Consider the formation of NO(g) from its elements. N₂(g) + O₂(g) ⇄ 2 NO(g)
(a) Calculate K_p at 25°C. Is the reaction product favored at equilibrium at this temperature?
(b) Assuming Δ_r H° and Δ_r S° are nearly constant with temperature, calculate Δ_rG° at 700°C. Estimate K_p from the new value of Δ_rG° at 700°C. Is the reaction product-favored at equilibrium at 700°C?
(c) Using K_p at 700°C, calculate the equilibrium partial pressures of the three gases if you mix 1.00 bar each of N₂ and O₂.