What is ∆Gº for the reaction where Keq=22.5? (R=8.314x10-3kJ/mol-K)
-7.71 kJ
-3.35 kJ
-2390 kJ
-1.28x1016kJ
What is ∆Gº for the reaction where Keq=22.5? (R=8.314x10-3kJ/mol-K) -7.71 kJ -3.35 kJ -2390 kJ -1.28x1016kJ...
What is the value of Keq if ∆Gº=15.6 kJ (R=8.314 J/mol-K)? 1.84x10-3 0.994 1.01 5.05x10-7
Determine Gº for a reaction when AG = -119.1 kJ/mol and Q = 0.043 at 298 K. (R = 8.314 J/mol · K)
If ∆Hº = 220 kJ/mol and ∆Sº = –150 J/mol•K, calculate ∆Gº, in units of kJ/mol, at 25ºC
Question 5 For a chemical reaction, AH° 238 = +135.7 kJ and A Sº= +0.379 kJ/K. Calculate A Gº 800 A-167.5 kJ B.-132.8 kJ C. +133.9k D-212.8 kJ E.-192.3 kJ ОА OB ОС OD ОЕ Question 6 0.5 pt For a chemical reaction, Hº 238 = +135.7 kJ and A Sº = +0.379 kJ/K. At what temperature will A Gº=0? A. 213K B. 402K C.358 K D. 470K E. 251K ОА OB Ос OD ОЕ Question 7 0.5 For a...
Calculate ∆Gº for the reaction, CH4(g)+2O2(g)→CO2(g)+2H2O(g), where ∆Gfº=-50.8 kJ/mol for CH4(g), -394 kJ/mol for CO2(g), and -229 kJ/mol for H2O(g).
Calculate ∆Gº for the reaction, CH4(g)+2O2(g)→CO2(g)+2H2O(g), where ∆Gfº=-50.8 kJ/mol for CH4(g), -394 kJ/mol for CO2(g), and -229 kJ/mol for H2O(g): 572 kJ -801 kJ -572 kJ 801 kJ
03(g) + OH(g) =H(g) + 2 O2(g) AG° = 5.8 kJ/mol at 298 K, A,Gº = 0 kJ/mol at 354 K, and 4 Gº = -2.0 kJ/mol at 373 K. (a) Calculate the equilibrium constant value for this reaction at 298K, 354 K, and 373 K. (b) At 354K, calculate the change in the Gibbs energy of the reaction, AG when the partial pressures of O3 and OH are kept at 10 bar and 30 bar, respectively, while O2 and...
Estimate ∆Gº at 750.0 K for the reaction SO2(g) + 3CO(g) → COS(g) + 2CO2(g) given that at 25.00 ºC ∆Hº=–300.8 kJ/mol and ∆Gº=–246.3 kJ/mol. A –756.7 kJ/mol B –163.7 kJ/mol C –119.6 kJ/mol D –246.3 kJ/mol E –54.5 kJ/mol
For a given reaction, Delta H = -19.9 kJ/mol and Delta S = -55.5 J/K-mol. Calculate the temperature in K where Delta G = 0. Assume that Delta H and Delta S do not vary with temperature. Also, what is the equilibrium constant at that temperature?
31. What is ∆G for a reaction where ∆G° = -4.5 kJ/mol and Q = 4.0 at 295 K? (R = 8.314 J/mol ・ K)