Unit IV 7. (a) How energy balance equation for adiabatic operation (b) 8. (a) (b) can be represented graphically? 10 Estimate the equilibrium constant at 600 K for the reaction At 298 K: C2H4(g) + H2O(g) → C₂H₂OH(g) At 298 K : AG° 2030 kcal/mol AF for H2O(g) = - 57798 cal/mol C2H5OH(g) = 56240 cal/mol = C2H4(g) 12496 cal/mol Discuss the General graphical procedure in detail. 10 The standard heat of gas phase reaction at 25°C =- (298 K) A+B →2R = 50000 J is Indicating that the reaction is strongly exothermic. It is planned to run this reaction at 1000 oC. What is the value of heat of reaction at this temperature? Is the reaction still exothermic at 1000°C. 5 5

The equilibrium constant for a certain reaction increases by a factor of 6.67 when the temperature is increased from 300.0 K to 350.0 K. Calculate the standard change in enthalpy (H) for this reaction (assuming H is temperature-independent).

Actually, the carbon in CO2(g) is thermodynamically unstable with respect to the carbon in calcium carbonate(limestone). Verify this by determining the standardGibbs free energy change for the reaction of lime,CaO(s), with CO2(g) to make CaCO3(s).

What is a spontaneous reaction?

For the system 2SO3(g)2SO2(g)+O2(g) K=1.32 at 627. What is the equilibrium constant at 555C?

When 7.11 g NH4NO3 is added to 100 mL water, the temperature of the calorimeter contents decreases from 22.1 C to 17.1 C. Assuming that the mixture has the same specific heat as water and a mass of 107 g, calculate the heat q. Is the dissolution of ammonium nitrate exothermic or endothermic?

Another step in the metabolism of glucose, which occurs after the formation of glucose6-phosphate, is the conversion of fructose6-phosphate to fructose1,6-bisphosphate(bis meanstwo): Fructose6-phosphate(aq) + H2PO4(aq) fructose l,6-bisphosphate(aq) + H2O() + H+(aq) (a) This reaction has a Gibbs free energy change of +16.7 kJ/mol of fructose6-phosphate. Is it endergonic or exergonic? (b) Write the equation for the formation of 1 mol ADP fromATR for which rG = 30.5 kJ/mol. (c) Couple these two reactions to get an exergonic process;write its overall chemical equation, and calculate theGibbs free energy change.

Suppose you have an endothermic reaction with H = +15 kJ and a S of + 150 J/K. Calculate G and Keq at 10,100, and 1000 K.

Determine the equilibrium constant for the reaction Sn+Pb2+Sn2++Pb

What is the sign of the standard Gibbs free-energy change at low temperatures and at high temperatures for the explosive decomposition of TNT? Use your knowledge of TNT and the chemical equation, particularly the phases, to answer this question. (Thermodynamic data for TNT are not in Appendix G.) 2C7H5N3O6(s) 3N2(g) + 5H2O() + 7C(s) + 7CO(g)