Question

Ethylene oxide, `C_2H_4O` decomposes when heated to give methane and carbon monoxide according to the reaction: `C_2H_4O_(g)` `rarr` `CH_4(g)` + `CO_(g)`. The following kinetic data were observed for the reaction at 688 K. (data below?)

Find the rate law and the value of the rate constant for this reaction.
Thank you in advance. :)

Experiment no. 1
Initial Concentration of `C_2H_4O` is 0.00272 M
Initial Rate is 5.57 x `10^-7` M/s
Experiment no. 2
Initial Concentration of `C_2H_4O` is 0.00544 M
Initial Rate is 1.11 x `10^-6` M/s

Answer 1

R= `2.04*10^-4 1/s`[C₂H₄O]

Explanation:

If the initial concentration of the rate constant is doubled, and it almost doubles the initial rate of the reaction, then the reaction is first order in respect to that reactant. And since this reaction only has one reactant, this reaction has an overall order of 1.

To find K
`5.57*10^-7M/s/ (.00272 M)= k`
`k =2.04*10^-4 1/s`