The concentration of R in the reaction $R \to P$ was measured as a function of time and the following data is obtained $\begin{array}{*{20}{l}} {\left[ R \right]\left( {molar} \right)\;\;\;1.00\;\;\;\;\;\;0.75\;\;\;\;\;0.40\;\;\;\;\;0.10}\\ {t\;\left( {min} \right)\;\;\;\;\;\;\;\;\;0.00\;\;\;\;\;0.05\;\;\;\;\;0.12\;\;\;\;\;0.18} \end{array}\;$ The order of the reaction is

JEE CHEMISTRY MCQ: CHEMICAL KINETICS

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The concentration of R in the reaction

R \to P

was measured as a function of time and the following data is obtained

\begin{array}{llllllllllllllllllll} {\left[ R \right]\left( {molar} \right)\;\;\;1.00\;\;\;\;\;\;0.75\;\;\;\;\;0.40\;\;\;\;\;0.10}\\ {t\;\left( {min} \right)\;\;\;\;\;\;\;\;\;0.00\;\;\;\;\;0.05\;\;\;\;\;0.12\;\;\;\;\;0.18} \end{array}\;

The order of the reaction is

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Correct option: A

Zero

Option A (Zero) is correct because the rate of change of concentration with respect to time is constant, indicating a zero-order reaction.

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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