$\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{3}\left(\mathrm{NO}_{2}\right)_{3}\right]$
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$S + HNO_3 \rightarrow H_2SO_4 + 6NO_2 + 2H_2O$
| $S.NO.$ | $[A]$ $mol.L^{-1}$ | $[B]$ $mol.L^{-1}$ | $Rate$ $mol.L^{-1}\,sec^{-1}$ |
| $I$ | $1 \times 10^{-2}$ | $2 \times 10^{-2}$ | $2 \times 10^{-4}$ |
| $II$ | $2 \times 10^{-2}$ | $2 \times 10^{-2}$ | $4 \times 10^{-4}$ |
| $III$ | $2 \times 10^{-2}$ | $4 \times 10^{-2}$ | $8 \times 10^{-4}$ |
Which of the following are correct statements -
$(a)$ Rate constant of the reaction $10^{-4}$
$(b)$ Rate law of the reaction is $k[A][B]$
$(c)$ Rate of reaction increases four times on doubling the concentration of both the reactant