Question

Using the data in the table, calculate the rate constant of this reaction.

A+B⟶C+DA+B⟶C+D

Trial	[?] (?)[A] (M)	[?] (?)[B] (M)	Rate (M/s)
1	0.290	0.240	0.0197
2	0.290	0.528	0.0953
3	0.522	0.240	0.0355

?=

Units=

Answer 1

From trials 1 and 2

[A] is kept constant at 0.290 M and [B] is increased from 0.240 M to 0.528 M. The rate increases from 0.0197 M to 0.0953 M

For trial 1

......(1)

For trial 2

......(2)

Divide equation (2) with equation (1)

Take natural logarithm on both sides

The order of reaction with respect to B is 2.

From trials 1 and 3

[B] is kept constant at 0.240 M and [A] is increased from 0.290 M to 0.522 M. The rate increases from 0.0197 M to 0.0355 M

For trial 1

......(1)

For trial 3

......(2)

Divide equation (3) with equation (1)

Take natural logarithm on both sides

The order of reaction with respect to A is 1.

The rate law expression is

Substitute values for trial 1

The rate constant