 \times {10^{ - 3}}\;{s^{ - 1}}?$

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 inversion of cane sugar into glucose and fructose according to the equation ${\mathrm{C}_{12}}{\mathrm{H}_{22}}{\mathrm{O}_{11}} + {\mathrm{H}_2}\mathrm{O} \to {\mathrm{C}_6}{\mathrm{H}_{12}}{\mathrm{O}_6} + {\mathrm{C}_6}{\mathrm{H}_{12}}{\mathrm{O}_6}$ is an example of

The half-life period of a first order reaction is 1 min 40 s. Calculate its rate constant.

Rate of a reaction $\mathrm{A}+\mathrm{B} \longrightarrow \mathrm{C}$ is given below as a function of differential concentrations of $\mathrm{A}$ and $\mathrm{B}$.

$\begin{array}{cccccccccccccccccccc} {{\text{Exp}}{\text{.}}}&{\left[ {\text{A}} \right]}&{\left[ {\text{B}} \right]}&{{\text{Rate}}} \\ {}&{{\text{mol }}{{\text{L}}^{ - 1}}}&{{\text{mol }}{{\text{L}}^{ - 1}}}&{{\text{mol }}{{\text{L}}^{ - 1}}\,{\text{tim}}{{\text{e}}^{ - 1}}} \\ {1.}&{0.01}&{0.01}&{0.005} \\ {2.}&{0.02}&{0.01}&{0.010} \\ {3.}&{0.01}&{0.02}&{0.005} \end{array}$

Determine the order of reaction with respect to $\mathrm{A}$ and and also calculate the half-life of $\mathrm{A}$ in the reaction.

Rate constant $(\mathrm{K})$ varies with temperature as given by equation $\log \mathrm{K}\left(\mathrm{min}^{-1}\right)=5-\frac{2000}{\mathrm{T}}$
Consider the following about this equation
(I) Pre exponential factor is $10^5$.
(II) $\mathrm{E}_\alpha$ is $9.212 \mathrm{~kcal}$.
(III) Variation of $\log \mathrm{K}$ with $1 / \mathrm{T}$ is linear.
Select the correct statement.

If the initial concentration of reactants are doubled half life becomes half. Then order of the reaction will be

Calculate the overall order of a reaction which has the rate expression

(a) Rate $=k[\mathrm{~A}]^{1 / 2}[{~B}]^{3 / 2}$

(b) Rate $=k[\mathrm{~A}]^{3 / 2}[{~B}]^{-1}$

For the elementary reaction $2 \mathrm{NO}+\mathrm{O}_2 \rightarrow 2 \mathrm{NO}_2,$ the volume of a container is tripled. The rate becomes

The rate for the reaction, $RCl + NaOH\left( {aq} \right) \to ROH + NaCl$ is given by $rate\mathrm{ } = K_1\left[ {RCl} \right].$ The rate of the reaction is

The given reaction,

$2\mathrm{FeC}{\mathrm{l}_3} + \mathrm{SnC}{\mathrm{l}_2} \to \mathrm{SnC}{\mathrm{l}_4} + 2\mathrm{FeC}{\mathrm{l}_2}$ is an example of:

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:

During a particular reaction $20 \%$ of the reactant decomposes in $1 \mathrm{~h},\,40 \%$ in $2 \mathrm{~h}, 60 \%$ in $3 \mathrm{~h}$ and so on. The unit of rate constant is

Which of the following is an incorrect statement about first-order reaction?

In Arrhenius equation $K = A\;{e^{ - {E_a}/RT}}$, the quantity $- {E_a}/RT$ is referred as:

In Arrhenius equation, the fraction of effective collisions is given by

When two reactants $A$ and $B$ are mixed to give products $C$ and $D$, the reaction quotient $Q$ at the initial stage of the reaction is best described by-