Calculate the ΔS°rxn of the following reaction at 223°C and standard pressure. =_____J/mol•K

For the reactionHCl(g) + NH3(g)NH4Cl(s)ΔG° = -98.5 kJ and ΔS° = -284.8 J/K at 272 K and 1 atm.The maximum amount of work that could be done by this reaction when 2.41 moles of HCl(g) react at standard conditions at this temperature is  kJ. --- For the reaction2H2S(g) + 3O2(g)2H2O(l) + 2SO2(g)ΔH° = -1124.0 kJ and ΔS° = -390.7 J/KThe maximum amount of work that could be done when 1.68 moles of H2S(g) react at 252 K, 1 atm is  kJ.Assume that ΔH° and ΔS° are independent of temperature.

What is the equilibrium constant for a reaction that has a ΔGrxn of -11.1 kJ at a temperature of 38.1 °C?  (Give your answer to 3 significant figures)

Consider the reaction CH4(g) + H₂O(g) 3H₂(g) + CO(g) Calculate the standard Gibbs free energy change for this reaction at 25°C from AH°rxn kJ/mol AG rxn and AS°rxn-

For the following reaction, calculate the a.ΔrxnH, b.ΔrxnS, c. ΔrxnG (25°C) of the following reaction. state whether or not the reaction is spontaneous H2 (g) + I2 (s) --> 2 HI (g)

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Using the values provided in the table below, calculate ΔHr for the following reaction: 2CO2(g) + 4H2O(g) → 2CH3OH(l) + 3O2(g)  a. -2158 kJ mol–1 b. 1354 kJ mol–1 c. -402 kJ mol–1 d. -435 kJ mol–1 e. -1354 kJ mol–1

Using enthalpies of formation, calculate deltaH for the following reaction at 25°C. Also calculate deltaS for this reaction from standard entropies at 25°C. Use these values to calculate deltaG for the reaction at this temperature. Species  deltaHf(kJ/mol)  S(J/mol⋅K) CH3OH(l) –238.7 126.8 O2(g) 0 205.0 CO2(g) –393.5 213.7 H2O(l) –285.8 69.95 2CH3OH(l) +3O2(g) --- 2CO2(g) + 4H2O(l) deltaH =  kJ deltaS =  J/K deltaG =  kJ

Determine AG for a reaction when AG = -141.5 kJ/mol and Q = 35 at 325 K. (R = 8.314 J/mol. K)

2. For the following reaction at 25°C, AG° is -118.4 kJ. At what pressure of O2 gas does AG = 0 at 25°C? 2 KCIO3 (s) + 2 KCI (s) + 3 O2 (g)