4 Use the data found in the Thermodynamic Values link under Reference Materials to calculate AH° and AS° at 25 °C for 2 NH3(g) N₂(g) + 3 H₂(g) Although the AH° and AS° values do change slightly with temperature, assume that the change is not large enough to significantly affect the outcome of the following calculation. Use the AH° and AS° values to determine the temperature (in K) at which this reaction will become nonspontaneous. Enter a number - no units.

Mg(s) + 2HCI(aq) MgCl, (aq) + H2 (g) + 1550kJ For this reaction at 25°C, Change in enthalpy: [ Select ] O because [ Select] • Change in entropy: [ Select ] O because [ Select ] · Change in Gibbs free energy: [ Select] thus • This reaction is [ Select ]

Consider the reaction: NH3 (g) + HCI (g) → NH4Cl (s) Given the following table of thermodynamic data at 298 K: Substance AH° (kJ/mol) S° (J/K-mol) NH3 (g) -46.19 192.5 HCI (g) -92.30 186.69 NH4Cl (s) -314.4 94.6 The value of K for the reaction at 25 °C is 1.1-10-16 9.3 - 1015 1.4.108 150 8.4. 104 Submit Request Answer

Use the standard free energy of formation data to determine the free energy change 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. MnO₂ (s) → Mn (s) + O₂ (g) b. H₂(g) + Br2 (1)→ 2HBr (g) c. Cu (s) + S (g) → CuS (s) d. 2LiOH (s) + CO₂ (g) → Li₂CO3 (s) + H₂O (g)

Delta H degrees and Delta S degrees for a reaction are –11.7 kJ/mol and –105 J/mol K, respectively. At what temperatures (in K) will this reaction be spontaneous under standard conditions?

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10) Use the Standard Free Energy of Formation values below to calculate Standard Free Energy for the balanced equation: PbCl₂(s) + 2NOF(g) →→→ PbF₂(s) + 2NOCl(g) Substance AGran (kJ/mol) PbCl₂(s) -314.2 NOF(g) -50.29 PbF₂(s) -630.9 NOCI(g) 66.07 Scanned with CamScanner

Dissolution of ionic compounds generally involves an increase in entropy (+ΔS°), but for a few specific metal ions, dissolution of the ionic compound can lead to a decrease in entropy. For example, the dissolution of magnesium chloride (MgCl2) has a ΔS° = -115 J K-1 mol-1. Explain this decrease in entropy

At 1120 K, AG° = 89.1 kJ/mol for the reaction 3 A (g) + B (g) →2 C (g). If the partial pressures of A, B, and C are 11.5 atm, 8.60 atm, and 0.510 atm respectively, what is the free energy for this reaction? %3D

In the reaction N2O4 = 2NO2, it is given that the AH298 and AS298 are +55.3kJ and +176J/K, respectively. Calculate AG at room temperature and discuss the spontaneity of this reaction at different temperature ranges.