Ethyl chloride vapor decomposes by the first-order reaction C2H5ClC2H4+HCl The a

Question

Ethyl chloride vapor decomposes by the first-order reaction
C2H5ClC2H4+HCl
The activation energy is 249 kJ/mol and the frequency factor is 1.6×1014s1.

Part A: Find the value of the specific rate constant at 710 K .Express your answer using two significant figures.

Part B: Find the fraction of the ethyl chloride that decomposes in 18 minutes at this temperature. Express your answer using one significant figure.

Part C:Find the temperature at which the rate of the reaction would be twice as fast. Express your answer using two significant figures.

Explanation / Answer

(A)

Ea = 249 kJ/mol

A = 1.6 x 10^14 s^-1

arrhenius equation

K = A e^-Ea / RT

K = (1.6 x 10^14) x e^- 249 / (8.314 x 10^-3) x710

K = 7.7 x 10^-5 s-1

specific rate constant = 7.7 x 10^-5 s-1

(B)

k = 1 /t * ln (Ao/A)

7.7 x 10^-5 = (1/ 18 x 60 ) * ln (Ao / A)

0.083 = ln (Ao / A)

Ao / A = 1.1

fraction = A / Ao = 1/1.1 = 0.92

92 % ethyl cholride decomposed

part C)

at temperature = 720K rate constant becomes twice.

for every change in temperature 10 K rate constant becomes twice

Related Questions

Navigate

• Browse (All)
• Browse E
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.