Question

Consider the reaction N2(g) + 2O2(g) 2NO2(g) Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K ANSWER:

Answer 1

The following reaction is given: N, (8)+20, (g) 2NO2(g) Determine Gibs free energy as shown eow: product-〉 G reactanit = [2x 5 1.29 kJinol]-[ 2x0 kJ/mo1+ 0 kJ/mol -102.58 k.J/mol The relation between ΔGo and equilibrium constant K is given below: AGRTInK Here, R is the universal gas constant; T is the temperature and K is the equilibrium constant Determine the value of K at 535 K as shown below: 102.58 kJ/mo!=-8314 J/mol . Kx535 Kxln (K) kJ 1000 J 102.58 kJ/mol 2478.8 J/molx xIn (K) -41.38 kJ/mol ln (K) K-1.06 x10-18 Hence, the value of K for reaction (1) is 1.06x10-15

The following reaction is given: NH,Cl (aq)NH, (g)+ HCl (aq) Determine Gibbs free energy as shown eow: AGo Gxoduct Greactant -13125 kJ/mol-16.48 kJ/ml-210.62 kJ/mol -342.87 kJ/mol The relation between AG° and equilibrium constant K is given below Here, R is the universal gas constant; T is the temperature and K is the equilibrium constant. Determine the value of K at 535 K as shown below: -342.87 k.J/mol -8.314 J/mol.Kx298.15 Kx In (K) -342.87 kJ/mol 2478.8 J/molx xIn (K kJ 1000 J 138.32 kJ/mol ln (K) K-118x1060 Hence, the value of K for reaction (2) is 1.18x100