Please helo me solve the answer with the work! Thank you very much in advance. E
ID: 537976 • Letter: P
Question
Please helo me solve the answer with the work! Thank you very much in advance.
Ethlylene reacts with hydrogen to produce ethane: H_2 C = CH_2 (g) + H_2 (g) rightarrow H_3 C - CH_3 (g). a. Using the data from the appendix in your text, find the Delta G degree for the reaction at 25.0 degree C. Is the reaction predicted to be product-favored under standard conditions? b. Calculate the K_p from the Delta G degree _rxn. Comment on the sign of the free energy and the magnitude of the equilibrium constant.Explanation / Answer
deltaGo data (Kj/mole): C2H6= -32.8, ethylene :68.24 and H2=0
C2H4+H2------->C2H6
standard gibbs free energy = sum of gibbs free energy of products- sum of gibbs free energy of reactants
deltaG0 =1* (-32.0)- (1*68.24+1*0)=-101.4 Kj (1,1 and 1 are coefficients off C2H6, C2H4 and H2 respectively)
when gibbs free energy change is -ve, the reaction is spontaneous and product favored.
deltaGo=-RTlnK, KP= equilibrium constant
101.4*1000= 8.314*298*lnKP, R= 8.314 J/mole.K,
lnKP= 101.4*1000/(8.314*298)= 40.93
KP=5.95*1017
the high value of equilibrium constant suggests product favorable reaction.