Please explain how you got your answer, thanks! N2O5 decomposes according to fir
ID: 787178 • Letter: P
Question
Please explain how you got your answer, thanks!
N2O5 decomposes according to first-order kinetics: 2N2O5(g) rightarrow 4NO2(g) + O2(g) At a certain temperature 20.0% of the initial N2O5decomposes in 2.10 h. Determine the rate constant. What fraction of the initial N2O5 will remain after 13.0 h? What is the half-life? If the initial concentration of N2O5 was 0.222 M, then what concentration remain after 24 h? a. rate constant (h-1) = b. [N2O5] (M) after 13 h = c. half-life (h) = d. [N2O5] (M) after 24 h = A.6.54 B.0.106 C.0.0174 D.0.252Explanation / Answer
1)
as it is a1st order
K =( 2.303/t)log(initial/final)
K = (2.303/2.1)log(100/100-20)
K =0.106 h^-1
2)
0.106 = (2.303/13)log(100/final)
final = 25.23
100-x = 25.23
x =74.77% completed
c) t 1/2 =0.693/k
t1/2 = 0.693/0.106
=6.53 h
d)
0.106 = 2.303/24log(100/100-x)
100-x =7.867
x = 92.14