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Select the rate law that corresponds to the data shown for the following reaction :
\begin{tabular}{cllc}
\multicolumn{4}{l}{\( \mathrm{A}+\mathrm{B} \longrightarrow \mathrm{C} \)} \\
\hline Expt. No. & \( (A) \) & \( ( \) B) & Initial Rate \\
\hline 1 & \( 0.012 \) & \( 0.035 \) & \( 0.10 \) \\
\hline 2 & \( 0.024 \) & \( 0.070 \) & \( 0.80 \) \\
\hline 3 & \( 0.024 \) & \( 0.035 \) & \( 0.10 \) \\
\hline 4 & \( 0.012 \) & \( 0.070 \) & \( 0.80 \) \\
\hline
\end{tabular}
(a) Rate \( =k[B]^{3} \)
(b) Rate \( =\mathrm{k}[\mathrm{B}]^{4} \)
(c) Rate \( =\mathrm{k}[\mathrm{A}][\mathrm{B}]^{3} \)
(d) Rate \( =\mathrm{k}[\mathrm{A}]^{2}[\mathrm{~B}]^{2} \)
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