Question

(a) Calculate ∆G for the reaction: C(s, graphite) + H2O (g) ↔ CO (g) + H2 (g) where temperature is 700 K, ∆G⁰ = 92 kJ and the initial pressure of each gas is P H2O = 0.67 atm, P CO = 0.23 atm, P H2 = 0.51 atm. (b) What direction would this reaction proceed?

Answer 1

The complete solution is

we know that AG = AGO RT ena cohere = reaction quotient Hene Temperature = I= 700K AGO = 92 KJ 922103J (²1 kJ= 1035) c cgraphites) + H₂O(g) = cocg) + H₂(g). Q = Peox PH2 l. P. 1) PHO Po = 0·23 atm P = 0.5l atm. Pho= 0.67 atm. QE 023 atm X 0.5 atm = 0 67 atm. - 0.17 atm R= 0.082 atm/mo.k. c) Gj - 920003 +0.08204mmo 700 eno:17 - 920001 +0.082 X700K X-)-27 - 920005't (-101.71 atmL) 9. 200oJ - 101.71 atm L. - 92oooJ-10305·795 (:1 alma 81694.21J - 81.69 KJ 6.115-10kg)/01•7) atmL = 101.3255 = 101:71 X101.325 : A G = 8169 kg

in the reaction ang No.of gas cous - No.of gaseous reactant product 2-1 Till = positive. If An= tve g then on increasing pressure the reaction coill Shift in backward. clirection. on decreasing the pressure the reaction will shift in forcoord dinection Here ang 1 = tve. on (1) ing pressure the reaction coi'll proceed in for wand direction. on cwing pressure the reaction coill proceed in backcourd direction.