Problem: The reaction2SO3(g) → 2SO2(g) + O2(g)is second order. If the concentration of SO3 decreases from 0.0360 moles/L to 0.0075 moles/L in 863 s, what is the rate constant for the reaction?a) 0.476 moles-1 L  s−1b) 0.0987 moles-1 L  s−1c) 5.23 moles-1 L  s−1d) 0.376 moles-1 L  s−1e) 0.122 moles-1 L  s−1 

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We’re being asked to determine the rate constant (k) of a second-order reaction:

2 SO3(g)  2 SO2(g) + O2(g)


The concentration of SO3 decreases from 0.0360 moles/L to 0.0075 moles/L in 863 s.


The integrated rate law for a second-order reaction is as follows:


1[A]t=kt+1[A]0


where: 

[A]t = concentration at time t

k = rate constant

t = time

[A]0 = initial concentration


81% (209 ratings)
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Problem Details

The reaction

2SO3(g) → 2SO2(g) + O2(g)

is second order. If the concentration of SO3 decreases from 0.0360 moles/L to 0.0075 moles/L in 863 s, what is the rate constant for the reaction?

a) 0.476 moles-1 L  s−1

b) 0.0987 moles-1 L  s−1

c) 5.23 moles-1 L  s−1

d) 0.376 moles-1 L  s−1

e) 0.122 moles-1 L  s−1

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