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Compounds 'A' and 'B' react according to the following chemical equation.
\[
\mathrm{A}(\mathrm{g})+2 \mathrm{~B}(\mathrm{~g}) \longrightarrow 2 \mathrm{C}(\mathrm{g})
\]
Concentration of either 'A' or ' \( \mathrm{B} \) ' were changed keeping the concentrations of one of the reactants constant and rates were measured as a function of initial concentration. Following results were obtained. Choose the correct option for the rate equations for this reaction.
\begin{tabular}{|c|c|c|c|}
\hline Experiment & \( \begin{array}{l}\text { Initial } \\
\text { concentration } \\
\text { of }[\mathbf{A}] / \mathbf{m o l ~ L}^{-1}\end{array} \) & \( \begin{array}{l}\text { Initial } \\
\text { concentration } \\
\text { of }[B] / \mathbf{m o l ~ L}^{-1}\end{array} \) & \( \begin{array}{l}\text { Initial rate of } \\
\text { formation of } \\
{[\mathbf{C}] / \mathbf{m o l ~ L}^{-1} \mathbf{s}^{-1}}\end{array} \) \\
\hline 1. & \( 0.30 \) & \( 0.30 \) & \( 0.10 \) \\
2. & \( 0.30 \) & \( 0.60 \) & \( 0.40 \) \\
3. & \( 0.60 \) & \( 0.30 \) & \( 0.20 \) \\
\hline
\end{tabular}
(i) Rate \( =k[\mathrm{~A}]^{2}[\mathrm{~B}] \)
(ii) \( \quad \) Rate \( =k[\mathrm{~A}][\mathrm{B}]^{2} \)
(iii) Rate \( =k[\mathrm{~A}][\mathrm{B}] \)
(iv) \( \quad \) Rate \( =k[\mathrm{~A}]^{2}[\mathrm{~B}]^{0} \)
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