Question

Initial-rate data at a certain temperature is given in the table for the reaction c2h5cl(g) ⟶ c2h4(g) + hcl(g) [c2h5cl]0 (m) initial rate (m/s) 0. 100 0. 630 x 10-30 0. 200 1. 26 x 10-30 0. 300 1. 89 x 10-30 determine the value and units of the rate constant.

Answer 1

The value of the rate constant is : 0.63 * 10⁻²⁹ s⁻¹ and The unit of the rate constant is : sec⁻¹

The chemical reaction :

C₂H₅Cl ------> C₂H₄(g) + HCl(g)  

Determine the value and unit of the rate constant ( K )

let the rate of reaction be expressed as

R = k [ C₂H₅Cl ]ⁿ  ---- ( 1 )

where : n = order

             k = rate constant

From the table

2 = 2ⁿ

therefore n = 1

Hence we can rewrite equation ( 1 ) as

R = k [ C₂H₅Cl ] ¹ ( first order reaction )  ---- ( 2 )

Next step : substitute the value of C₂H₅Cl  and initial rate into equation 2

0.630 * 10⁻³⁰ = k ( 0.1 ) ¹ M

Therefore : K = 0.630 * 10⁻²⁹ s⁻¹

Hence we can conclude that The value of the rate constant is : 0.63 * 10⁻²⁹ s⁻¹ and The unit of the rate constant is : sec⁻¹.

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