3. How is the equilibrium position of this reaction affected by the following changes?
2802 (g) + O2 (g) <-→ 2 S03(g) + heat
a. Lowering the temperature.
b. Decreasing the pressure
c. Removing oxygen
d. Adding sulfur trioxide (SO3).

Explanation: a) Reaction is exothermic because heat is released

                       If temperature is lowered, amount of products is increased,

                      equilibrium transfers to right

b) If pressure decreases, equilibrium transfers to direction in which amount of gas moles is greater, also in left (reactants)

c) If Oxygen is removed, reaction which produces more oxygen is favoured, also balance changes to reactansts (left)

d) Adding product causes equilibrium transfer to left (reactansts)

answer : one can design an experiment using a liquid and an additive that can be added to the liquid and observe the chemical changes in the reaction species.

one would need a beaker which is filled with a known amount of the liquid in which thermometer is placed to measure the temperature changes; after addition of the additive to the liquid solution one can note down the temperature change and find whether the reaction is endothermic or exothermic in nature. by subtracting the initial temperature value with the final temperature one can find the temperature changes.

various combinations of liquid and additive can be used. liquid in this case can be a known quantity of water and additives can be epsom salt or without epsom salt the experiment can be conducted to notice the changes. water and ice, hydrogen peroxide and dry yeast, vinegar and baking soda,etc.