Question

18. Assuming that, since the physical states do not change, the values of ΔH and ΔS do not change as we raise the temperature, and using, NH3(g), Δ =-46,0 kJ mol., S' = +1 92.5 J mol·i K-1 calculate a value for the free energy change, Δ G for the reaction below, at 500 ℃ N2(g) + 3H2(g) 2 NH3(g) -> a. +7.2 kJ b. +61.3 kJ c. +18.8 kJ d. +54.2 kJ e. +83.3 kJ

Answer 1

5tandard entopy oF Change oF a Reaction: 4S. Mp S. Ceach Product ) -- Zn, s (each reactant) Sigma -Sum of.. np: Coefficient吇Product nyCoeffi cient ofreactant . 4s S tandar d entropy change of a reaction each Product吋 standard entropy react ion (each Producl) 5 Teach Yea ctant) ש Standard entropy of each veactant of a reat ion

AG p (each Products) g maSum of" npCoedficient of Producb nyCoeffrcient of reactan t r= Standard Gibbs rree energy chang chanaL Standar d Gibbs &Yee energy ^format ion ซึ่ each Produ cts AG Fleach products) Changa AG leach reactantsStandard ibbs Free eneryFormati op of each reactants

98.3 oo03 = Ан. -T AS react ion reaction -92.0«J + 153.2859 KJ z+61.3 KJ reaction