Because of the changing color of the solution as the following reaction proceeds

Question

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) Experiment# [MnO4-] (M) [H2C2O4](M) [H+] (M) Initial Rate (M/s) 1 1.0x10^-3 1.0x10^-3 1.0x10^-3 2.0x10^-4 2 2.0x10^-3 1.0x10^-3 1.0x10^-3 8.0x10^-4 3 2.0x10^-3 2.0x10^-3 1.0x10^-3 1.6x10^-3 4 2.0x10^-3 2.0x10^-3 2.0x10^-3 1.6x10^-3 his 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 III above. Please provide a step by step work.

Explanation / Answer

initial rate = 1/10 *(d CO2/dt)

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