chemistry

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The decomposition of N2O5 proceeds according to the following equation
2 N2O5(g) → 4 NO2(g) + O2(g).
The rate constant, k, for the reaction at 298 K is 2.20 x 10-3 min-1. If a reaction is set up in a vessel at 298 K, with an initial concentration of 0.343 mol L-1; what is the concentration of reactant N2O5(g) in mol/L after 42 minutes?

• chemistry -

The units of min^-1 tell you that the reaction is first order.
So ln(No/N) = kt.
No is starting.
N is end
k from problem
t = 42 min

• chemistry -

298/0.343 = 868

868/42 = 21.000

• chemistry -

Nope. You didn't substitute. And you know the answer can't be right. You start with 0.343 mol, it decomposes and you have more than you started with after 43 mn. I don't think so.

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