1. Calculate the enthalpy for this reaction: 3NO 2 (g) + H 2 O(ℓ) ---> 2HNO 3 (aq) + NO(g) given the following thermochemical equations: 2NO (g) + O 2(g) 2NO 2(g) ΔH o f = ─ 116 kJ 2N 2(g) + 5O 2(g) + 2H 2 O (l ) 4HNO 3(aq) ΔH o f = ─ 256 kJ N 2(g) + O 2(g) 2NO (g) ΔH o f = 183 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.
1. Calculate the enthalpy for this reaction: 3NO 2 (g) + H 2 O(ℓ) ---> 2HNO 3 (aq) + NO(g)
given the following thermochemical equations:
2NO (g) + O 2(g) 2NO 2(g) ΔH o f = ─ 116 kJ
2N 2(g) + 5O 2(g) + 2H 2 O (l ) 4HNO 3(aq) ΔH o f = ─ 256 kJ
N 2(g) + O 2(g) 2NO (g) ΔH o f = 183 kJ
2.Calculate the enthalpy for this reaction: 2C (s) + H 2(g) ---> C 2 H 2(g) given the following thermochemical
equations:
C 2 H 2(g) + O 2(g) 2CO 2(g) + H 2 O (l) ΔH 0 f = – 1299.5 kJ
C (s) + O 2(g) CO 2(g) ΔH 0 f = – 393.5 kJ
H 2(g) + O 2(g) H 2 O (l) ΔH 0 f = –285.8kJ
3.
A key step in the production of sulfuric acid is the oxidation of SO 2(g) to SO 3(g) :
2 SO 2(g) + O 2(g) 2 SO 3(g)
4. Calculate ΔG 0 for the combustion of 1 mol ethanol, C 2 H 5 OH.
C 2 H 5 OH (l) + 3O 2(g) . 2CO 2(g) + 3H 2 O (g)
The standard free energies of formation are: ΔG 0 f of C 2 H 5 OH.=-174.8 kJ , ΔG 0 f of O 2(g) = 0,
ΔG 0 f of CO 2(g) = -394.4 kJ, ΔG 0 f of H 2 O (g) = -228.6 kJ
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