A 1 mole sample of ideal gas expands isothermally at 300 K from a volume of 20.00 L to a volume of 30.00 L. Calculate the ΔG and the ΔS for this process.

The dissolution of ammonium nitrate occurs spontaneously in water at 25 °C. As NH4NO3 dissolves, the temperature of the water decreases . What are the signs of ΔrH, ΔrS, and ΔrG for this process? Note:  Decide thermodynamics aspect (exothermic or endothermic by Temperature change and using sign of Delta T, decide the free energy change

When temperature increases from – 15.0 °C to + 15.0 °C, the thermodynamic equilibrium constant for the reaction increases four times.  Calculate the standard enthalpy for the reaction.

Use the reaction for the formation of NH3 from its elements N2(g) and H2(g) . This reaction has the following thermodynamic data:  ΔfHo (NH3) = - 45.9 kJ/mol and ΔfSo (NH3) = - 99.1 J/mol*K at 298 K a) Write a balanced equation (whole number ratios) for this process and write out the expression for the reaction quotient Q using partial pressures. b) Without doing any calculations, explain how the progression of the reaction will change (more reactants or more products) with respect to 1) increasing temperature, and 2) increasing pressure. c) Calculate the equilibrium constant K at 298 K d) Assuming that : ΔfHo  is independent of temperature, calculate K at - 78o C