Gibbs Free Energy

Which conditions represent a process which is thermodynamically favorable at all temperatures?

• S > 0 and H > 0

• S < 0 and H > 0

• S > 0 and H < 0

• S < 0 and H > 0

If a reaction is exothermic, and decreases in entropy, then the reaction will be favorable at:

• All temperatures.

• No temperatures.

• High temperatures.

• Low temperatures.

When the value of Gibbs free energy is zero

• The reaction is at equilibrium

• The reaction can happen

• The reaction can still be feasible

• The reaction will be reversible

Gibbs free energy will tell you

• That a reaction is spontaneous

• That a reaction will not occur

• That a reaction is both feasible and spontaneous

• The Entropy is at zero

Which equation represents the relationship between ΔG, ΔH, and ΔS

• ΔG = ΔH + TΔS

• ΔH = ΔG - ΔS

• ΔG = ΔS - TΔH

• ΔG = ΔH - TΔS

Predict the sign (+, -, or 0) of ∆G_f°, ∆H_f°, ∆S_f°, respectively, for the deposition of carbon dioxide (CO₂) at room temperature and atmospheric pressure. CO₂ (g) → CO₂ (s)

• -, +, +

• 0, +, +

• -, +, -

• +, -, -

Delta G is negative indicates

• reaction is exothermic

• reaction is endothermic

• reaction is spontaneous

• reaction is not spontaneous

Which combination of ΔH and ΔS NEVER has a spontaneous reaction?

• +ΔH and +ΔS

• +ΔH and -ΔS

• -ΔH and -ΔS

• -ΔH and +ΔS

Tags

NGSS.HS-PS1-4

Which of these would ALWAYS indicate a process is spontaneous?

Spontaneous reactions are driven by

• increasing enthalpy and increasing entropy.

• decreasing enthalpy and decreasing entropy.

• increasing enthalpy and decreasing entropy.

• decreasing enthalpy and increasing entropy.