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The first order constant is 4.82 x 10-3 s-1 at 70C for the decomposition of the...

The first order constant is 4.82 x 10-3 s-1 at 70C for the decomposition of the following reaction: 2N2O5 (g) -> 4NO2 + O2 (g)

Suppose that you start with .0175M of N2O5 (g)

a.) What is the molarity of N2O5 that remains after 15 minutes (note: the rate constant is in seconds)

b.) How many seconds will it take for the quantity of N2O5 to drop to .015M?

c.) What is the half life of N2O5 at 70C?

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Answer #1

a) K = (2.303 /t) log [A] / [A]

[A0] = 0.0175 M , [A] = ?

t = 15 min = 900 s

K = 4.82 x 10-3 s-1

4.82 x 10-3  = (2.303 / 900) log [0.0175] / [A]

1.88 = - 1.76 - log [A]

log [A] = -3.64

[A] = 0.00023 M

b) [A] = 0.015 M , t = ?

4.82 x 10-3  = (2.303 / t) log [0.0175] / [0.015]

4.82 x 10-3  = (2.303 /t) 0.067

2.303 / t = 0.072

t = 32 s

c) for first order reaction

t1/2  = 0.693 / K = 0.693 / 0.00482

t1/2   = 143.8 s

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