Bioenergetics
First Law of Thermodynamics; energy can be transferred from one form to another, it cannot be
created or destroyed.
Second Law of Thermodynamics; for a spontaneous reaction, the entropy of the universe
increases.
Third Law of Thermodynamics; A perfect crystal at 0K has an entropy of 0.
The quantity of heat transferred depends on the size of the temperature difference, quantity of
material, identity of the material. Specific heat capacity is the amount of heat energy required to
increase the temperature of 1g of a substance by 1K.
q (heat transferred (J)) = c (specific heat capacity (J/g/K)) x m (mass of substance (g)) x t
(change in temperature(K))
E Change in internal energy (J) = Q Heat transferred to or from system (J) + W Work
transferred to or from system (J)
Energy is the capacity to do work. Work is done when a force is acting and displacing an object.
w = work done at constant pressure x change in volume (W=−PΔV)
The energy of a closed system can be transferred as work or heat. Heat is the transfer of energy
that gives rise to chaotic motion in the surroundings. Work is the transfer of energy that gives rise
to a uniform motion in the surroundings.
The enthalpy change when 1 mole of a
Enthalpy Change of compound is formed from elements in
Formation standard states. Enthalpy Change = products -
reactants
The enthalpy change when 1 mole of a
compound undergoes complete combustion in
Enthalpy Change of
excess oxygen with all reactants and products
Combustion
in standard states. Enthalpy Change =
reactants - products
Enthalpy Heat content of a system at constant pressure.
Enthalpy Change Heat energy change of a system at a constant
pressure. Enthalpy Change of Reaction = total
Bioenergetics 1
First Law of Thermodynamics; energy can be transferred from one form to another, it cannot be
created or destroyed.
Second Law of Thermodynamics; for a spontaneous reaction, the entropy of the universe
increases.
Third Law of Thermodynamics; A perfect crystal at 0K has an entropy of 0.
The quantity of heat transferred depends on the size of the temperature difference, quantity of
material, identity of the material. Specific heat capacity is the amount of heat energy required to
increase the temperature of 1g of a substance by 1K.
q (heat transferred (J)) = c (specific heat capacity (J/g/K)) x m (mass of substance (g)) x t
(change in temperature(K))
E Change in internal energy (J) = Q Heat transferred to or from system (J) + W Work
transferred to or from system (J)
Energy is the capacity to do work. Work is done when a force is acting and displacing an object.
w = work done at constant pressure x change in volume (W=−PΔV)
The energy of a closed system can be transferred as work or heat. Heat is the transfer of energy
that gives rise to chaotic motion in the surroundings. Work is the transfer of energy that gives rise
to a uniform motion in the surroundings.
The enthalpy change when 1 mole of a
Enthalpy Change of compound is formed from elements in
Formation standard states. Enthalpy Change = products -
reactants
The enthalpy change when 1 mole of a
compound undergoes complete combustion in
Enthalpy Change of
excess oxygen with all reactants and products
Combustion
in standard states. Enthalpy Change =
reactants - products
Enthalpy Heat content of a system at constant pressure.
Enthalpy Change Heat energy change of a system at a constant
pressure. Enthalpy Change of Reaction = total
Bioenergetics 1
