Given the following enthalpies of reaction: C + O2 ---> CO2 ΔH = -393.5 kJ H2 + 1/2 O2 ---> H2O ΔH = -285.8 kJ 2C2H6 + 7O2 ---> 4CO2 + 6H2O ΔH = -3119.6 kJ Use the law of Hess to calculat the enthalpy change for the reaction: 2C + 3H2 ---> C2H6 ΔH = ? A. +1559.8 kJ B. -84.6 kJ C. +787 kJ D. -156.3 kJ
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 the following enthalpies of reaction:
C + O2 ---> CO2 ΔH = -393.5 kJ
H2 + 1/2 O2 ---> H2O ΔH = -285.8 kJ
2C2H6 + 7O2 ---> 4CO2 + 6H2O ΔH = -3119.6 kJ
Use the law of Hess to calculat the enthalpy change for the reaction: 2C +
3H2 ---> C2H6 ΔH = ?
A. +1559.8 kJ
B. -84.6 kJ
C. +787 kJ
D. -156.3 kJ
Answer:-
This question is answered by using the simple concept of Hess law of constant heat change whether a reaction takes place in single step of a number of steps.
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