Question

Given that a reaction absorbs energy and has an activation energy of 50 kJ/mol, which of the following statements are correct?

a) The reverse reaction has an activation energy equal to 50 kJ/mol.
b) The reverse reaction has an activation energy less than 50 kJ/mol.
c) The reverse reaction has an activation energy greater than 50 kJ/mol.
d) The change in internal energy is less than zero.
e) The change in internal energy is greater than zero.

Answer 1

The reverse reaction has an activation energy less than 50 kJ/mol and the change in internal energy is greater than zero.

Step-by-step explanation:

The correct statements are b) The reverse reaction has an activation energy less than 50 kJ/mol and e) The change in internal energy is greater than zero.

The reverse reaction of a reaction that absorbs energy will release energy. Therefore, the reverse reaction will have a lower activation energy than the forward reaction. This means that statement b) is correct.

The change in internal energy is determined by the difference in energy between the products and the reactants. Since a reaction that absorbs energy has higher energy products, the change in internal energy will be greater than zero. Therefore, statement e) is correct.