h: 8.314 x103 ks) molk 1773 K 25. At 1500°C the equilibrium constant for the reaction CO(g) + 2H₂(g) + CH3OH(g) has the

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H 8 314 X103 Ks Molk 1773 K 25 At 1500 C The Equilibrium Constant For The Reaction Co G 2h G Ch3oh G Has The 1 (32.41 KiB) Viewed 46 times

h: 8.314 x103 ks) molk 1773 K 25. At 1500°C the equilibrium constant for the reaction CO(g) + 2H₂(g) + CH3OH(g) has the value K₂=1.4 x 10-7. Calculate AG" for this reaction at 1500°C. AG=(-2.303) 1loyk a. 105 kJ/mol b. 1.07 kJ/mol = (-2.303) (8.314x(0-3k5/mlk) (1773 k) (log(14 x 10")) (-2.303) (8.314 x(03k5/mlk) (1773 k) (-6.85387) C. -233 kJ/mol -105 kJ/mol = (-33.as k3/mol) (6.854) e: 233 kJ/mol = 232.7 * 5/mpl 233 kJ/mol 26. What is the AG for of CH₂OH in the previous reaction if the AG" for of CO is -137.16 KJ/mol? a. -370 kJ/mol b. -95.8 kJ/mol C. 370 kJ/mol d. 95.8 kJ/mol e. 130 kJ/mol