Because of the changing color of the solution as the following reaction proceeds, the rate law can be determined by measuring the rate of disappearance of the permanganate ion (MnO4-). 2MnO4-(aq)+ 5H2C2O4(aq) + 6H+(aq) -> 2Mn2+(aq) + 10CO2(g) + 8H2O(l)
The following initial rate data was found for the reaction:
[MnO4] (M)= 2.0 x 10^-3
[H2C2O4] (M)= 2.0 x 10^-3
[H+] (M)= 1.0 x 10^-3
The reaction is second order for MnO4, first order for H2C2O4 and zero order for H+. This reaction could also be monitored by measuring the formation of CO2(g). Determine the initial rate of the reaction in terms of appearance of CO2(g) in M/sec given the same conditions as in experiment above.
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some one help please!