JEE CHEMISTRY MCQ: CHEMICAL KINETICS

1 Medium

1 of 1

Application +4 | -1

The first order rate constant for the decomposition of ethyl iodide by the reaction

{C_2}{H_5}I\left( g \right) \to {C_2}{H_4}\left( g \right) + HI\left( g \right)

at 600 K is

1.60 \times {10^{ - 5}}\,\,{s^{ - 1}}.

Its energy of activation is 209 kJ/mol, T the rate constant of the reaction at 700 K is.

View answer and explanation

Correct option: B

6.36 \times {10^{ - 3}}\,\,{s^{ - 1}}

Option B (

6.36 \times {10^{ - 3}}\,{s^{ - 1}}

) is correct because it is calculated using the Arrhenius equation relating rate constants at different temperatures.

More Questions from CHEMICAL KINETICS

Practice All Chapter MCQs →

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

\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}

k

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

C_0 \sqrt{T}

C_0

T

100 \mathrm{~kJ/mol}.

75 \%

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

27^{\circ} \mathrm{C}

2.303 \times 8.314=19.147