The rate constant $(K)$ for the reaction $2A + B \to product $ was found to be $2.5 \times {10^{ - 5}}\;{\rm{litre}}\;{\rm{mo}}{{\rm{l}}^{ - 1}}\;{\sec ^{ - 1}}\;\;after\;\;15\sec ,\;2.60 \times {10^{ - 5}}\;{\rm{litre}}\;{\rm{mo}}{{\rm{l}}^{ - 1}}\;{\sec ^{ - 1}}\;{\rm{after}}\;\;30\sec $ and $2.55 \times {10^{ - 5}}\;{\rm{litre}}\;{\rm{mo}}{{\rm{l}}^{ - 1}}\;{\sec ^{ - 1}}\;{\rm{after}}\;\;50\;{\rm{sec}}{\rm{.}}$ The order of reaction is:

JEE CHEMISTRY MCQ: CHEMICAL KINETICS

1 Easy

1 of 1

Analyzing +4 | -1

The rate constant

(K)

for the reaction

2A + B \to product

  was found to be

2.5 \times {10^{ - 5}}\;\mathrm{litre}\;\mathrm{mo}{\mathrm{l}^{ - 1}}\;{\sec ^{ - 1}}\;\;after\;\;15\sec ,\;2.60 \times {10^{ - 5}}\;\mathrm{litre}\;\mathrm{mo}{\mathrm{l}^{ - 1}}\;{\sec ^{ - 1}}\;\mathrm{after}\;\;30\sec

and

2.55 \times {10^{ - 5}}\;\mathrm{litre}\;\mathrm{mo}{\mathrm{l}^{ - 1}}\;{\sec ^{ - 1}}\;\mathrm{after}\;\;50\;\mathrm{sec}\mathrm{.}

The order of reaction is:

View answer and explanation

Correct option: A

Option A (2) is correct because the rate constant K remains approximately constant over time, and the units of K (litre mol^-1 sec^-1) indicate a second-order reaction.

More Questions from CHEMICAL KINETICS

Practice All Chapter MCQs →

The reaction

\mathrm{A}_2+\mathrm{B}_2 \rightarrow 2 \mathrm{AB}

follows the mechanism

\begin{aligned} & {{\text{A}}_2}\mathop \rightleftharpoons \limits_{{{\text{k}}_{ - 1}}}^{{{\text{k}}_1}} {\text{A}} + {\text{A (fast) }} \\ & \mathrm{A}+\mathrm{B}_2 \xrightarrow{\mathrm{k}_2} \mathrm{AB}+\mathrm{B} \text { (slow) } \\ & \mathrm{A}+\mathrm{B} \rightarrow \mathrm{AB} \text { (fast) } \end{aligned}

The overall order of the reaction is: For the first order reaction with the rate constant

k

, which expression gives the rate half-life period?

(Initial\mathrm{ }conc.\mathrm{ } = a)

Which of the following is a zero order reaction? 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? Arrhenius equation is The energy of activation for an uncatalysed reaction is

100 \mathrm{~kJ/mol}.

Presence of a catalyst lowers the energy of activation by

75 \%

. The

\log _{10} \frac{K_2}{K_1}

of the ratio of rate constant of catalysed and uncatalysed reactions at

27^{\circ} \mathrm{C}

is?

Assume the frequency factor is same for both reactions. (Given

2.303 \times 8.314=19.147

)