JEE CHEMISTRY MCQ: CHEMICAL KINETICS

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The half-life for the first-order decomposition of nitramide

\mathrm{NH}_4 \mathrm{NO}_2(\mathrm{aq}) \rightarrow \mathrm{N}_2 \mathrm{O}(\mathrm{g})+\mathrm{H}_2 \mathrm{O}({l})

is 123 minutes at

27^{\circ} \mathrm{C}

. If

200 \mathrm{~ml}

0.02 \mathrm{~M}

\mathrm{NH}_4 \mathrm{NO}_2

solution is allowed to decompose, then how long must the reaction proceed to produce

49.26 \mathrm{~ml}

of 'wet'

\mathrm{N}_2 \mathrm{O}(\mathrm{g})

measured at

27^{\circ} \mathrm{C}

and

785 \mathrm{~mm} \mathrm{~Hg}?

The vapour pressure of water at

27^{\circ} \mathrm{C}

25 \mathrm{~mm} \mathrm{~Hg}

View answer and explanation

Correct option: A

123 \mathrm{~min}

Option A (123 min) is correct because the reaction proceeds for one half-life to produce the given amount of N₂O.

More Questions from CHEMICAL KINETICS

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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