Answer:
The order of the reaction is 1.
Explanation:
[tex]N_2O_5(g)\rightarrow NO_3(g)+NO_2(g)[/tex]
The rate law of the reaction ;
[tex]R=k[N_2O_5]^x[/tex]
The rate of the reaction from T = 0 s to 25 s, [tex][N_2O_5]=1.000 M[/tex] to [tex][N_2O_5]=0.822 M[/tex] respectively.
[tex]R=-\frac{0.822 M-1.000 M}{25s-0 s}=0.00712 M/s[/tex]
[tex]0.00712 M/s=k[0.822 M]^x[/tex] ..[1]
The rate of the reaction from T = 25 s to 50 s, [tex][N_2O_5]=0.822 M[/tex] to [tex][N_2O_5]=0.677 M[/tex] respectively.
[tex]R=-\frac{0.677 M-0.822 M}{50s-25 s}=0.0058 M/s[/tex]
[tex]0.00646 M/s=k[0.677 M]^x[/tex] ..[2]
[1] ÷ [2]
[tex]\frac{0.00712 M/s}{0.0058 M/s}=\frac{k[0.822 M]^x}{k[0.677 M]^x}[/tex]
Solving for x:
x = 1.05 ≈ 1
The rate law of the reaction ;
[tex]R=k[N_2O_5]^1[/tex]
The order of the reaction is 1.
