Answer:
a) T = 298 K
⇒ ΔG° = 173.1 KJ/mol
∴ ΔG° > 0.....the reaction occurs spontaneously in the reverse direction as given.
⇒ K = 4.542 E-31
b) T = 2000 K:
⇒ ΔG° = 1161.745 KJ/mol
ΔG°(2000K) > 0; We confirm that the reaction becomes more spontaneous as the temperature increases.
Explanation:
N2(g) + O2(g) → 2 NO(g)
a) ΔG°(298K) = 2 ΔG°fNO = 2(86.55 KJ/mol)
⇒ ΔG°(298K) = 173.1 KJ/mol
∴ ΔG° > 0.....the reaction is spontaneous
∴ R = 8.314 E-3 KJ/mol.K
⇒ K = e∧(-173.1/(8.314E-3)(298)) = 4.542 E-31
b) T = 2000 K
⇒ ΔG°(2000K) = - (Ln (4.542 E-31))(8.314 E-3 KJ/mol.K)(2000K)
⇒ ΔG°(2000K) = 1161.745 KJ/mol
∴ ΔG°(2000K) > 0; We confirm that the reaction becomes more spontaneous as the temperature increases