Question

A certain reaction is second order in N₂  and second order in H₂. Use this information to complete the table below. Round each of your answers to 3 significant digits.

[N2]	[H2]	initial rate of reaction
0.311 M	2.02 M	5.00 x 104M/s
0.311 M	9.15 M	_________M/s
0.884 M	0.710 M	__________M/s

Answer 1

Given,

[N₂] = 0.311 M

[H₂] = 2.02 M

initial rate = 5 * 10⁴ M/s

The reaction is of second order with each of the reactant, so

rate = k[N₂]²[H₂]²

(5 * 10⁴ M/s) = k (0.311 M)² (2.02 M)²

k = (5 * 10⁴) / 0.3946

k = 12.67 * 10⁴ M^-3s^-1

Given,

[N₂] = 0.311 M

[H₂] = 9.15 M

k = 12.67 * 10⁴ M^-3s^-1

rate = k[N₂]²[H₂]²

rate = 12.67 * 10⁴ * (0.311)² (9.15)²

= 1.026 * 10⁶ M/s

Given,

[N₂] = 0.884 M

[H₂] = 0.710 M

k = 12.67 * 10⁴ M^-3s^-1

Now,

rate = k[N₂]²[H₂]²

rate = 12.67 * 10⁴ * (0.884)² * (0.710)²

= 4.99 * 10⁴ M/s

The table is,

[N2]	[H2]	Initial rate of reaction
0.311 M	2.02 M	5.00 * 104 M/s
0.311 M	9.15 M	1.026 * 106 M/s
0.884 M	0.710 M	4.99 * 104 M/s