Gibbs Free Energy and Thermodynamics

What does ΔH° < 0 and ΔS° < 0 mean in terms of spontaneity?

• The process is spontaneous

• The process is non-spontaneous

• The process is spontaneous at high temperatures

• The process is spontaneous at low temperatures

What does ΔG° represent in the Gibbs Free Energy equation?

• Enthalpy change

• Temperature

• Entropy change

• Gibbs free-energy change

What does an increase in overall entropy indicate in a reaction?

• The reaction is not spontaneous.

• The reaction is spontaneous.

• The reaction requires continuous energy supply.

• The reaction stops midway.

Do enthalpy changes alone determine whether a reaction is spontaneous or not?

• Yes

• No

• Sometimes

• Only at high temperatures

What contributes to the spontaneity of a reaction?

• Only enthalpy

• Only entropy

• Both enthalpy and entropy

• Neither enthalpy nor entropy

What does ΔS represent in the formula for free-energy change?

• Entropy change

• Enthalpy change

• Temperature change

• Free-energy change

What does the term "theoretically feasible" imply about a reaction with a negative ΔG?

• The reaction can occur under the right conditions

• The reaction will definitely occur

• The reaction cannot occur

• The reaction will occur at a constant rate

What is the primary limitation of using ΔG to predict reaction feasibility?

• It doesn't provide information about the reaction rate

• It doesn't consider temperature

• It doesn't consider enthalpy

• It doesn't consider entropy

What is the unit of ΔS in the given reaction?

• J K⁻¹ mol⁻¹

• kJ mol⁻¹

• J mol⁻¹

• kJ K⁻¹ mol⁻¹

What is the enthalpy change (ΔH) in the given reaction?

• -822 kJ mol⁻¹

• -740973.8 J mol⁻¹

• -271.9 J K⁻¹ mol⁻¹

• 90 J K⁻¹ mol⁻¹