Asked by Freddy
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.
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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Answered by
Freddy
some one help please!
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