The first-order decomposition of N2O5 at 328 K has a rate constant of 1.70 × 10-3...

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The first-order decomposition of N2O5 at 328 K has a rate constant of 1.70 × 10-3...

The first-order decomposition of N2O5 at 328 K has a rate constant of 1.70 × 10-3 s-1. If the initial concentration of N2O5 is 2.88 M, what is the concentration of N2O5 after 12.5 minutes?

This is what I did:

k = 1.70 x 10^.3

Ao= 2.88M

t = 12.5 min

Af= ???

I used the equation [Af]= -Kt + ln [Ao] (this equals .0359) which is wrong. What did I do wrong?

science chemistry

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The first-order decomposition of N2O5 at 328 K has a rate constant of 1.70 × 10-3...

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