In a certain experiment, 0.7000 mol of hydrogen gas reacted with 0.7000 mol of solid iodine at a constant 1 atm pressure, producing 1.4000 mol of solid hydrogen iodide and absorbing 36.9 kJ of heat in the process. Which of the following thermochemical equations correctly describes this experiment? a. H2(g) + I2(s) → 2HI(s); ΔH° = –52.72 kJ b. H2(g) + I2(s) → 2HI(s); ΔH° = 36.9 kJ c. H2(g) + I2(s) → 2HI(s); ΔH° = –36.9 kJ d. H2(g) + I2(s) → 2HI(s); ΔH° = 73.8 kJ e. H2(g) + I2(s) → 2HI(s); ΔH° = 52.72 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.
In a certain experiment, 0.7000 mol of hydrogen gas reacted with 0.7000 mol of solid
iodine at a constant 1 atm pressure, producing 1.4000 mol of solid hydrogen iodide and
absorbing 36.9 kJ of heat in the process. Which of the following thermochemical
equations correctly describes this experiment?
a. H2(g) + I2(s) → 2HI(s); ΔH° = –52.72 kJ
b. H2(g) + I2(s) → 2HI(s); ΔH° = 36.9 kJ
c. H2(g) + I2(s) → 2HI(s); ΔH° = –36.9 kJ
d. H2(g) + I2(s) → 2HI(s); ΔH° = 73.8 kJ
e. H2(g) + I2(s) → 2HI(s); ΔH° = 52.72 kJ
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