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| $S.NO.$ | $[A]$ $mol.L^{-1}$ | $[B]$ $mol.L^{-1}$ | $Rate$ $mol.L^{-1}\,sec^{-1}$ |
| $I$ | $1 \times 10^{-2}$ | $2 \times 10^{-2}$ | $2 \times 10^{-4}$ |
| $II$ | $2 \times 10^{-2}$ | $2 \times 10^{-2}$ | $4 \times 10^{-4}$ |
| $III$ | $2 \times 10^{-2}$ | $4 \times 10^{-2}$ | $8 \times 10^{-4}$ |
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
$Hb{O_2} + {H_3}{O^ + }C{O_2} \rightleftharpoons \left( {{H^ + } - Hb - C{O_2}} \right) + {O_2} + {H_2}O$
Release of $O_2$ is favoured when there is
$\left( I \right)A + {e^ - } \to {A^\circleddash }\,\,\,\,\,\,{E^o} = + 0.24\,V$
$\left( {II} \right){B^ - } + {e^ - } \to {B^{ - 2}}\,\,\,\,\,\,{E^o} = + 1.25\,V$
$\left( {III} \right){C^ - } + 2{e^ - } \to {C^{ - 3}}\,\,\,\,\,\,{E^o} = + 0.15\,V$
$\left( {IV} \right)D + 2{e^ - } \to {D^{ - 2}}\,\,\,\,\,\,{E^o} = + 0.68\,V$