CoH12 (1) + 902 (g) 6CO:(g) + 6H;O() For CeH12(0), AH; =- 151.9 kJ/mol. AH; (CO,,g)=-393.5kJ / mol AH; (H,0,1)=-285.8kJ / mol. Molecular oxygen (O2) is a stable allotrope of oxygen. (ii)From the following data, C(graphite) + O2(g) → CO2(9) AHm = -393.5 kJ/mol H2(g) + | 0:(9) → H¿O(1) AH,, = -285.8 kJ/mol 2C;Hs (9) + 70:(9) → 4CO2(g) + 6H;O() AHm =-3119.6 kJ/mol calculate the enthalpy change for the reaction 2C(graphite) + 3H2(9) → C;H«(g) (b) Consider this reaction: 2CH;OH() + 302 → 4H;0() + 2CO2(9) AH = - 1452.8 kJ/mol What is the value of AH if (i) the equation is multiplied throughout by 2, (ii) the direction of the reaction is reversed so that the products become the reactants and vice versa, (ii) water vapor instead of liquid water is formed as the product? Hint: 2H,0(I) –→ 2H,0(g) AH = 88.0kJ / 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.
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