Determine the free energy (in kJ/mol) for the decomposition of ammonia at 25.0 °C when
the partial pressures are PN2 = 0.87 atm, PH2 = 0.25 atm and PNH3 = 12.9 atm, and ΔG°rxn
-1 =33.0kJmol .
Calculate the vapor pressure (in Torr) of mercury under standard conditions. Use Appendix D to look up the required standard thermodynamic values. (Recall the pressure conversions: 1 atm = 1.01325 bar = 1.01325x105 Pa = 760 Torr)
Benzene has a vapor pressure of 75.0 Torr at 22.0 °C and an enthalpy of evaporation of
-1 o
33.9 kJ mol . Calculate the temperature (in C) when the vapor
pressure will reach 248.3
Torr.
Determine the free energy (in kJ/mol) for the decomposition of ammonia at 25.0 °C when the...
1. Ice melts at 0C° with an enthalpy of fusion = 6.01 kJ mol-1 . An ice cube with a mass of 20.0g is placed inside an incubator at 40.0C°. Determine the total entropy change (in J/K) of this system. 2. Calculate the total entropy change (in J/K) when 50.0 g of H2 gas initially in a tank at a pressure of 145 psi is withdrawn from the tank under a constant pressure of 23.0 psi at standard room temperature....
Benzene has a vapor pressure of 75.0 Torr at 22.0 °C and an enthalpy of evaporation of 33.9 kJ mol-1. Calculate the temperature difference (in oC) when the vapor pressure reaches 248.3 Torr. Please answer in full solutions. Thank you!
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction N2 (g) + 3H2(g) -------> 2NH3(g) the standard change in Gibbs free energy is ΔG° = -72.6 kJ/mol. What is ΔG for this reaction at 298 K when the partial pressures are PN2 = 0.200 atm PH2 = 0.350 atm PNH3 = 0.850
AGº is -32.7 kJ/mol of N2 for the reaction N2 (g) + 3H2 (g) = 2NH3(g) This calculation was for the reaction under standard conditions—that is, with all gases present at a partial pressure of 1 atm and a temperature of 25°C. Calculate AG for the same reaction under the following nonstandard conditions: . PN2 = 2.00 atm, PH2 = 7.00 atm, PNH3 = 0.021 atm, . and T = 100°C.