1. Calculate the value of ΔG˚, in kJ/molrxn, for the reaction at 298 K. 2. Given that the value of ΔH˚ for the reaction at 298 K is +105 kJ/molrxn, calculate the value of ΔS˚ for the reaction at 298 K. Include units with your answer.

ΔG= ΔH-TΔS If ΔH=0, what does this mean regarding to the ΔS  if the ΔG for the reaction is +3.4 kJ/mol?

What is the ΔG of a reaction if ΔH is 129.2 kJ and ΔS is 324.1 J/K when the reaction takes place at 316.9 K?     102800 kJ     26.49 kJ     231.9 kJ     -102600 kJ     -129.2 kJ

The free energy change is related to the enthalpy change and the entropy change: ΔG = ΔH – T ΔS.   What is ΔS for reaction 3?    Question 8 options:   –200 J mol–1 K–1   400 J mol–1 K–1   200 J mol–1 K–1

For each of the following reactions, calculate ΔH∘rxn, ΔS∘rxn, and ΔG∘rxn at 25 ∘C. State whether or not the reaction is spontaneous. If the reaction is not spontaneous, would a change in temperature make it spontaneous? If so, should the temperature be raised or lowered from 25 ∘C?2CH4(g)→C2H6(g)+H2(g), Calculate ΔS∘rxn at 25 ∘C. 2NH3(g)→N2H4(g)+H2(g) Calculate ΔS∘rxn at 25 ∘C. N2(g)+O2(g)→2NO(g) Calculate ΔS∘rxn at 25 ∘C. 2KClO3(s)→2KCl(s)+3O2(g) Calculate ΔS∘rxn at 25 ∘C.

A certain reaction is spontaneous at 65 ° C. If the enthalpy change for the reaction is  15 kJ/mol,  what is the minimum value of  Δ S (in J/K · mol) for the reaction.

From the values of ΔH and ΔS calculate the minimum temperature at which each reaction will become spontaneous. Enter "None" if the reaction is not spontaneous at any temperature. ΔH = -389 kJ/mol,  ΔS = 27.8  J/K · mol

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

The element gallium (Ga) freezes at 29.8°C its ΔHfus = 5.59 kJ/ mol. Calculate the valueof ΔS when 1.0 mol gallium freezes at its normal melting point. Is ΔS positive ornegative? Calculate the value of ΔS when 30.0 g of Ga(l) solidifies at 29.8 °C

For a given reaction, ΔH∘∘= +35.5 kJ/mol and ΔS∘∘= +83.6 J/(K∙∙ mol). In what temperature range is the reaction spontaneous? Assume that ΔH∘∘ and ΔS∘∘ do not vary with temperature.