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:
[A]t = concentration at time t
k = rate constant
t = time
[A]0 = initial concentration
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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