Thermodynamics Flashcards
In thermodynamics what does q stand for?
q= heat, absorbed by the system from the surroundings
In thermodynamics what does w stand for?
w= work done by the system on the surroundings.
What do we assume about pressure in this class?
Biological processes occur under constant pressure.
What does DeltaH= qp mean?
qp is the heat absorbed by the system at constant pressure. Which in biological systems is always the case.
What are the units of entropy?
J*K-1
What is the entropy equation?
S=Kb*Ln(W)
Kb= Boltzmann constant
W= the number of energetically equivalent ways of a range of components in the system.
Assuming constant P and T, what can we assume about a negative Delta G?
It’s a spontaneous process. (Exergonic)
When does Delta G = 0?
When reaction is at equilibrium.
What are the two Gibbs free energy equations without constants?
Delta G = G(final)-G(initial) = Delta H - T*Delta S
Write out the equation of chemical equilibria for free energy of compound A at concentration [A].
What does this represent?
The “partial molar free energy” of compound A, also called the “chemical potential” of compound A – at a well defined “standard state”.
What equation shows the dependence of Delta G on the concentrations of the reactants. Write it out then check.
What part of this equation is concentration dependent? What about independent?
Keq = ?
Does Delta G determine the rate of a reaction?
NO! The rate of a process depends on the detailed mechanism of the process and is independent of the absolute value of Delta G.
