Answer:
The order of the reaction is zero and the rate constant 0.018 M/s.
Explanation:
[tex]C_2H_5I(g)\rightarrow C_2H_4(g) + HI(g)[/tex]
The order of the reaction be = x
The rate law of the reaction ;
[tex]R=k[C_2H_5I]^x[/tex]
1. Rate of the reaction when concentration changes from 2.00 M to 1.73 M in interval of 0.0 minutes to 15.0 minutes.
[tex]R=-\frac{1.73M-2.00M}{15.0 min-0.0min}=0.018 M/min[/tex]
[tex]0.018 M/min=k[1.73 M]^x[/tex]..[1]
2. Rate of the reaction when concentration changes from 2.00 M to 1.73 M in interval of 15.0 minutes to 30.0 minutes.
[tex]R=-\frac{1.46 M-1.73M}{30.0 min- 15.0 min}=0.018 M/min[/tex]
[tex]0.018 M/min=k[1.46 ]^x[/tex]...[2]
[1] ÷ [2]
[tex]\frac{0.018 M/min}{0.018 M/min}=\frac{k[1.73 M]^x}{k[1.46 M]^x}[/tex]
x = 0
The order of the reaction 0.
The rate law of the reaction ;
[tex]R=k[C_2H_5I]^0[/tex]
[tex]0.018 M/min=k[1.73 M]^0[/tex]
[tex]k=0.018 M/min[/tex]
The order of the reaction is zero and the rate constant 0.018 M/s.
