Question

The reaction ch3-n ≡ c → ch3-c ≡ n is a first-order reaction. at 230.3°c, k = 6.29 ⋅ 10-4s-1. if [ch3 = n≡c] is 1.00 ⋅ 10-3 initially, [ch3 = n≡c] is ________ after 1.000 ⋅ 103 s.

Answer 1

The answer is 5.33 x 10^-4

to find the answer follow these steps:

the reaction is first order reaction

here k = 6.29 x 10^-4 s^-1

initial concentration = 1.00 x 10^-3

After time t = 1.000 x 10^3 s concentration is = ?

So, - 6.29 x 10^-4 x 1.00 x 10^3 + ln (1.00 x 10^-3) = - 7.54 

C = e ^ - 7.54= 5.33 x 10^-4 M

Answer 2

Answer:Concentration of [$CH_3=N\equiv C] after [tex]1.000\times 10^3 s$ is $2.38\times 10^{-8} mol/L$.

Explanation:

Rate constant of the reaction = k = $6.29\times 10^{-4} s^{-1}$

Initial concentration of $[A_o]=1.00\times 10^{-3} mol/L$

Concentration after time t= [A]

$t = 1.000\times 10^3 s$

$log[A]=2.303\times \log[A_o]-kt$

$log[A]=2.303\times \log[1.00\times 10^{-3}]-6.29\times 10^{-4} s^{-1}\times 1.000\times 10^3 s$

$[A]=2.38\times 10^{-8} mol/L$

Concentration of [$CH_3=N\equiv C] after [tex]1.000\times 10^3 s$ is $2.38\times 10^{-8} mol/L$.