For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction C₂H(g) + H₂(g) = 2 CH₂(g) the standard change in Gibbs free energy is AG° = -72.6 kJ/mol. What is AG for this reaction at 298 K when the partial pressures are PC₂H₂ = 0.100 atm, PH₂ = 0.200 atm, and PCH, = 0.600 atm? AG= 7.0885 Incorrect kJ/mol

For a certain chemical reaction, the standard Gibbs free energy of reaction at  15.0   °C  is  147.   kJ . Calculate the equilibrium constant  K  for this reaction.Round your answer to  2  significant digits.

For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction N, (g) + 3 H, (g) 2 NH,(g) the standard change in Gibbs free energy is AG° = -32.8 kJ/mol. What is AG for this reaction at 298 K when the partial pressures are PN, = 0.500 atm, Pi, = 0.100 atm, and PNH, = 0.600 atm? AG = kJ/mol

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

For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction N₂(g) + 3 H₂(g) ⇒ 2NH₂(g) the standard change in Gibbs free energy is AG° = −32.8 kJ/mol. What is AG for this reaction at 298 K when the partial pressures are PN₂ = 0.100 atm, PH₂ = 0.100 atm, and PNH₂ = 0.750 atm? AG = 737 kJ/mol

A student determines the value of the equilibrium constant to be 2.69×10-10 for the following reaction.Fe2O3(s) + 3H2(g)2Fe(s) + 3H2O(g)Based on this value of Keq:G° for this reaction is expected to be (greater, less) fill in the blank than zero.Calculate the free energy change for the reaction of 2.05 moles of Fe2O3(s) at standard conditions at 298K.     G°rxn =  ____kJ

The standard reaction free energy AG° = 29. kJ for this reaction: Fe2O3(g) + 2H2 (g) --> 2 Fe(s) + 3H2O(l) Use this information to complete the table below. Round each of your answers to the nearest kJ.

For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction C₂H(g) + H₂(g) = 2 CH₂(g) the standard change in Gibbs free energy is AG° = -69.0 kJ/mol. What is AG for this reaction at 298 K when the partial pressures are PC₂H₂ = 0.350 atm, PH₂ = 0.500 atm, and PCH, = 0.950 atm? AG = kJ/mol

For a certain chemical reaction, the standard Gibbs free energy of reaction is - 149. kJ. Calculate the temperature at which the equilibrium constant K = 1.3 × 1026. Round your answer to the nearest degree. T=