. The following initial rate data were found for the reaction Mno Jo HC 1 x 103

Question

. The following initial rate data were found for the reaction Mno Jo HC 1 x 103 1x 10 2 x 103 1x10- 2 x 103 2 x10-3 2 x 103 2 x 103 'lo Initial Rate (M/s) 1.0 1.0 1.0 2.0 2 x 104 8×10 4 1.6 × 10-3 1.6 x 10-3 Write the rate law for this reaction. Calculate k, remember to include unit. (8 points) 15. One possible mechanism for the gas phase reaction of hydrogen with nitrogen monoxide is step 1 slow: H2(g) + 2 NO(g) N2O(g) + H2O(g) step 2 fast: N20(g)+Hz(g)N2(g)+H20(g) (6 points) a.) What is the equation for the overall reaction? Use the smallest integer coefficients possible b.) Which species acts as a reaction intermediate? c.) Write the rate law for the overall reaction that is consistent with this mechanism

Explanation / Answer

14.

General rate law expression is,

r = k[MnO4-]x[H2C2O4]y[H+]z ----------> (A)

do (2) / (1)

8 * 10-4 / (2 * 10-4) = [2 * 10-3 / (1 * 10-3)]x

4 = 2x

22 = 2x

x = 2

So, Order with respect to MnO4- = 2

Now, do (3) / (2)

1.6 * 10-3 / (8 * 10-4) = [2 * 10-3 / (1 * 10-3)]y

2 = 2y

y = 1

So, the order with respect to H2C2O4 = 1

Now, do (4) / (3)

1.6 * 10-3 / (1.6 * 10-3) = (2.0 / 1.0)z

1 = 2z

20 = 2z

z = 1

So, order with respect to H+ = 0

Therefore,

Rate law expression can be written as,

r = k[MnO4-]2[H2C2O4]1

So, Over all order of reaction = 2 + 1 = 3

From (1)

2 * 10-4 = k (1*10-3) * ( 1*10-3)

k = 2 * 102 L2/mol2.s

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