For a first order reaction, $A \longrightarrow$ products, the initial concentration of $\mathrm{A}$ decrease from $0.1 \mathrm{~M}$ to $0.05 \mathrm{~M}$ in 1 minutes. The initial rate of the reaction (in $\mathrm{M} \mathrm{s}^{-1}$ ) is

JEE CHEMISTRY MCQ: CHEMICAL KINETICS

1 Medium

1 of 1

Application +4 | -1

For a first order reaction,

A \longrightarrow

products, the initial concentration of

\mathrm{A}

decrease from

0.1 \mathrm{~M}

0.05 \mathrm{~M}

in 1 minutes. The initial rate of the reaction (in

\mathrm{M} \mathrm{s}^{-1}

) is

View answer and explanation

Correct option: C

1.15 \times 10^{-3}

Option C (

1.15 \times 10^{-3}

) is correct because the rate of a first-order reaction is directly proportional to the concentration of the reactant, and the rate constant can be calculated from the half-life.

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

)