We recently did a lab testing the reaction between KMnO 4 , H 2 C 2 O 4 and H 2

ID: 1032794 • Letter: W

Question

We recently did a lab testing the reaction between KMnO4, H2C2O4 and H2O. These were the reactions:

These were the times (in minutes) recorded idnetifying a color change:

Exp. 1: trial 1 3:15, trial 2 3:43

Exp. 2: trial 1 4:28, trial 2 4:43

Exp. 3: trial 1 6:30, trial 2 6:47

We are asked to determine:

1) The order of the reaction with respect to [KMnO4].

2) The order of the reaction with respect to [H2C2O4].

3) The overall order of the reaction.

4) The rate constant.

5) The rate of the reaction if you were to mix

30mL of H2C2O4

15mL of KMnO4

5mL of H2O

KMnO4
~0.02M H2C2O4
~0.5M H2O Experiment 1 10.0mL 20.0mL 0.0mL Experiment 2 5.00mL 20.0mL 5.0mL Experiment 3 10.0mL 10.0mL 10.0mL

Rate of reaction

From the given data,

1) Experiment 1 and 2, [H2C2O4] is constant and KMnO4 is halved, no change in rate of reaction observed,

order with respect to KMnO4 = 0

2) Experiment 1 and 3, [KMnO4] is constant and H2C2O4 is halved, the rate of reaction is doubled,

order with respect to H2C2O4 = inverse relation

3) Overall rate law becomes,

rate = k/[H2C2O4]

4) rate constant k = 3.3 x 5 = 16.5 M^2/s

5) rate when,

[H2C2O4] = 30/50 = 0.6

rate = 3.3/0.6 = 5.5 M/s

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