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, and the enthalpy of reaction is -20.0 kJ/mol. Which statement below is true?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 of 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

c. The reaction is endothermic

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