Given these three reactions and their Δ?∘ values reaction 1: C(s)+2H2(g)⟶CH4(g) Δ?∘1=−74.6 kJ/mol reaction 2: C(s)+2Cl2(g)⟶CCl4(g) Δ?∘2=−103 kJ/mol reaction3: H2(g)+Cl2(g)⟶2HCl(g) Δ?∘3=−184.6 kJ/mol calculate the value of Δ?∘rxn for the following reaction. CH4(g)+4Cl2(g)⟶CCl4(g)+4HCl(g) Δ?∘rxn=? kJ/mol 1. −547 kJ/mol−547 kJ/mol 2. −362 kJ/mol−362 kJ/mol 3. −213 kJ/mol−213 kJ/mol 4. −398 kJ/mol
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 these three reactions and their Δ?∘ values
reaction 1: C(s)+2H2(g)⟶CH4(g) Δ?∘1=−74.6 kJ/mol
reaction 2: C(s)+2Cl2(g)⟶CCl4(g) Δ?∘2=−103 kJ/mol
reaction3: H2(g)+Cl2(g)⟶2HCl(g) Δ?∘3=−184.6 kJ/mol
calculate the value of Δ?∘rxn for the following reaction.
CH4(g)+4Cl2(g)⟶CCl4(g)+4HCl(g) Δ?∘rxn=? kJ/mol
1. −547 kJ/mol−547 kJ/mol
2. −362 kJ/mol−362 kJ/mol
3. −213 kJ/mol−213 kJ/mol
4. −398 kJ/mol
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