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.

the answer is the

they are made of gases.

they have a spherical shape.

they make energy through fusion.