1. Given that A,H° = –2219 kJ/mol-rxn and that A, S° = -216 J/K · mol-rxn at 25 °C, determine the value of A,G° at 25 °C for the reaction C3HS (g) + 5 O2(g) → 3 CO2 (g) +4 H2O(l) (a) -2283 kJ/mol-rxn Answer + (b) -2214 kJ/mol-rxn Answer (c) -2155 kJ/mol-rxn Answer + (d) 6.218 x 104 kJ/mol-rxn Answer +

Determine the  ΔH of formation for sulfur trioxide gas if: 2 SO2 (g) +  O2 (g) --> 2 SO3 (g)    ΔH = -300 kJ SO2 (g)  -->    O2 (g) + S (s)    ΔH = 200 kJ The standard state of sulfur is S  (s).         -500 kJ/mol     -400 kJ/mol     - 350 kJ/mol     +200 kJ/mol     +100 kJ/mol

Determine the  ΔH of formation for sulfur trioxide gas if: 2 SO2 (g) +  O2 (g) --> 2 SO3 (g)    ΔH = -300 kJ SO2 (g)  -->    O2 (g) + S (s)    ΔH = 200 kJ The standard state of sulfur is S  (s).         - 350 kJ/mol     -500 kJ/mol     +200 kJ/mol     +100 kJ/mol     -400 kJ/mol

A 0.576 g sample of liquid C5H12 was combusted using excess oxygen gas inside a bomb calorimeter, with the products being carbon dioxide gas and liquid water. The calorimeter's heat capacity is 4.957 kJ °C^-1. If the temperature inside the calorimeter increased from 25.0 °C to 35.1 °C, determine A,U for this reaction in kl mol (with respect to C3H12). Do not worry about how realistic the final answer is.

1. A reaction with AH° = -64.0 kJ/ mole has K = 1.00 X 108 at 25.0 °C. What would be the value of K at 0.00 °C? 2. A reaction with AH° = 618.0 kJ/mole has K = 1.00 X 1060 at 25.0 °C. What would be the value of K at 500.0 °C?

1. For the reaction: CO(g) +H₂O(g) → CO2(g) +H2(g) Calculate AG at room temperature (25 °C) ΔΗ°= -41.2 kJ AS = -135 J/K

Calculate ΔHf for HCN(g) at 25°C, given the following related reaction at 25°C, 2 NH3(g) + 3 O2(g) + 2 CH4(g) ---> 2 HCN(g) + 6 H2O(g); ΔHrxn = -870.8 kJ and the heats of formation of some species are ΔHf = -80.3 kJ/mol for NH3(g), -74.6 kJ/mol for CH4, and -241.8 kJ/mol for H2O(g). Answers are in kJ/mol.

Given the data in the table below, determine ΔH°rxnfor the reaction             4NO (g)  +  6 H2O (l) →  4NH3 (g)  +  5 O2 (g)

Consider the reaction that happens at -13 °C: 1A + 2B 8C + 6D. Using the data from the table: B C D AH; (kJ mol 1) 309 144.4 149.5 s° (U mol 1 K1) 61.4 33.6 76.4 153.4 calculate AG° (in kJ) of the reaction. (assume that values of AH and S do not change with the temperature) Enter a number with sign (+ or -) to 1 decimal place in kJ.

Methanol, CH3OH , is formed from methane and water in a two‑step process. Step 1: CH4(g)+H2O(g)--->CO(g)+3H2(g)      ΔS∘= 214.7 J/K Step 2: CO(g)+2⁢H2⁡(g)⟶CH3OH(l)       Δ⁢S∘= −332.3 J/K   Calculate ΔH∘ and ΔG∘ at 298 K for step 1 and step 2. At what temperature in K does step 1 and step 2 become spontaneous? Is step 1 and step 2 spontaneous at temperatures greater or less than the calculated temperature?