The reaction between hydrogen gas and carbon to produce the gas known as ethylene is:2 H2(g) + 2 C(s) → H2C=CH2(g), ∆G = +16.3 kcal/mol (+68 kJ/mol) 25 °C.Is this reaction spontaneous at 25 °C?

What are the signs of ∆H, ∆S and ∆G for the spontaneous conversion of a solid into gas?

Consider the combustion of butane gas and predict the signs of ΔS, ΔH and ∆G.

C₄H₁₀(g) + 13/2 O₂(g) ⟶ 4 CO₂(g) + 5 H₂O(g)      

A particular reaction has ΔG = –350 kJ and ΔS = –350 J/K at 24°C. How much heat will be released/absorbed?

For a reaction in which ΔH = 125 kJ and ΔS = 325 J/K, determine the temperature in Celsius above which the reaction is spontaneous.