How does Activation Energy Affect Reaction Rate?

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SUMMARY

The activation energy for the reaction 2N2O5 (g) → 2N2O4 (g) + O2 (g) is established at 103 kJ/mol. To determine the temperature at which the reaction rate is 80.0 times greater than at 300 K, the Arrhenius equation must be utilized. The gas constant is specified as 8.314 J/mol*K. Clarification is needed regarding the temperature unit, as the discussion raises the possibility of a misinterpretation between Celsius and Kelvin.

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dgoudie
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[SOLVED] Activation Energy related to rate.

The activation energy for the reaction : 2N_{2}O_{5} (g) \rightarrow 2N_{2}O_{4} (g) + O{2} (g), is 103 kJ/mol.

The gas constant is 8.314 J/mol*K
Using only information given in this problem calculate the temperature at which the rate of the reaction is 80.0 times greater than it is at 300.0 degrees C (Notice that the given information concerns rates, not rate constants.)


I'm not really sure how do go about this question. do I still use Arrhenius's Equation?

any help would be greatly appreciated. thanks
 
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Yes, you can use the Arrhenius equation. Did you really mean 300 C? Are you sure it isn't 300 K? As far as I know, this very complicated first-order reaction was only studied over the temperature range 0 C to 123 C but I may be wrong. Please check.
 

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