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The first-order decomposition of N2O at a fixed temperature has a rate constant of 0.385 s-1....

The first-order decomposition of N2O at a fixed temperature has a rate constant of 0.385 s-1. If the initial concentration of N2O is 21.4 M, what is the concentration of N2O after 50 s?

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Answer #1

[A0]   = 21.4M

t   = 50s

K   = 0.385s^-1

K    = 2.303/t log[A0]/[A]

0.385 = 2.303/50 log21.4/[A]

log21.4/[A]    = 0.385*50/2.303

log21.4/[A]       = 8.3586

21.4/[A]          = 10^8.3586

21.4/[A]           = 228349465.8

[A]                 = 21.4/228349465.8   = 9.37*10^-8 M

The concentration of N2O after 9.37*10^-8 M

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