For each of the following reactions write the correct expression for KC. For Kp, either write the correct expression or put n/a (not available) if there is no correct expression. a) N2(g) + O2(g) ⇋ 2 NO(g) (1.1) b) Fe2O3(s) + 3 CO(gas) ⇋ 2 Fe(ℓ) + 3 CO2(g) (1.2) c) CH3Cl(aq) + OH-(aq) ⇋ CH3OH(aq) + Cl-(aq
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.
For each of the following reactions write the correct expression for KC. For Kp, either write the correct
expression or put n/a (not available) if there is no correct expression.
a) N2(g) + O2(g) ⇋ 2 NO(g) (1.1)
b) Fe2O3(s) + 3 CO(gas) ⇋ 2 Fe(ℓ) + 3 CO2(g) (1.2)
c) CH3Cl(aq) + OH-(aq) ⇋ CH3OH(aq) + Cl-(aq) (1.3)
Equilibrium constant, Kc for a reaction is defined as the product of the molar concentrations of the products, each raised to the power equal to a stoichiometric coefficient divided by the product of the molar concentrations of the reactant each raised to the power equal to its stoichiometric coefficient .
& the most important convention to be kept in mind is that the active mass of a pure solid or pure liquid is considered to be constant.
Equilibrium constant, Kp for a reaction is defined as the product of the partial pressure of the products, each raised to the power equal to a stoichiometric coefficient divided by the product of the partial pressure of the reactant each raised to the power equal to its stoichiometric coefficient .
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