Section 1 Flashcards
What happens to the system when the concentration has increased/decreased?
Increase - system consumes some of the added components
Decrease - system produces some of the removed components
What are the three ways to change pressure?
1) changing the conc of the gaseous element
2) adding an inert gas
3) changing the volume of a vessel
T/F - change in temperature is the only way to change the constant
True
What is necessary for a process to be spontaneous?
Suniv > o
What is a chemical equilibrium?
When the concentrations of the reactants and products have reached constant values
Qc is greater than Kc?
Reverse direction
Qc is less than Kc
Forward direction
What equilibrium constant reflects the solubility of compound?
Ksp
When Change of Free Energy<0 is spontaneous, what direction is it favouring?
Forward direction to form more products
When Change of Free energy>0, reaction is spontaneous and goes which direction?
Reverse direction
What is the common ion effect
Adding an ion “common” to an equilibrium system, causes reaction mixture to change
Boyle’s law
V = constant/p
Ideal gas law
PV=nRT
Charles’ law
V=constant x T
Avogadros law
V= constant x n
What is potential energy
Energy due to the position of the object relative to other objects
Kinetic energy
Energy due to the motion of an object
What is an open system
Exchanges both matter and energy with surroundings
What is a closed system
Cannot exchange matter but can energy with surrounding
What is an isolated system
Cannot exchange matter or energy with the surrounding
Change of a Usys> 0
System ends up with more energy
Change of Usys < 0
System lose energy
Two ways the volume would expand in a system
- Increase the temp
- Decrease pressure
What is the standard enthalpy of formation of a compound
^Hf’ - enthalpy change for the reaction that produces one mole of the compound in it’s standard state
