Use the standard free energy data in the attached table to determine (1) ΔHrxn, (2) ΔSrxn, (3) ΔSsurr, and ΔSuniv for each of the following reactions, which are run under standard state conditions and 25 °C. Identify each as either spontaneous or nonspontaneous at these conditions. (a) Fe2O3(s)+3CO(g)⟶2Fe(s)+3CO2(g) (b) CaSO4⋅2H2O(s)⟶CaSO4(s)+2H2O(g)
- Use the standard free energy data in the attached table to determine (1) ΔHrxn, (2) ΔSrxn, (3) ΔSsurr, and ΔSuniv for each of the following reactions, which are run under standard state conditions and 25 °C. Identify each as either spontaneous or nonspontaneous at these conditions.
(a) Fe2O3(s)+3CO(g)⟶2Fe(s)+3CO2(g)
(b) CaSO4⋅2H2O(s)⟶CaSO4(s)+2H2O(g)
2. Calculate ΔG° for each of the following reactions from the equilibrium constant at the temperature given.
(a) H2(g)+I2(g)⟶2HI(g) T=400°C Kp=50.0
(b) CaCO3(s)⟶CaO(s)+CO2(g) T=900°C Kp=1.04
(c) HF(aq)+H2O(l)⟶H3O+(aq)+F−(aq) T=25°C Kp=7.2×10−4
(d) AgBr(s)⟶Ag+(aq)+Br−(aq) T=25°C Kp=3.3×10−13
3. Calculate the equilibrium constant at 25 °C for each of the following reactions from the value of ΔG° given.
(a) O2(g)+2F2(g)⟶2OF2(g) ΔG°=−9.2 kJ
(b) I2(s)+Br2(l)⟶2IBr(g) ΔG°=7.3 kJ
(c) 2LiOH(s)+CO2(g)⟶Li2CO3(s)+H2O(g) ΔG°=−79 kJ
4. Calculate the equilibrium constant at the temperature given. (Hint: Use formation free energy ΔGf⁰ values to calculate ΔG for the reaction first)
(a) I2(s)+Cl2(g)⟶2ICl(g) (T=100°C)
(b) H2(g)+I2(s)⟶2HI(g) (T=0.0°C)
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