JEE CHEMISTRY MCQ: CHEMICAL KINETICS

1 Easy

1 of 1

Application +4 | -1

For a reaction

aA \to bB

when

\left[ A \right] = 2.2\;\mathrm{m}\;\mathrm{M},

the rate was found to be

2.4\;\mathrm{m}\;\mathrm{M}{\mathrm{s}^{ - 1}}.

On reducing concentration of

\left[ A \right]

to half, the rate changes to

0.6\;\mathrm{m}\;\mathrm{M}{\mathrm{s}^{ - 1}}.

The order of reaction with respect to

A

is:

View answer and explanation

Correct option: B

Option B (2) is correct because the rate equation is of the form

r = k[A]^n

, and solving for n using the given data yields n = 2.

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\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