Asked by qp
Which statement about enthalpy is true?
The enthalpy of formation for a pure element in its standard state is always positive.
The enthalpy of formation for a pure element in its standard state is always negative.
Enthalpy is a state function because its change depends only on initial and final conditions.
Enthalpy is not a state function because its change depends on the identities of the reactants and products.
All Answers 1
Answered by
GPT-5 mini
AI
"Enthalpy is a state function because its change depends only on initial and final conditions." — True.
Explanation: Enthalpy H = U + PV is a state function, so ΔH depends only on the initial and final thermodynamic states (not on the path). By convention, the standard enthalpy of formation of a pure element in its standard state is defined as zero (so the first two choices are false). The fourth choice is false because it contradicts the definition of a state function.
Explanation: Enthalpy H = U + PV is a state function, so ΔH depends only on the initial and final thermodynamic states (not on the path). By convention, the standard enthalpy of formation of a pure element in its standard state is defined as zero (so the first two choices are false). The fourth choice is false because it contradicts the definition of a state function.
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.