Balance each equation, predict the sign of ΔS°rxn if possible, and calculate its value at 298 K:

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.

A helium-filled balloon at 1.00 atm pressure has a volume of 1.200 L. It is placed in a freezer and its volume decreases, stopping at 1.010 L.  (Assume that the static internal and external pressures are equal, that the balloon contains only helium, and helium behaves as an ideal gas.)  Calculate ΔE for the gas in the balloon.

Calculate ΔG°rxn, ΔH°rxn, and ΔS°rxn of the following reaction: 2O3(g) -> 3O2(g)

Under the conditions shown below for the following reaction. Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g) AG° = -28.0 kJ P(CO) = 4.2 atm, P(CO2) = 1.8 atm Calculate AGrxn at 298 K, and indicate if the reaction is more or less spontaneous under these conditions than under standard conditions?

Answer this question without using numbers from the book (or anywhere else!) ΔS for the following reaction is negative. True or false?   2 CO(g) + O2(g) → 2 CO2(g)

Consider each of the following thermodynamic quantities, and give the appropriate sign of each as positive, negative, zero, or undetermined.  ΔHorxn for the combustion of a hydrocarbon. So for any element in its standard state at 1 atm and 298 K.   ΔHof for any element in its standard state at 1 atm and 298 K.  ΔSosystem for a spontaneous process.

What is the standard free-energy change ΔG° at 25°C for the following reaction? See the Supplemental Data for ΔGf° data. C(graphite) + 2 Cl2(g) → CCl4(l)   A)  kJ/molB) Calculate the value of the thermodynamic equilibrium constant

Which pure substance under standard conditions would have the highest entropy?   O2   HCl   CH3OH   S