1. Determine ΔG° at 298.15K for the reaction: 4Fe (s) + 3O2 (g) → 2Fe2O3 (s) Given that ΔH° = -1648 kJ ; ΔS° = -549.3 J/K 2. What mass of sucrose must be burned to produce 2600 J of heat? The enthalpy of combustion of sucrose is : -5.65 x 103kJ/mol

Using H° data, calculate the standard enthalpy change for the reaction at 298K. 2 NH3(g) HNO3(aq) --> NO2(g) 2 H20(1) AH° (KJ/mol) -46.19 -206.6 33.84 -285.83 (Note: the table AH values are located directly below the corresponding compound, this is the number found in the Appendix)

Given ΔGorxn = -1,114.8 kJ/mol for the following reaction and the listed ΔGof values below each substance, calculate ΔGof (in kJ/mol) for D(ℓ) at 25 oC.    2 A (ℓ) + 3 B (g) →→ 2 C (g) + 4 D (ℓ) ΔGof  (kJ/mol) -110.7   258.4   -581.7   ?

For the reaction: CuS (s) + H₂(g) → H₂S (g) + Cu (s) Given: ΔS ⁰ (CuS) = 66.5 J/mole-K ΔHf ⁰ (CuS) = -53.1 kJ/mol ΔS ⁰ (H₂S) = 205 J/ mole-K ΔHf ⁰ (H₂S) = -20.6 kJ/mol ΔS ⁰ (Cu) = 33.3 J/ mole-K ΔH f ⁰ (Cu) = 0.0 kJ/mol ΔS ⁰ (H₂) = 131 J/ mole-K ΔH f ⁰(H₂) = 0.0 kJ/mol The standard free energy of the reaction ΔG ⁰ rxn is A) -37.9 kJ/mole B) 44.6 kJ/mole C) -20.3 kJ/mole D) +20.3kJ/mole and spontaneous E) +37.9 kJ/mole

The standard state Gibb's energy and entropy changes are known for the reaction: 2H, S(g) + 30,(g)=2H20(g) + 2SO2(g) What is the standard state enthalpy change for the reaction at 25 C? 120 kJ 52 J AGº ASº Mole Mole K -68 kJ/mol 154 kJ/mol 104 kJ/mol O -119 kJ/mol

A reaction has an equilibrium constant (K) of 90.9.  If the entropy of this reaction is -69.1 J/mol K at a temperature of 280 K, what is the enthalpy of this reaction in kJ/mol?Report your answer to one decimal place. ΔG = ΔH - T ΔSΔG = -RT ln K

Calculate the standard free energy for the reaction given.  2 CH 3OH( l) + 3 O 2( g) → 2 CO 2( g) + 4 H 2O( l)     a -797.8 kJ   b -2069.8 kJ   c -1404.8 kJ   d -465.2 kJ

Calculate AS°surr for the reaction shown below using the provided thermodynamic properties information. 2 PCI3 (g) + O2 (g) → 2 POCI3 (g) AH°f Substance (kJ/mol) PCI3 (g) -288.01 POCI3 (g) -542.2 1.706 kJ/(mol•K) 8.530 x 10-1 kJ/(mol•K) 10.17 kJ/(mol•K) 254.1 kJ/(mol•K) 20.33 kJ/(mol•K)