We’re being asked to determine the value of k at 30°C. We’re given the activation energy and the rates at two different temperatures.
This means we need to use the two-point form of the Arrhenius Equation:
k1 = rate constant at T1
k2 = rate constant at T2
Ea = activation energy (in J/mol)
R = gas constant (8.314 J/mol•K)
T1 and T2 = temperature (in K)
For the reaction
2N2O5(g) → 4NO2(g) + O2(g)
The activation energy is 1.0 × 105 J/mol and the value of k at 20◦C is 2.0 × 10−5 s-1 . What is the value of k at 30◦C?
A. 2.0 × 10−5 s-1
B. 2.0 × 10−6 s-1
C. 8.4 × 10−13 s-1
D. 9.3 × 10−4 s-1
E. 7.3 × 10−5 s-1
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