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The following initial rate data are for the reduction of nitric oxide with hydrogen
2 NO 211N, 211,0
Experiment
1
INO).M
0,475
IM
0.411
mit Rate, M.
0.144
0.575
0.000
0.478
0.000
0,822
0.822
0.217
1.IS
1
Complete the rate law for this reaction in the box below
Use the form KIA"", where 'T' is understood for morn and concentrations taken to the zero power do not appear. Don't enter for morn
Rate
From these data, the rate constant is
m?!
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Answer 1

1.553 M^2s^-1

Step-by-step explanation:

Now let us consider experiments 1,2,3.

In experiment 1 and 2, the concentration of NO is doubled and the initial rate of reaction is quadrupled.

0.575/0.144 = 4

So;

2^2 =4

In experiment 2 and 3

The concentration of reaction of H2 is doubled and the rate of reaction is doubled.

0.575/0.287 = 2

2^1 =2

So we can now write;

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

Taking up the first reaction;

0.144 =k [0.475]^2 [0.411]

k = 0.144/ [0.475]^2 [0.411]

k = 1.553 M^2s^-1