Humans are heterotrophs that consume food for energy. These foods comprise of sugars that are broken down by enzymic activity within the body for producing energy. This process, called cellular respiration, occurs according to the chemical equation: C6H12O6(aq) + 6O2(g) 6CO2(g) + 6H2O(l) ΔH = –2802.7 kJ mol –1 a) Write an expression for the equilibrium constant for this reaction. b) At equilibrium, the concentration of the reactants and products are determined as [CO2] = 0.30 M, [O2] = 0.040 M and [C6H12O6] = 0.065 M. Determine the value of the equilibrium constant (Kc) and predict the whether the products or reactants will be favoured at equilibrium. c) Given that the concentrations of the reactants and products at a particular time are [CO2] = 0.65 M, [O2] = 0.020 M and [C6H12O6] = 0.055 M, determine the reaction quotient (Qc). Compare the Kc and Qc values and predict the favoured direction of the reaction.
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.
Humans are heterotrophs that consume food for energy. These foods comprise of sugars that are broken down by enzymic activity within the body for producing energy. This process, called
C6H12O6(aq) + 6O2(g) 6CO2(g) + 6H2O(l)
ΔH = –2802.7 kJ mol –1
a) Write an expression for the equilibrium constant for this reaction.
b) At equilibrium, the concentration of the reactants and products are determined as [CO2] = 0.30 M, [O2] = 0.040 M and [C6H12O6] = 0.065 M. Determine the value of the
equilibrium constant (Kc) and predict the whether the products or reactants will be
favoured at equilibrium.
c) Given that the concentrations of the reactants and products at a particular time are
[CO2] = 0.65 M, [O2] = 0.020 M and [C6H12O6] = 0.055 M, determine the reaction
quotient (Qc). Compare the Kc and Qc values and predict the favoured direction of the
reaction.
d) Explain the effect on equilibrium of
i) Increasing temperature
ii) Increasing pressure
iii) Decreasing the concentration of oxygen
iv) Increasing the concentration of carbon dioxide
v) Adding a catalyst
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I relation to the above question?
d) Explain the effect on equilibrium of
i) Increasing temperature
ii) Increasing pressure
iii) Decreasing the concentration of oxygen
iv) Increasing the concentration of carbon dioxide
v) Adding a catalyst
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