Consider the following reversible reaction 2NO(g) ⇌ N2(g) + O2(g) ΔH = -183 kJ that has an equilibrium constant (Kc) value of 20.25 at a certain high temperature T: a) Write the equilibrium constant expression for the reaction - Leaving Cert Chemistry - Question 9 - 2014

Given the reaction:

2NO(g) ⇌ N2(g) + O2(g)

If 2 moles of NO are decomposed, using stoichiometry:

• 2 moles of NO produce 1 mole of N2.

Thus, when 2 moles of NO decompose, the number of moles of nitrogen gas (N2) produced will be:

$N_2 = \frac{2}{2} = 1 \text{ mole}$

Le Chatelier's principle states that if an external change is applied to a system at equilibrium, the equilibrium will shift in such a way as to counteract that change. In other words, the system will adjust its position of equilibrium to minimize the effect of the change.

In catalytic converters, the type of catalysts used is typically precious metals such as platinum, palladium, and rhodium. These metals facilitate the chemical reactions involved in converting harmful exhaust gases into less harmful emissions.

Catalysts in catalytic converters primarily operate through heterogeneous catalysis, where the solid catalyst surface interacts with gaseous reactants. This allows for active sites on the catalyst to adsorb reactants, effectively lowering the activation energy needed for reactions to occur.

Lead compounds are known to poison catalytic converters. The presence of lead in fuel can coat the catalysts and block active sites, significantly reducing their effectiveness in catalyzing the necessary reactions.