Answer: [tex]rate=k[UO_2^+]^2[H^+][/tex]
Explanation:
Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.
The balanced chemical reaction is:
[tex]2UO_2^+4H^+\rightarrow U^{4+}+UO_2^{2+}+2H_2O[/tex]
[tex]rate=k[UO_2^+]^n[H^+]^m[/tex]
where k = rate constant
n = order with respect to [tex]UO_2^+[/tex] = 2
m = order with respect to [tex]H^+[/tex] = ?
n+ m = 3
2+ m = 3
m = 1
Thus m = order with respect to [tex]H^+[/tex] = 1
[tex]rate=k[UO_2^+]^2[H^+]^1[/tex]
