Explain the activation energy of a certain reaction

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Reference no: EM13149663

The activation energy of a certain reaction is 45.3kJ/mol . At 24{~}^{\circ}\rm C , the rate constant is 0.0160s^{-1} . At what temperature in degrees Celsius would this reaction go twice as fast? I get that you use the arrhenius equation but can some explain in detail how you get T2 by itself after everything is set up properly?

Reference no: EM13149663

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Explain the activation energy of a certain reaction : The activation energy of a certain reaction is 45.3kJ/mol . At 24{~}^{\circ}\rm C , the rate constant is 0.0160s^{-1} . At what temperature in degrees Celsius would this reaction go twice as fast?

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