Calculate ΔGrxn at 298 K under the conditions shown below for the following reaction.  Remember what does NOT appear in equilibrium constant expressions.  And also remember that this is NOT the Gibbs free energy under standard conditions.             SO3(g) + H2O(g) → H2SO4(liq)                   ΔG°= -90.5 kJ                  PSO3 = 0.20 atm, PH2O = 0.88 atm

Using reaction free energy to predict equilibrium composition Consider the following equilibrium: 2NOCI (g) = 2NO (g) + Cl2 (g) AGº =41. kJ Now suppose a reaction vessel is filled with 7.45 atm of nitrosyl chloride (NOCI) and 6.59 atm of chlorine (Cl₂) at 335. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of C₁₂ tend to rise or fall? ☐ x10 fall Is it possible to reverse this tendency by adding NO? In other words, if you said the pressure of C12 will tend to rise, can that be changed to a tendency to fall by adding NO? Similarly, if you said the pressure of C₁₂ will tend to fall, can that be changed to a tendency to rise by adding NO? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO needed to reverse it. Round your answer to 2 significant digits. yes no atm

[2] [a] The forward reaction is spontaneous for a particular reversible reaction. What can you conclude about the reverse reaction? AG = [b] What does the sign of the free energy have to be such that a reaction is spontaneous? AS = [c] [i] Under what conditions of enthalpy and entropy change is a reaction always spontaneous? AH= [ii] Under what conditions of enthalpy and entropy change is a reaction never spontaneous? - ΔΗ AS [d] If the entropy change is unfavorable for a certain reaction, is the reaction more likely to be spontaneous at a high temperature or a low temperature? [e] If the enthalpy change is unfavorable, but the entropy change is favorable, would a high temperature or a low temperature be more likely to lead to a spontaneous reaction?

Consider the gas-phase equilibrium, CH3OH(g) CO(g) + 2H2(g). For this reaction, standard free-energy and standard enthalpy changes for this reaction are -60 kJ/mol at 200°C and +95 kJ/mol (independent of temperature). What is free-energy change for this reaction at 200°C when partial pressures of CO, H2 and CH3OH are 8.0, 8.0 and 0.05 bar. 23.68 kJ/mol O-23.68 kJ/mol O-52.68 kJ/mol 52.68 kJ/mol