🤓 Based on our data, we think this question is relevant for Professor Alghoul's class at GSU.
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).
We first need to convert the activation energy from kJ/mol to J/mol:
1 kJ = 103 J
The reaction between nitrogen dioxide and carbon monoxide is NO2(g) + CO(g) NO(g) + CO2(g). The rate constant at 701 K is measured as 2.57 M-1s-1 and that at 895 K is measured as 567 M-1s-1.
Use the value of the activation energy (Ea = 1.50 x 102 kJ/mol) and the given rate constant of the reaction at either of the two temperatures to predict the rate constant at 551 K.
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Based on our data, we think this problem is relevant for Professor Alghoul's class at GSU.