General Chemistry Flashcards
(28 cards)
Boyle’s Law
P1V1 = P2V2
Charle’s Law
V1/T1 = V2/T2
Gay-Lussac’s Law
P1/T1=P2/T2
Hund’s Rule
e- only double up in orbitals if all orbitals first have 1 e-.
Aufbau Principle
Direction of increasing n+1 value.
Q < Keq
∆G < 0, reaction proceeds towards products –>
Q = Keq
∆G = 0, equilibrium
Q > Keq
∆G > 0, reaction proceeds toward the reactants <–
↓pH
↑respiration to blow off CO2
↓pH
↑respiration to blow off CO2
↑pH
↓respiration, trapping CO2
+∆H and +∆S
Spontaneous at HIGH temperatures.
+∆H and -∆S
Non-spontaneous at ALL temperatures.
-∆H and +∆S
Spontaneous at ALL temperatures.
-∆H and -∆S
Spontaneous at LOW temperatures.
Keq > 1
Favors product formation. ∆G < 0
Keq = 1
Reaction is at equilibrium. ∆G = 0
Keq < 1
Favors reactant formation. ∆G > 0
1 atm to mmHg
1 atm = 760 mmHg
1 atm to torr
1 atm = 760 torr
1 atm to kPa
1 atm = 101.3 kPa
1 atm to psi
1 atm = 14.7 psi
How does the volume of a real gas compare to that of an ideal gas at moderately ↑P, ↓V or ↓T?
Real gases will occupy less volume than predicted by the ideal gas law because the particles have intermolecular attractions.
How does the volume of a real gas compare to that of an ideal gas at extremely ↑P, ↓V or ↓T?
Real gases will occupy more volume than predicted by the ideal gas law because the particles occupy physical space.
