The Haber-Bosch process is used to produce ammonia. First methane is converted into CO and hydrogen, and then the H is used in the following reaction (all in the gas phase) From tables we find that GENH3(298 K) = -16,450 J/mol, and HNH(298 K) = -46,110 J/mol. We will assume that the heat of reaction remains constant with temperature, for this problem. Typical operating conditions are high pressure and T = 400 C = 673 K, but for this problem we will let the system pressure P = 10 bar. Starting with 5.0 mol N, 7.0 mol H, and 1.5 mol NH3, provide the values below. answer: nN = YN2 N = 5.311 mol, 7.94 mol, nNH3 = 0.874 mol AG= AH = K(298 K)= K(673 K) = mol N5 = mol H = N + 3H = 2NH3 mol NH3 = J/mol of N consumed J/mol of N consumed mol mol mol If order to increase the yield of ammonia, we should make P (higher) / (lower)?