Question

In: Chemistry

The reaction:    2NO (g)   +   2H2 (g)       N2 (g)   +   2H2O (g) a. Determine the rate...

The reaction:    2NO (g)   +   2H2 (g)       N2 (g)   +   2H2O (g)

a. Determine the rate order for the reaction.

b. Write a rate law, including the value for k.

[NO] [H2] Rate M/s0.

420 0.122 0.136

0.210 0.122 0.0339

0.210 0.244 0.0678

0.105 0.488 0.0339

Solutions

Expert Solution

Let the rate law be,

Rate law = k[NO]x[H2]y

From the table,

0.136 = k[0.420]x[0.122]y .....(1)

0.0339 = k[0.210]x[0.122]y.....(2)

0.0678 = k[0.210]x[0.244]y ......(3)

Dividing eq1 by eq2 we get,

0.136/0.0339 = [0.420/0.210]x

4.0 = [2]x

[2]2=[2]x

x = 2

Now dividing eq3 by eq2, we get

0.0678/0.0339 = [0.244/0.122]y

2 = [2]y

[2]1 = [2]y

y = 1

So, order of the reaction is x+y = 2+1 = 3

Rate law = k[NO]2[H2]1

Lets find out the value of k,

From eq1,

k = 0.136/[0.420]2[0.122]1

= 0.136/0.0215

= 6.30

From eq2,

k = 0.0339/[0.210]2[0.122]1

= 0.0339/0.00538

= 6.30

From eq 3,

k = 0.0678/[0.210]2[0.244]1

= 0.0678/0.01076

= 6.30

Thus, k = 6.30

Hence rate law,

Rate = 6.30[NO]2[H2]1

queen_honey_blossom answered 2 years ago
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