At 25.00 °C, a reaction was determined to have a AH of 25.00 kJ/mol and AS of 262.0 J/mol K. Calculate the AG in kJ/mol for this reaction.

Explain what happens as a reaction starts with G0 (negative) and reaches the point where G=0.

Use thermochemical data (Appendix C) to decide whether the equilibrium constant for the following reaction will increase or decrease with temperature. 2NO2(g)+7H2(g)2NH3(g)+4H2O(g)

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?

Using values of fH and S, calculate rG for each of the following reactions at 25 C. (a) 2 Na(s) + 2 H2O() 2 NaOH(aq) + H2(g) (b) 6 C(graphite) + 3 H2(g) C6H6() Which of these reactions is (are) predicted to be product-favored at equilibrium? Are the reactions enthalpy- or entropy-driven?

Calculate G at 355 K for each of the reactions in Question 17. State whether the reactions are spontaneous.

9.83 A student performing a calorimetry experiment combined 100.0 mL of 0.50 M HCl and 100.0 mL of 0.50 M NaOH in a coffee cup calorimeter. Both solutions were initially at 20.0°C, but when the two were mixed, the temperature rose to 23.2°C. (a) Suppose the experiment is repeated in the same calorimeter but this time using 200 mL of 0.50 M HCl and 200.0 mL of 0.50 M NaOH. Will the T observed he greater than, less than, or equal to that in the first experiment, and why? (b) Suppose that the experiment is repeated once again in the same calorimeter, this time using 100 mL of 1.00 M HCl and 100.0 mL of 1.00 M NaOH. Will the T observed he greater than, less than, or equal to that in the first experiment, and why?

Heater Meals are food packages that contain their own heat source, lust pour water into the heater unit, wait a few minutes, and voila! You have a hot meal. Mg(s) + 2 H2O() Mg(OH)2(s) + H2(g) (a) Confirm that this is a product-favored reaction at equilibrium at 25 C. (b) What mass of magnesium is required to produce sufficient energy to heat 225 mL of water (density = 0.995 g/mL) from 25 C to the boiling point?

The equilibrium constant for a reaction is 31015 (a) Without carrying out any calculation, discuss whether ?G° for the reaction is positive or negative. (b) Calculate ?G° for this reaction.

For the reaction TiCl2(s) + Cl2(g) TiCl4(), rG = 272.8 kj/mol-txn. Using this value and other data available in Appendix L, calculate the value of fG for TiCl2(s).