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The kinetic data for the given reaction \( A(g)+2 B(g) \stackrel{k}{\longrightarrow} C(g) \) is provided in the following table for three experiments at \( 300 \mathrm{~K} \)
\begin{tabular}{|c|c|c|c|}
\hline Ex. No. & {\( [\boldsymbol{A} / \boldsymbol{M}] \)} & {\( [\boldsymbol{B} / \boldsymbol{M}] \)} & Initial rate \( \left(\boldsymbol{M} \mathbf{~ s e c}^{-\mathbf{1}}\right) \) \\
1. & \( 0.01 \) & \( 0.01 \) & \( 6.930 \times 10^{-6} \) \\
2. & \( 0.02 \) & \( 0.01 \) & \( 1.386 \times 10^{-5} \) \\
3. & \( 0.02 \) & \( 0.02 \) & \( 1.386 \times 10^{-5} \) \\
\hline
\end{tabular}
In another experiment starting with initial concentration of \( 0.5 \) and \( 1 M \) respectively for \( A \) and \( B \) at \( 300 \mathrm{~K} \), find the rate of reaction after 50 minutes from the starting of experiment (in \( M / \mathrm{sec}) \)
(a) \( 6.93 \times 10^{-4} \)
(b) \( 0.25 \times 10^{-7} \)
(c) \( 4.33 \times 10^{-5} \)
(d) \( 3.46 \times 10^{-4} \)
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