Question

check my work Determine the rate law and the value of k for the following reaction using the data provided.

2 N2O5(g) → 4 NO2(g) + O2(g) [ N2O5]i (M) Initial Rate (M-1s-1)
0.093 4.84 x 10-4
0.084 4.37 x 10-4
0.224 1.16 x 10-3

A) Rate = 5.6 × 10-2 M-1s-1[N2O5]2
B) Rate = 6.0 × 10-1 M-2s-1[N2O5]3
C) Rate = 1.6 × 10-3 M1/2s-1[N2O5]1/2
D) Rate = 1.7 × 10-2 M-1/2s-1[N2O5]3/2
E) Rate = 5.2 × 10⁻3 s-1[N2O5]
Answer: E

Answer 1

the rate equal rate=k[a]

rate=k[N2O5]^2
(4.84*10^-4)=k(0.093)
divide by .093

5.6*10^-2 = k

the units for k

m/s=k(m)^2
m/s * 1/m^2
k= m^-1s^-1

k= 5.6*10^-2 m^-1s^-1

what did i do wrong to not get E

Answer 2

i think it is just an error

Answer 3

@Preetha

Answer 4

@mayankdevnani

Answer 5

@abb0t