CHEMISTRY

To what temperature would the reaction below need to be heated to have a rate constant of 8.474e-4 M-1s-1 if the rate constant was 2.7000e-4 M-1s-1 at 327.00°C and the activation energy was 166.000 kJ/mol?
H2(g) + I2(g) ↔ 2HI(g)

a. 609.24°C

b. 336.09°C

c. 348.37°C

d. 377.90°C

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  1. Use the Arrhenius equation. Don't forget to convert kJ/mol to J/mol. And K must go into the equation as kelvin.

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