Calculating value of equilibrium constant

Question

Assignment:

Question 1. At 25 degees C, ΔH^o for the combustion of liquid octane, C₈H₁₈(l) to form CO₂(g) and H₂O(l) is -5471kJ/mol. Calculate ΔE^o for this reaction at 25 degrees C.

Question 2. The molar heat of vaporization of benzene, C₆H₆, at 1 atm is 30.8 kJ/mol. The boiling point of benzene at 1 atm is 78.3 degree C. Calculate the entropy change when 11.5g of benzene boils at the temperature.

Question 3. The heat capacity of a bomb calorimeter, is 87.5kJ/K (this value is for the total heat capacity including that of the water jacket around the reaction chamber). If 67.2g of methane(g) is combusted under such reaction conditions, what will be the increase in temperature on the calorimeter? What if ΔE combustion for CH₄(g) is -885.4 kJ/mol?

Question 4. The standard free energies of the formation of SO₂(g) is -300.4 kJ/mol and SO₃(g) is -370.4 kJ/mol. Calculate the value of the equilibrium constant at 25 degrees C for the reaction:

2SO₂(g) + O₂ ----------> 2SO₃(g)

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