For the reaction 4HCl(g) + O₂ (g) → 2H₂O(g) + 2Cl₂ (g) AH° -114.4 kJ and AS° = -128.9 J/K The standard free energy change for the reaction of 2.26 moles of HCl(g) at 327 K, 1 atm would be This reaction is favored under standard conditions at 327 K. Assume that AHⓇ and AS are independent of temperature. kj.

Calculate AGo for a reaction for which AH° = 24.6 kJ and AS° = 132 J/K at 298 K. Is this reaction spontaneous under these conditions? O -16.3 J; spontaneous O 16.3 kJ; nonspontaneous O -14.7 kJ ; spontsneous O 14.7 kJ ; nonspontaneous

For the reaction 2C,H6(g) + 702(g)4CO2(g) + 6H2O(g) AH° = -2855.4 kJ and AS° = 92.7 J/K The standard free energy change for the reaction of 1.77 moles of C,H6(g) at 335 K, 1 atm would be kJ. This reaction is (reactant, product) | favored under standard conditions at 335 K. Assume that AH° and AS° are independent of temperature.

For the reaction2CO(g) + O2(g)2CO2(g)ΔG° = -515.1 kJ and ΔS° = -173.1 J/K at 294 K and 1 atm.The maximum amount of work that could be done by this reaction when 1.66 moles of CO(g) react at standard conditions at this temperature is  kJ.

The standard free energy of the hydrolysis of ATP to ADP: ATP (aq) → ADP (aq) + (aq) phosphate in solution is ∆G^0 = -313kJ/mol at 37˚C, 1 atm, all solutes are in their standard states at 1 mol/L Assume ideal solution behaviour.a) For a ratio of ATP to ADP of 10, what must be the concentration of phosphate to obtain ∆G = -40.0 kJ/mol for the hydrolysis?b) If the ratio of ATP to ADP is 10, what is the concentration of phosphate at equilibrium? What do you conclude from your answer (i.e., is the hydrolysis practical based on phosphate concentration)?

11:03 1 Question 19 of 20 Submit For a reaction for which AH = -142 kJ/mol and AS = -178 J/mol· K, which of the following statements is true? A) The reaction is spontaneous above 798 K. B) The reaction is spontaneous below 798 K. C) The reaction will never reach equilibrium. D) The reaction will never be spontaneous.

Given ΔHrxn = -98.9 kJ and ΔSrxn = - 94.0 J/K at 25 oC for the combination reaction of sulfur dioxide plus one oxygen atom to yield sulfur trioxide in the gas phase, is this reaction spontaneous or nonspontaneous?     spontaneous     nonspontaneous     neither

For the reaction CO(g) + 3H2(g) → CH4(g) + H2O(g) AH = -206.1 kJ and AS° = -214.7 J/K The standard free energy change for the reaction of 1.52 moles of CO(g) at 253 K, 1 atm would be This reaction is reactant favored under standard conditions at 253 K. Assume that AH° and AS are independent of temperature. kJ.

For a particular reaction, AH = 134.1 kJ/mol and AS = 35.0 J/(mol-K). Calculate AG for this reaction at 298 K. AG= What can be said about the spontaneity of the reaction at 298 K? The system is spontaneous in the reverse direction. The system is spontaneous as written. The system is at equilibrium. kJ/mol

For the reaction 2NH3(g) + 3N,0(g)→4N2(g) + 3H,O(g) AH° = -879.5 kJ and AS° = 288.1 J/K The standard free energy change for the reaction of 2.42 moles of NH3(g) at 267 K, 1 atm would be kJ. This reaction is (reactant, product) favored under standard conditions at 267 K. Assume that AH° and AS° are independent of temperature.