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?
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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.
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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
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