Ammonia gas is formed from hydrogen gas and nitrogen gas according to the following chemical reaction: 3 H2(g) + N2(g) --> 2 NH3(g) ΔH = - 92.4 kJ/rxn Calculate the total energy released (in kJ) if one mole of ammonia gas is formed. Calculate the total energy released (in kJ) if six moles of hydrogen gas and two moles of nitrogen gas are combined and the above reaction occurs. Calculate the total energy released (in kJ) if you combine 6.00 g of hydrogen gas and 24.00 g of nitrogen gas and the above reaction occurs.
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.
Ammonia gas is formed from hydrogen gas and nitrogen gas according to the following
3 H2(g) + N2(g) --> 2 NH3(g) ΔH = - 92.4 kJ/rxn
- Calculate the total energy released (in kJ) if one mole of ammonia gas is formed.
- Calculate the total energy released (in kJ) if six moles of hydrogen gas and two moles of nitrogen gas are combined and the above reaction occurs.
- Calculate the total energy released (in kJ) if you combine 6.00 g of hydrogen gas and 24.00 g of nitrogen gas and the above reaction occurs.
- Which is more likely to be
thermodynamically favored, the forward reaction or the reverse reaction? Why?
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