Oxalic acid. H_2C_2O_4, is oxidized by permanganate ion to CO_2 and H_2O 2MnO_4(

Question

Oxalic acid. H_2C_2O_4, is oxidized by permanganate ion to CO_2 and H_2O 2MnO_4(aq) + 5H_2C_2O_2(aq) + 6H^+(aq) Rightarrow 2Mn^2+ (aq) + 10CO_2(g) + 8H_2O(I) The Rate law is Rate = k [MnO_4] [H_2C_2O_4] What is the order with respect to each reactant? What is the overall order? One proposed mechanism for the decomposition of N_2O_5 to NO_2 is shown below. What is the rate law for the overall reaction based on the proposed mechanism? Ethylene oxide, C_2H_4O, decomposes when heated to give methane and carbon monoxide C_2 H_4O_(g) rightarrow CH_4(g) + CO_(g) The following kinetic data were observed for the reaction at 688K Find the Rate law and the value of the rate constant for this reaction

Explanation / Answer

1.

the order with respect to each reactants, must be in the rate of reaction

with respect o MnO4- --> first orders since it is powered to the 1st

with respect toH2C2O4 --> first orders since it is powered to the 1st

overall order = a+b = 1+1 = 2

it must be second order with respect to all reaction

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