Consider the reaction $$\left[ \mathrm { Fe } ( \mathrm { CN } ) _ { 6 } \right] ^ { 4 - } \underset { k _ { - 1 } } { \longleftarrow } \left[ \mathrm { Fe } ( \mathrm { CN } ) _ { 6 } \right] ^ { 3 - } + e ^ { - }$$
The net reaction rate is given by
A) $$k _ { 1 } \left[ F e ^ { 2 + } \right]$$
B) $$k _ { 1 } \left[ F e ^ { 2 + } \right] - k _ { - 1 } \left[ F e ^ { 3 + } \right]$$
C) $$k _ { 1 } \left[ F e ^ { 2 + } \right] + k _ { - 1 } \left[ F e ^ { 3 + } \right]$$
D) none of the above

Question

Consider the reaction $$\left[ \mathrm { Fe } ( \mathrm { CN } ) _ { 6 } \right] ^ { 4 - } \underset { k _ { - 1 } } { \longleftarrow } \left[ \mathrm { Fe } ( \mathrm { CN } ) _ { 6 } \right] ^ { 3 - } + e ^ { - }$$ 
 The net reaction rate is given by
A) $$k _ { 1 } \left[ F e ^ { 2 + } \right]$$
B) $$k _ { 1 } \left[ F e ^ { 2 + } \right] - k _ { - 1 } \left[ F e ^ { 3 + } \right]$$
C) $$k _ { 1 } \left[ F e ^ { 2 + } \right] + k _ { - 1 } \left[ F e ^ { 3 + } \right]$$
D) none of the above

Quizplus · Accepted Answer

The net reaction rate is the difference between the forward and reverse reaction rates. The forward reaction rate is given by k1[Fe2+], and the reverse reaction rate is given by k-1[Fe3+]. Therefore, the net reaction rate is given by k1[Fe2+] - k-1[Fe3+].

Consider the Reaction The Net Reaction Rate Is Given by A)

Consider the Reaction The Net Reaction Rate Is Given by
A)