A zero-order reaction has a constant rate of 3.20×10−4M/s. If after 45.0 seconds the concentration has dropped to 3.50×10−2M, what was the initial concentration?
K =1/t * [A0]-[A]
K = 3.2*10^-4 M = 0.00032M
[A] = 3.5*10^-2M = 0.035M
t = 45second
K =1/t * [A0]-[A]
K* t = [A0]-[A]
0.00032*45 = [A0]-0.035
0.0144 =[A0] -0.035
[A0] = 0.0144+0.035
[A0] = 0.0494M
initial conc is 0.0494M
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