For a one step reaction, the activation energy for the forward reaction is 40.0

Question

For a one step reaction, the activation energy for the forward reaction is 40.0 kJ mol-1, and the enthalpy of reaction is -20.0 kJ mol-1. Which statement below is true?

Select one:

a. The activation energy of the forward reaction would be affected to a greater extent than the activation energy of the reverse reaction by addition of a catalyst.

b. The value for the enthalpy of reaction would be decreased by addition of a catalyst.

c. The reaction is endothermic.

d. The reverse reaction is slower than the forward reaction (smaller rate constant).

e. The reaction rate would be decreased by an increase in temperature.

Explanation / Answer

option d is correct

from the data it is clear that reaction is exothermic. so forward reaction favours more than backward reaction

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