NO(g) + CO(g) ↔ (1)/(2)N2(g) + CO2(g) ∆H = -89.3 kj. What conditions would favour maximum conversion of nitrogen (II) oxide and carbon (II) oxide in the rea...

NO(g) + CO(g) ↔ (1)/(2)N2(g) + CO2(g) ∆H = -89.3 kj.

What conditions would favour maximum conversion of nitrogen (II) oxide and carbon (II) oxide in the reaction above?

Answer Details

The given reaction is exothermic, which means it releases heat when the reaction proceeds. According to Le Chatelier's principle, increasing the pressure and decreasing the temperature favors the reaction that produces fewer moles of gas. In this case, the reaction produces 2 moles of gas (N2 and CO2) from 2 moles of gas (NO and CO). So, decreasing the temperature and increasing the pressure will shift the equilibrium towards the side with fewer moles of gas, i.e., the forward reaction. Therefore, the conditions that would favor maximum conversion of nitrogen (II) oxide and carbon (II) oxide are low temperature and high pressure. Hence, the correct answer is: Low temperature and high pressure.