A student determines the value of the equilibrium constant to be 7.94×10-37 for the following reaction. H2S(g) + 2H2O(l)3H2(g) + SO2(g) Based on this value of Keq: G° for this reaction is expected to be (greater, less)  than zero. Calculate the free energy change for the reaction of 1.85 moles of H2S(g) at standard conditions at 298K.      G°rxn =  kJ

A student determines the value of the equilibrium constant to be 4.30×10-15 for the following reaction. 2CO₂(g) + 5H₂(g)C₂H₂(g) + 4H₂O(g) Based on this value of Keq: AG° for this reaction is expected to be (greater, less) Calculate the free energy change for the reaction of 1.72 moles of CO₂(g) at standard conditions at 298K. AGOrxn= kj Submit Answer than zero. Retry Entire Group 9 more group attempts remaining

A student determines the value of the equilibrium constant to be 55.2 for the following reaction. C2H4(g) + H,O(g)- →CH;CH2OH(g) Based on this value of Keqi AG° for this reaction is expected to be (greater,less) than zero. Calculate the free energy change for the reaction of 1.64 moles of C,H.(g) at standard conditions at 298K. kJ rxn

10) Use the Standard Free Energy of Formation values below to calculate Standard Free Energy for the balanced equation: PbCl₂(s) + 2NOF(g) →→→ PbF₂(s) + 2NOCl(g) Substance AGran (kJ/mol) PbCl₂(s) -314.2 NOF(g) -50.29 PbF₂(s) -630.9 NOCI(g) 66.07 Scanned with CamScanner

A student determines the value of the equilibrium constant to be 6.29×104 for the following reaction.S(s,rhombic) + 2CO(g)SO2(g) + 2C(s,graphite)Based on this value of Keq:G° for this reaction is expected to be (greater, less) fill in the blank  than zero.Calculate the free energy change for the reaction of 1.85 moles of S(s,rhombic) at standard conditions at 298K.    G°rxn = _____ kJ

[Review Topics] [References] Use the References to access important values if needed for this question. A student determines the value of the equilibrium constant to be 1.21x1012 for the following reaction. CO(g) + Cl2(g)- COC12(g) Based on this value of Keg AG° for this reaction is expected to be (greater,less) than zero. Calculate the free energy change for the reaction of 1.65 moles of CO(g) at standard conditions at 298K. AG rxn kJ

[References] Use the References to access important values if needed for this question. A student determines the value of the equilibrium constant to be 1.54 x 1025 for the following reaction. CO(g) + 3H₂(g) → CH4 (9) + H₂O(g) Topics] Based on this value of Keq: AGO for this reaction is expected to be than zero. Calculate the free energy change for the reaction of 1.73 moles of CO(g) at standard conditions at 298 K. AGO kj rxn Submit Answer Retry Entire Group 4 more group attempts remaining

The law of thermodynamics states that every spontaneous process moves towards greater ontropy. second first O third O fourth

What must the reaction quotient Q be, if the free energy is -961.941 kJ at 25.0°C? 5C2H2(g) + 5 H2(g) → C10H20(g) AGO = -925. 150 kJ.

For the reaction CH4 (9) + H₂O(g) → 3H₂(g) + CO(g) AH = 206.1 kJ and AS = 214.7 J/K The standard free energy change for the reaction of 1.83 moles of CH4 (9) at 345 K, 1 atm would be kj. This reaction is favored under standard conditions at 345 K. Assume that AH and AS are independent of temperature.