alculate ΔGmix for the following mixtures at 298 K and 1.00 atm,, assuming these gases behave as ideal gases. 6.00 moles of N2,and 7.00 moles of O2 7.00 moles of CO2and 7.00 moles of N2 How do the two values compare? What does this tell us about ΔGmix?

For a chemical reaction that has a ∆Go value of +24 kJ/mol, what value must Q have for this system to be at equilibrium

For a particular reaction at 180.9 °C, AG = 527.78 kJ/mol, and AS = 953.96 J/(mol · K). Calculate AG for this reaction at -3.7 °C. AG = kJ/mol

Given the values of AH, ASn, and T, determine ASuniy and predict whether or not each reaction is spontaneous. (Assume that all reactants and products are in their standard states.) a. AH = -95 kJ; AS;n = -157 J/K; T = 298 K b. AH = -95 kJ; AS"n = -157 J/K; T = 855 K Calculate the Gibbs free energy for the above sets (a) and (b)

Two different gases occupy the two bulbs shown here. Consider the process that occurs when the stopcock is opened, assuming the gases behave ideally. Predict the signs of ∆H and ∆S for the process.

What is entropy, and what is ΔS for a reaction, and what does it mean if ΔS is positive or negative?

Consider the reaction below for the decomposition of carbon tetrachloride gas:  CCl4(g)    ------>     C(s)     +        2Cl2 (g)    ΔH = + 95.7 kJ;  ΔS = + 142.2 J/K  If the reaction above is not spontaneous at 25 oC, determine at what temperature (if any) the reaction becomes spontaneous.