Consider the oxidation of NO to NO2: NO(g) + 1/2 O2(g) → NO2(g). Calculate ΔG°rxn at 25 °C given the following standard Gibbs free energies of formation: ΔG°f(NO) = 86.6 kJ/mol, ΔG°f(O2) = 0 kJ/mol, ΔG°f(NO2) = 51.3 kJ/mol.

Consider the following reaction: CO2(g) + CCl4(g) ⇌ 2COCl2(g). Calculate ΔG for this reaction at 25 °C under these conditions: PCO2 = 0.140 atm, PCCl4 = 0.185 atm, PCOCl2 = 0.755 atm. Given that ΔG°f for CO2(g) is −394.4 kJ/mol, what is the value of ΔG?

Consider the following reaction: C2H4(g) + H2(g) → C2H6(g) with ΔH = -137.5 kJ and ΔS = -120.5 J/K. Calculate ΔG at 25 °C and determine whether the reaction is spontaneous.

Consider the following reaction: I2(g) + Cl2(g) ⇌ 2ICl(g) with Kp = 81.9 at 25 °C. Calculate ΔG⁰rxn for the reaction at 25 °C under equilibrium conditions. Express your answer in kilojoules.

Consider the following reaction: I2(g) + Cl2(g) ⇌ 2ICl(g) with Kp = 81.9 at 25 °C. Calculate ΔG⁰rxn for the reaction at 25 °C under standard conditions.

For the vaporization of benzene, ΔHvap = 30.7 kJ/mol and ΔSvap = 87.0 J/(K·mol). Does benzene boil at 75 °C and 1 atm pressure?

Which of the following conditions indicates that a chemical reaction is spontaneous at constant temperature and pressure?

Which of the following conditions indicates that a chemical reaction is spontaneous at constant temperature and pressure?

Which of the following conditions will result in a spontaneous reaction at standard conditions according to the Gibbs free energy equation ΔG°rxn = ΔH°rxn - TΔS°rxn?