Question

Consider the reaction A+B⟶C . The rate of reaction is 1.23*10-4. [A] will go from a 0.4321 M to a 0.4444 M concentration in what length of time?

Answer 1

The initial concentration of A was reduced from 2M to 1M in 1 hr.

Thus, the concentration is reduced to half and the time is half life period. It is equal to 1 hr.

The concentration of A was reduced from 1M to 0.25M in 2 hours.

Thus, the concentration is reduced to one fourth and the time is two half life periods. It is equal to 2 hrs. Thus, half life is 1 hr.

Hence, the half life is independent of the concentration.

Hence, the reaction is of first order.

Answer 2

Answer:

100 seconds

Explanation:

r =1.23 * 10^-4

delta A = 0.4321 - 0.4444 = -0.0123

r = -delta A/t

1/t = -r/delta A = 1.23 *10^-4 / 1.23 * 10^-2

t = 100 seconds