At 45oC, its rate constant is 6.22 x 10-4 / s. If the initial concentration of N2O5 in solution is 0.100 mol/L

Question

The rate law for the decomposition of dinitrogen pentoxide, N2O5, into N2O4 and O2 is k [N2O5].

At 45oC, its rate constant is 6.22 x 10-4 / s. If the initial concentration of N2O5 in solution is 0.100 mol/L, how many minutes will it take for the concentration to drop below 0.010 mol/L?

Answer 1

N2O5 -> N2O4 + 1/2 O2

-d[N2O5]/dt=k[N2O5]

k dt = -1/[N2O5] d[N2O5]

integrate both sides

kt= -ln ( [N2O5]initial -[N2O5]final )

t= -ln (0.100 mol/L - 0.010 mol/L) / 6.22 x 10-4 / s

i dont have a calculator on my side and im too lazy to get it haha sorry;P ill leave everything to you here  on.