The activation energy of the forward reaction would be affectedto a greater exte

Question

The activation energy of the forward reaction would be affectedto a greater extent than the activation energy of the reversereaction by addition of a catalyst.

The value for the enthalpy of reaction would be decreased byaddition of a catalyst.

The reverse reaction has a higher activation energy than theforward reaction.

The reaction is endothermic.

The activation energy of the forward reaction would be affectedto a greater extent than the activation energy of the reversereaction by addition of a catalyst.

Explanation / Answer

1.)    The activation energy of the forward reactionwould be affected to a greater extent than the activation energy ofthe     reverse reaction by addition of acatalyst. This is not true: a catalyst should affect a greater activationenergy more than it would a smaller activation energy. Sincethe enthalpy of the reaction is negative, energy is released. Thus the reverse reaction would have a greater energy ofactivation. 2.)   The value for the enthalpy of reaction would bedecreased by addition of a catalyst. This is not true: the enthalpy of the reaction is the energy of theheats of formation of the beginning and ending products. Since the catalyst is not consumed, at cannot change the energy ofeither. 3.)   The reverse reaction has a higher activation energythan the forward reaction. This is true. Since the enthalpy of the reaction is negative,energy is released. Thus the reverse reaction would have agreater energy of activation. 4.)   The reaction is endothermic. This is not true. The enthalpy of the reaction is negative,so energy is being produced and the reaction is exothermic.

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