Ch.6 Equations
Ideal Gas Law
PV=nRT
1st Law of Thermodynamics
^E(universe) = ^E(system) + ^E(surroundings)=0
Boyle's Law: What two variables are related and how are they effect each other?
(Not at the molecular level)
Pressure and volume. If one increases the other decreases.
Under STP what is the pressure and temperature?
Pressure: 1atm
Temperature: 273K
In your calorimetry lab what was the system?
The metal
Mol Fraction
x= n(a)/n(total)
Change in internal energy of a system (^E)
^E = q + w
Charles' Law: What variables are related and how do they effect each other?
(Not at the molecular level)
Volume and temperature. If one increases the other will increase
What is Effusion?
the process by which a gas escapes through a small
hole in its container into an evacuated space
What is the unit of energy?
Joules (J)
Graham's Law of Effusion
1/(square root)M
Calorimetry(heat) equation
q=c*m*^T
Avogadro's Law: What variables are related and how do they effect each other?
(Not at the molecular level)
Volume and mols. As one increases the other will increase.
What are the units of R?
atm*L/mol*K
What is the meaning of Δ?
Overall change in state.
(final-initial)
1. Molar Mass
2. Density
1. M= mRT/PV
2. d= PM/RT
Constant volume calorimetry
q(cal)= C(cal) * ^T
According the Charles' Law at the molecular view, if you increase the temperature of the gas how does that effect the volume and pressure of the gas?
If you increase the temperature, the gas particles will move faster which will result in more collisions, increasing the pressure of the gas. The volume of the container will increase until the pressure of the atmosphere and the pressure of the gas are equal.
When do real gases deviate from ideal behavior?
At low temperatures and high pressure
If a chemical reaction occurs in a flask, in a lab in the SLC what is the system and what are the surroundings?
System: chemical reaction
Surroundings: Everything else
What are the two equations that involve partial pressure?
In what situations would you use each of the equations?
P(total)=P(a)+P(b)+P(c), P(a)=x(a) * P(total)
ex. If you were given multiple partial pressures and asked to find a total pressure. If you were asked to find the partial pressure of a gas given the number of mols of each gas in a mixture and the total pressure of the mixture.
Change in energy of reaction if it occurs at a constant volume
^E(rxn)= q(rxn)/mol or q(v)
According to Avogadro's Law at the molecular view, if you increase the number of moles in a container how does that effect the volume and pressure?
If you increase the number of moles, the gas particles will have less empty space which will result in more collisions, increasing the pressure of the gas. The volume of the container will increase until the pressure of the atmosphere and the pressure of the gas are equal.
Calculate the ratio of effusion rates of Cl2 to O2.
0.671
What are the units of specific heat?
J/g*C