Sulfur dioxide, SO2(g), can react with oxygen to produce sulfur trioxide, SO2(g), by the reaction 2SO2(g) + O2(g)2 → SO3(g)

The standard enthalpies of formation for SO2(g) and SO3(g) are

ΔHf= [SO2(g)] = -296.8 kJ/mol
ΔHf= [SO2(g)] = -395.7 kJ/mol

Calculate the amount of energy in the form of heat that is produced when a volume of 1.64 L of SO2(g) is converted to 1.64 L of SO3(g) according to this process at a constant pressure and temperature of 1.00 bar and 25.0 °C . Assume ideal gas behavior.

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.