Question

For a spontaneous process, the incorrect statement is:

• A. \((\Delta G_{\text{system}})_{T,P}>0\)
• B. \((\Delta S_{\text{system}}) + (\Delta S_{\text{surroundings}})>0\)
• C. \((\Delta G_{\text{system}})_{T,P}<0\)
• D. \((\Delta U_{\text{system}})_{S,V}<0\)

Answer 1

The Correct Option is A

For a spontaneous process at constant temperature and pressure:

• Gibbs Free Energy (\(\Delta G\)) must be negative: \(\left(\Delta G_{\text{system}}\right)_{T,P}<0\).
• The total entropy change (system + surroundings) must be positive: \(\left(\Delta S_{\text{system}}\right) + \left(\Delta S_{\text{surroundings}}\right)>0\).
• Internal energy change (\(\Delta U\)) can vary depending on the process but is typically negative under adiabatic conditions.

Option 3, which states \(\left(\Delta G_{\text{system}}\right)_{T,P}>0\), is incorrect because a positive \(\Delta G\) implies a non-spontaneous process.