Question

Calorimetric studies show that the reaction is exothermic. 2NO2(g) N2O4(g) + 14.1 kcal. Based on this information, which one--if any--of the following additional changes would increase the molar concentration at equilibrium of N2O4(g)?

Answer 1

The reaction in consideration is
\(2NO_{2}(g)\rightarrow N_2O_4(g)\)
and since it is exothermic, \(∆H<0\) and hence Heat is a product
\(2NO_{2}(g)\rightarrow N_2O_4(g)+\text{Heat}\)

You can employ the Le Chatelier's Principle to understand how to shift the equilibrium to the products, and hence, increase the equilibrium concentration of N2O4(g).
-You can disturb the products (i.e., increase or decrease the concentration of reactants)
-You can disturb the temperature (recall you can consider Heat as another compound)
-You can disturb the pressure (and inversely, the volume). Remember the rule for this, by comparing the mols of products and reactants on either side.

Tell me how can you increase the products, given that the above are the methods?