Malachite is a green copper mineral with the formula Cu₂CO3(OH)2. It can be converted into copper metal in a number of ways. One method extracts the metal by reacting the malachite with sulfuric acid to form CuSO4, and then adding iron to the CuSO4 solution which, after they react, forms FeSO4 and copper metal. The balanced chemical reactions are: Cu₂CO3(OH)2 (s) + 2 H₂SO4 (aq) →2 CuSO4 (aq) + 3 H₂O (1) + CO₂(g) CuSO4 (aq) + Fe (s) FeSO4 (aq) + Cu (s) If the final solution is dried, and 3.28 g of iron sulfate is collected, how many grams of malachite were originally used? i Hint Save for Later ! g of malachite were originally used. Assistance Used Attempts: 1 of 3 used Submit Answer
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.
Given that,
Malachite reacts with H2SO4 to form CuSO4
Cu2CO3(OH)2 + 2H2SO4 2CuSO4 + 3H2O + CO2
On adding iron metal to CuSO4 forms FeSO4 and Cu metal
CuSO4 + Fe FeSO4 + Cu
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