Which of the following reactions would you expect to proceed at a faster rate at room temperature? Why? (Hint: Think about which reaction would have the lower activation energy.)
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101. This reaction has an activation energy of zero in the gas phase: CH3 + CH3 -C2H5 a. Would you expect the rate of this reaction to change very much with temperature? b. Why might the activation energy be zero? c. What other types of reactions would you expect to have little or no activation energy?
A certain reaction has an activation energy of 37.51 kJ/mol. At what Kelvin temperature will the reaction proceed 5.00 times faster than it did at 349 K?