A initial mixture containing 3 moles of N2, 1 mole of H2, and 4 moles of...

 

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A initial mixture containing 3 moles of N2, 1 mole of H2, and 4 moles of NH3 is heated to 1200 K and allowed to come into equilibrium at 1 atm total pressure. (a) Write the reaction. (b) Calculate the equilibrium constant for this reaction at 1200 K from the following information: - the enthalpy of formation of NH3(g) at 298K is AH298=-136 kJ/mole - the heat capacities (Cp) of H2 and N2 are 3.5R and that of NH3(g) is 5R - (R = gas constant) The standard entropy of the reaction at 1200 K can be estimated from the "entropy rule- of-thumb" A initial mixture containing 3 moles of N2, 1 mole of H2, and 4 moles of NH3 is heated to 1200 K and allowed to come into equilibrium at 1 atm total pressure. (a) Write the reaction. (b) Calculate the equilibrium constant for this reaction at 1200 K from the following information: - the enthalpy of formation of NH3(g) at 298K is AH298=-136 kJ/mole - the heat capacities (Cp) of H2 and N2 are 3.5R and that of NH3(g) is 5R - (R = gas constant) The standard entropy of the reaction at 1200 K can be estimated from the "entropy rule- of-thumb"