Problem: For the reaction2N2O5(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-1B. 2.0 × 10−6  s-1C. 8.4 × 10−13  s-1D. 9.3 × 10−4  s-1E. 7.3 × 10−5  s-1

FREE Expert Solution

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:

ln k2k1=-EaR[1T2-1T1]

where:

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)


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Problem Details

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 30C? 

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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