Use the set of three reactions shown below to answer the questions that follow.2NO(g) + O2(g) → 2NO2(g) ΔH = -116 kJ2N2(g) + 5O2(g) + 2H2O(l) → 4HNO3(aq) ΔH = -256 kJN2(g) + O2(g) → 2NO(g) ΔH = +183 kJIf 57.4 g of NO g is reacted with excess oxygen, how much heat energy is produced? What mass of liquid water will be consumed during the production of 39600 J of energy assuming that there is excess nitrogen and oxygen? Determine the heat of reaction in kJ for the reaction below.3NO2(g) + H2O(l) → 2HNO3(aq) + NO(g)
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.
Use the set of three reactions shown below to answer the questions that follow.
2NO(g) + O2(g) → 2NO2(g) ΔH = -116 kJ
2N2(g) + 5O2(g) + 2H2O(l) → 4HNO3(aq) ΔH = -256 kJ
N2(g) + O2(g) → 2NO(g) ΔH = +183 kJ
If 57.4 g of NO g is reacted with excess oxygen, how much heat energy is produced?
What mass of liquid water will be consumed during the production of 39600 J of energy assuming that there is excess nitrogen and oxygen?
Determine the heat of reaction in kJ for the reaction below.
3NO2(g) + H2O(l) → 2HNO3(aq) + NO(g)
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