2 NEXT > In a 1.0 L container at high temperature, 0.20 mol N₂ and 0.15 mol O₂ are allowed to react. Set up the expression for Qc. Each reaction participant must be represented by one tile. Do not combine terms. Once the expression is constructed, solve for Qc to determine the direction of the reaction. Qc N₂(g) + O₂(g) = 2 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.
![Predict the equilibrium concentration of O₂ in the reaction described below by
constructing an equilibrium expression for Qc, constructing an ICE table, writing an
equilibrium expression for Kc, and solving for the equilibrium concentration. Complete
Parts 1-4 before submitting your answer.
N₂(g) + O₂(g) = 2 NO(g)
4
NEXT >
In a 1.0 L container at high temperature, 0.20 mol N₂ and 0.15 mol O₂ are allowed to react. Set up the
expression for Qc. Each reaction participant must be represented by one tile. Do not combine terms.
Once the expression is constructed, solve for Qc to determine the direction of the reaction.
[0]
[0.050]
0.030
[1.0]
[0.201²
1
9.0 x 10-4
Qc
=
[0]²
[0.15]²
1.1 x 104
2
[1.01²
[0.40]²
[0.20]
[0.30]²
3
[0.15]
[0.050]²
[0.40]
0
✓ RESET
[0.30]
33](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1f7ea230-2d40-478d-b19d-f38aba3f28c1%2Fd470b559-6afb-4ede-ab8a-9679c7dd9098%2Fyqg33c_processed.png&w=3840&q=75)
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