Charasteristics of Gas
Volume, Pressure, Temperature
Units for volume
Litres - L (si unit) dm^3 - decimeter cubed (convenient and used used in IB)
Units for temperature
C - degrees celsius K - kelvin
Celsius to Kelvin formula
K = C + 273.15
What is the lowest temperature possible in K
0 K: absolute zero
Pressure
The force applied over an area (m^2)
Units for pressure
N/m^2 Pa - pascal
Converting pressure units
1.0 atm = 101325 Pa = 101.325 kPa = 1.01325 bar = 760 torr = 760 mmHg = 14.6959 psi
mmHg
Mercury
Standard Temperature and Pressure (STP)
"Standard" set of conditions exactly 273 kPa and 100. kPa
Standard Ambient Temperature and Pressure (SATP)
exactly 298 K and 100 kPa
Gas Laws
As pressure increases, volume decreases
As temperature increases, volume increases
As temperature decreases, pressure decreases
As temperature increases, pressure increases
As pressure increases, volume decreases
P ∝ 1/V PV = constant
As temperature increases, volume increases
T ∝ V T/V = constant
As temperature decreases, pressure decreases As temperature increases, pressure increases
P ∝ T P/T = constant
Boyle's Law
P1V1=P2V2 @ Constant T
Charlses' law
V1/T1 = V2/T2 @ Constant P
Gay Lussac's Law
P1/T1 = P2/T2 @ Constant V
Combined Gas Laws
P1V1/T1=P2V2/T2 @ constant mols
Units for gas laws
T - always use Kelvin P, V - units do not matter as long as the units are the same on both sides
Avogadro's Law
As you add additional gas to a system, the volume of that gas will increase
temperature and pressure are held constant
n ∝ V V1/n1 = V2/n2
Ideal Gases + model for the behaviour of gases
I) The volume of gas particles themselves are negligable compared to the volume of the gas II) There are no attractive forces between the gas particles
Ideal Gas Law formula
PV = nRT
R
Ideal gas constant (in units J/k * mol) Volume in Ideal Gas Law formula must be in m^3, pressure in Pa, and temperature in K
Thermodynamics
The study of how heat works energy + temperature relate to each other
1st Law of Thermodynamics - Conservation of Energy
energy cannot be created or destroyed
you can only transfer energy
Heat
A form of energy Thermal energy
Kinetic Energy
the energy of motion Kinetic Energy - 1/2m(^2)
m
mass
V
velocity
Temperature (energetics)
a measure of the average kinetic energy
energy is added to substance -> internal energy goes up -> particles have more kinetic energy -> particles move faster -> higher temperature
Boltzmann Distribution
Potential Energy
energy that is stored in a system
Enthalpy (H)
total internal energy of a system
stored in the bonds
ΔH (delta H)
change in Enthalpy
ΔH = Hproducts - Hreactants
Endothermic
total internal energy goes up (increases)
absorbs heat
ΔH is positive
Exothermic
total internal energy does down (decreases)
releases heat
ΔH is negative
Endothermic reaction
Exothermic reaction
Measuring Enthalpy - Heat Capacity calorimetry
the science or act of measuring changes in state variables of a body for the purpose of deriving the heat transfer associated with changes of its state due, for example, to chemical reactions, physical changes, or phase transitions under specified constraints (google)
Calorimetry equation
q = CpmΔT
q
Heat energy (J - energy measured in joules)
Cp
Heat capacity (J/g*K)
ΔT
Change in temperature (K, C)
ΔH
change in enthalpy
Average Bond Enthalpy
The energy needed to break 1 mole of a bond of a gaseous molecule averaged over similar compounds
Stability in reactions
The products are more stable than the reactants, as they have a lower energy level, making it easier to maintain
Hess’s Law
The enthalpy change for a reaction that is carried out in a series of steps is equal to the sum of the enthalpy changes for the individual steps