If you have 35.67g of Copper (II) Sulfate how many grams of just copper are present? Convert 35.67g of Copper (II) Sulfate into mols . Convert 35.67g of Copper (II) Sulfate into molecules of Copper (II) Sulfate.
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.
Mass of Copper(II) sulfate = 35.67 grams
For determination of number of grams of Copper present in 35.67 g of Copper(II) sulfate we determine the molar mass of Copper(II) sulfate .
The molecular formula of Copper(II) sulfate is CuSO4.
Molar mass of CuSO4 is :
Therefore molar mass of CuSO4 is 159.607 grams.
There is one Cu atom present in CuSO4. So, if 159.607 grams of CuSO4 contains 63.546 grams of Copper then 35.67 grams of CuSO4 will contain is given by:
Therefore, 35.67 g of CuSO4 contains 14.20 grams of Copper.
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