a certain temperature, the half-life of the first order decomposition of cyclohe

Question

a certain temperature, the half-life of the first order decomposition of cyclohexene (shown below) is 1.72 hr.
cyclohexene ? ethene + 1,3-butadiene
Answer the following questions about the decomposition of cyclohexene and report all answers to three significant figures.

1. If the initial concentration of cyclohexene is 8.41×10-2 M, calculate the time (in hr) required for the concentration of cyclohexene to decrease to 63 % of the initial concentration.
2. If the initial concentration of cyclohexene is 8.41×10-2 M, calculate the concentration (in M) after 3.53 hr.
a certain temperature, the half-life of the first order decomposition of cyclohexene (shown below) is 1.72 hr.
cyclohexene ? ethene + 1,3-butadiene
Answer the following questions about the decomposition of cyclohexene and report all answers to three significant figures.

1. If the initial concentration of cyclohexene is 8.41×10-2 M, calculate the time (in hr) required for the concentration of cyclohexene to decrease to 63 % of the initial concentration.
2. If the initial concentration of cyclohexene is 8.41×10-2 M, calculate the concentration (in M) after 3.53 hr.
a certain temperature, the half-life of the first order decomposition of cyclohexene (shown below) is 1.72 hr.
cyclohexene ? ethene + 1,3-butadiene
Answer the following questions about the decomposition of cyclohexene and report all answers to three significant figures.

1. If the initial concentration of cyclohexene is 8.41×10-2 M, calculate the time (in hr) required for the concentration of cyclohexene to decrease to 63 % of the initial concentration.
2. If the initial concentration of cyclohexene is 8.41×10-2 M, calculate the concentration (in M) after 3.53 hr.

Explanation / Answer

1.

a = initial concentration

at = concentration at time t

k = 0.693 / t 1/2

k = 0.693/ 1.72 hour^-1

t = (2.303 log (a / a t ))/ k

put a = a

and at = 0.63 a

t = 1.1469 hours

2.

3.53 = (2.303 log (a/ at)) / k

log (a/at) = 3.53 * k / 2.303

a / at = 4.1454

at = a / 4..1454 = 2.0287 * (10)^ -8 M

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