The reaction: C2H5Cl(g) rightarrow C2H4(g) + HCl(g) is first order in C2H5CI. Th

Question

The reaction: C2H5Cl(g) rightarrow C2H4(g) + HCl(g) is first order in C2H5CI. The rate constant is 1.60xl0'6 s'1 for the reaction conducted at 650. K. In an investigation into the decomposition of C;H;Cl(g). an initial concentration of 0.165 M was used, a) What will be the concentration of C;H;Cl(g) after 125 hours? b) How long will it take for the concentration of C2H5CI to drop to 0.100 M? c) How many hours will it take for 75.0% of the C;H;C1 to decompose? d) Determine the half-life, in hours, for this reaction at 650. K.

Explanation / Answer

Let initial conc = A

conc. at time t = a)

a)

kt = ln (A/a)

1.6 * 10^(-6) * 125 * 2600 = ln (0.165 / a)

a = 0.0803 M

b)

1.6 * 10^(-6) * t = ln(0.165/0.1)

t = 86.94 hours or 85hr and 56 min

c)

for 75% decomposition a = A/4

1.6 * 10^(-6) * t = ln(1/4)

t = 240.6 hr or 240hr and 36min

d)

halg-life = ln(2) / k

= ln(2) / (1.6 * 10^(-6))

= 120.33hrs or 120hr and 20 min

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