The thermochemical equation showing the formation of ammonia (NH3) from its elements is: N2 (g) + 3 H2 (g) —> 2 NH3 (g) ΔH = -92 kJ This equation shows that 92 kJ of heat is: a. Lost to the surroundings when one mole of hydrogen is used up in the reaction. b. Absorbed from the surroundings when one mole of nitrogen reacts. c. Absorbed from the surroundings when one mole of ammonia is formed. d. Lost to the surroundings when 2 moles of ammonia is formed.
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.
Trending now
This is a popular solution!
Step by step
Solved in 2 steps
