Book: Key Terms: Ch. 20 Flashcards
adenosine triphosphate (ATP)
.
coupling of reactions
When two reactions are coupled, one step supplies enough free energy for the other to occur.
entropy (S)
S = k ln(W), where k is the Boltzmann constant, and W is the number of microstates. Entropy describes the amount of disorder in a system.
free energy (G)
G = H - T S, where H is enthalpy, S is entropy, and T is temperature in kelvin. The equation for the free energy of a reaction can be rewritten as ∆G = ∆H - T ∆S, and the change in the free energy is a measure of the spontaneity of a reaction. If ∆G < 0, it is spontaneous; if ∆G > 0, it isn’t. If ∆G = 0, the process is at equilibrium.
microstate
Each quantized state of a system is called a microstate, and at any instant, the total energy of the system is dispersed throughout one microstate.
second law of thermodynamics
All real processes occur spontaneously in the direction that increases the entropy of the universe (system + surroundings).
spontaneous change
Spontaneous change of a system is one that occurs under specified conditions without a continuous input of energy from outside the system.
standard entropy of reaction (∆Sº_rxn)
The entropy change that occurs when all the reactants and products are in their standard states. If there is an increase in moles of gas, ∆Sº_rxn > 0, and if there’s a decrease, ∆Sº_rxn < 0. The general equation for ∆Sº_rxn is given as:
∆Sº_rxn = m Σ Sº_products - n Σ Sº_reactants
standard free energy change (∆Gº)
The standard free energy change of a reaction occurs when all of the components of the system are in their standard states: ∆Gº_sys = ∆Hº_sys - T ∆Sº_sys
standard free energy of formation (∆Gº_f)
All substances have values for this. It is the energy change that occurs when 1 mol of a compound is made from its elements, with all components in their standard states. The general equation is:
∆Hº_rxn = m Σ Hº_(f)products - n Σ Hº_(f)reactants
standard molar entropy (Sº)
A way of specifying the entropy of substances that takes into account the fact that entropy is an extensive property; Sº has units of J / mol K and it is typically given for a substance at 298 K with other std conditions.
third law of thermodynamics
A perfect crystal has zero entropy at absolute zero: S_sys = 0 at 0 K.