Enthalpy of forward and reverse reactions

[Karina Rahadian 2G]

How do the enthalpy change for a reverse and forward reaction differ? Thanks!

[DylanNgo3F]

The net change in energy of a reaction is called the enthalpy of change. There really isn't a difference between the forward and backward reactions because the enthalpy change would be the same; just the opposite sign.

[Natasha Sutkin 2B]

Enthalpy change is a state function, meaning that it is only the net change. To find the enthalpy of reaction for a reversed reaction, you would just change the sign.

[Natalie Min 1C]

The enthalpy change for the reverse reaction is the negative of the enthalpy change for the forward reaction. For example, if the forward reaction released 40kJ of energy (delta H = -40kJ), the reverse reaction would require 40kJ of energy (delta H = 40kJ).

[Raya Amin 2A]

Yes, like everyone else is saying because enthalpy is a state function, the change in enthalpy is always represented by (final enthalpy - initial enthalpy). As a result, if you switch the forward and reverse reactions, the sign of delta H will also switch. In other words, if the forward reaction is originally endothermic and the reverse reaction is exothermic, and then you switch the order of the reaction, the forward reaction will now become exothermic (with a negative delta H).

[505468108]

If a reaction is reversed, the enthalpy is the opposite sign of the original reaction. Thus if the forward reaction is endothermic, the reverse reaction is exothermic.