Exam 17: Gibbs Energy and Thermodynamics

Calculate Δ_rG at 298 K under the conditions shown below for the following reaction: $\quad$$\quad$ CaCO₃(s)→ CaO(s)+ CO₂(g) $\quad$$\quad$ Δ_rG° =+131.1 kJ mol^-1 $\quad$$\quad$ P(CO₂)= 0.033 atm

Calculate Δ_rG at 298 K under the conditions shown below for the following reaction: $\quad$$\quad$ 2Hg(g)+ O₂(g)→ 2HgO(s) $\quad$$\quad$ ΔG° = -180.8 kJ mol^-1 $\quad$$\quad$ P(Hg)= 0.025 atm,P(O₂)= 0.037 atm

Calculate ?_rG for the evaporation of methanol at 25°C under nonstandard conditions when $\mathrm { PCH } _ { 3 } \mathrm { OH }$ = 100.0 mbar $\quad$$\quad$$\quad$ CH₃OH(l)? CH₃OH(g)

Consider a reaction that has a positive Δ_rH and a positive Δ_rS.Which of the following statements is TRUE?

Determine Δ_rG° at 298 K using the following information: FeO(s)+ CO(g)→ Fe(s)+ CO₂(g)Δ_rH°= -11.0 kJ mol^-1; Δ_rS°= -17.4 J K^-1 mol^-1

How is a nonspontaneous process made spontaneous?

Which of the following processes have a Δ_rS > 0?

Place the following in order of increasing standard molar entropy. $\quad$ H₂O(l) $\quad$ H₂O(g) $\quad$ H₂O(s)

Consider a reaction that has a positive Δ_rH and a negative Δ_rS.Which of the following statements is TRUE?

Calculate Δ_rG° at 298 K using the following information: $\quad$$\quad$$\quad$$\quad$$\quad$ 2H₂S(g)+ 3O₂(g)→ 2SO₂(g)+ 2H₂O(g)Δ_rG° = ? Δ_fH° (kJ mol^-1)-20.6 $\quad$$\quad$$\quad$ -296.8 $\quad$$\quad$ -241.8 S°(J K^-1 mol^-1)205.8 $\quad$ 205.2 248.2 $\quad$$\quad$ 188.8

Use Hess's law to calculate Δ_rG° using the following information: $\quad$$\quad$ NO(g)+ O(g)→ NO₂(g) $\quad$$\quad$$\quad$$\quad$$\quad$$\quad$ Δ_rG° = ? $\quad$$\quad$ 2O₃(g)→ 3O₂(g) $\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$ Δ_rG° = +489.6 kJ mol^-1 $\quad$$\quad$ O₂(g)→ 2O(g) $\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$ Δ_rG° = +463.4 kJ mol^-1 $\quad$$\quad$ NO(g)+ O₃(g)→ NO₂(g)+ O₂(g) $\quad$$\quad$$\quad$ Δ_rG° = - 199.5 kJ mol^-1

How many microstates are possible in a collection of four particles that are present,with two particles each in two connected flasks?

Calculate Δ_rG at 298 K under the conditions shown below for the following reaction: $\quad$$\quad$ Fe₂O₃(s)+ 3CO(g)→ 2Fe(s)+ 3CO₂(g) $\quad$ ΔG° = -28.0 kJ mol^-1 $\quad$$\quad$ P(CO)= 1.4 atm,P(CO₂)= 2.1 atm

Calculate Δ_rG at 298 K under the conditions shown below for the following reaction: $\quad$$\quad$ 3O₂(g)→ 2O₃(g) $\quad$$\quad$$\quad$ Δ_rG° = +326 kJ $\quad$$\quad$ P(O₂)= 0.41 atm,P(O₃)= 5.2 atm

Calculate Δ_rS° for the following reaction.The S° for each species is shown below the reaction. $\quad$$\quad$$\quad$$\quad$$\quad$$\quad$ C₂H₂(g)+ H₂(g)→ C₂H₄(g) S°(J J K^-1 mol^-1) $\quad$ 200.9 $\quad$ 130.7 $\quad$ 219.3

Calculate Δ_rG° at 298 K using the following information: $\quad$$\quad$$\quad$$\quad$$\quad$ 2H₂S(g)+ 3O₂(g)→ 2SO₂(g)+ 2H₂O(g)Δ_rG° = ? Δ_fG°(kJ mol^-1)-33.4 $\quad$$\quad$$\quad$ -300.1 $\quad$ -228.6

Place the following in order of increasing molar entropy at 298 K. $\quad$ CO₂ $\quad$ C₃H₈ $\quad$ SO

Consider a reaction that has a negative Δ_rH and a positive Δ_rS.Which of the following statements is TRUE?

Estimate Δ_rG° for the following reaction at 387 K. $\quad$$\quad$ HCN(g)+ 2H₂(g)→ CH₃NH₂(g)Δ_rH°= -158.0 kJ mol^-1; $\quad$ Δ_rS°= -219.9 J K^-1 mol^-1

What is the name of the reaction that achieves the theoretical limits with respect to the change in Gibbs energy in thermodynamics?