Sulphuric acid can be prepared by burning sulphur in oxygen (equation 1), then oxidize the sulphur di-oxide gas that formed in the presence of a catalyst to sulphur tri-oxide gas (equation 2) and then lastly absorb the sulphur tri-oxide gas in water (equation 3). Equation 1: S (s) + O2 (g) → SO2 (g) Equation 2: 2SO2 (g) + O2 (g) → 2SO3 (g) Equation 3: SO3 (g) + H2O (liq.) → H2SO4 (aq) Calculate the mass of sulphuric acid (in kg) that can be prepared from 10 kg of sulphur. Then calculate the volume of sulphuric acid (in dm3; density of sulphuric acid = 1.83 g/cm3). Lastly also calculate the mass of oxygen (in kg) that is nessessary for the formation of sulphuric acid from elemental sulphur.
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
Sulphuric acid can be prepared by burning sulphur in oxygen (equation 1), then oxidize the sulphur di-oxide gas that formed in the presence of a catalyst to sulphur tri-oxide gas (equation 2) and then lastly absorb the sulphur tri-oxide gas in water (equation 3).
Equation 1: S (s) + O2 (g) → SO2 (g)
Equation 2: 2SO2 (g) + O2 (g) → 2SO3 (g)
Equation 3: SO3 (g) + H2O (liq.) → H2SO4 (aq)
Calculate the mass of sulphuric acid (in kg) that can be prepared from 10 kg of sulphur. Then calculate the volume of sulphuric acid (in dm3; density of sulphuric acid = 1.83 g/cm3). Lastly also calculate the mass of oxygen (in kg) that is nessessary for the formation of sulphuric acid from elemental sulphur.
Step by step
Solved in 3 steps with 3 images
