The reaction below is at equilibrium at a temperature t. there are four possible changes listed. select all the changes that will shift the equilibrium so as to produce more products
mgo(s) + so3(g) + 95 kj < > mgso4(s)
i – increase the temperature
ii – increase the volume
iii – add more mgo
iv – remove so3

(a) i and iii
(b) i
(c) i, ii and iii
(d) i, ii, iii and iv

The correct answer is B.

Explanation:

Heterogeneous equilibrium is that in which reagents and products are present in more than one phase.

When the reaction is carried out in a closed container, three equilibrium phases are present: solid magnesium oxide, solid magnesium sulfate and gaseous sulfur trioxide.

Hence, the equilibrium contant is given by:

The concentrations in the equilibrium equation are the relationships of the real concentrations between the concentrations in the standard state. Since the standard state of a pure solid is the pure solid itself, the ratio of concentrations for a pure solid is equal to one.

Now, we analyse each statement:

I) As the reaction is endothermic (ΔH>0), increasing the temperature shifts the balance to the right because excess heat will be used to form more products.

II) Increasing the volume will decrease the concentration of SO₃, so Q>K and then this shifts the balance to the left.

III) As it is a heterogeneous balance, adding MgO will not affect the balance.

IV) Removing SO3 will decrease its concentration and therefore the reaction equilibrium will shift to the left.

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