The following reaction is at equilibrium:

2R(g) + 3S(g)  2T(g)      llH is negative

which conditions (A-E) would produce most of the product T?

Answer:

6) B

In order to produce more T, we need the forward reaction to occur.

The forward reaction is exothermic since ∆H is negative. This means that the forward reaction releases energy. If we lower the temperature, the forward reaction will be favoured. Therefore, more T will be formed if temperature is low.

A high pressure causes the equilibrium shifts to the side with the lower number of moles. There are 5 moles on the left side and 2 moles on the left side. Therefore a high pressure will favour a higher production of T.

If we add more of the reactants, more products will be formed. If we add R and S, more T will be formed.

So we need the following conditions:

Low temperature, high pressure, add R and S. This corresponds to B.