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Kinetic Molecular Theory (KMT)
Ideal Gas Law
Combined Gas Law
Root Mean Square Velocity
Ideal Gas Law + Density = Molar Mass
100
The measure of kinetic energy.
What is temperature?
100
The Ideal Gas Law and the gas constant for the equation.
What is PV=nRT and 0.08206 L atm/K mol?
100
The Combined Gas Law.
What is P1V1/T1=P2V2/T2?
100
The equation for Root Mean Square Velocity.
What is µrms=√((3 RT)/M)?
100
The equation for calculating molar mass when given the ideal gas law and density.
What is Molar mass=dRT/P?
200
Can be assumed negligible (zero).
What is the volume of the individual particles of a gas?
200
the volume of 0.341 moles of CO2 at 22 degrees C and 1.04 atm. V(volume)=[(0.341 mol)(0.08206 L atm/K mol)(295 K)]/1.04 atm
What is 7.94 L?
200
the end volume of a gas at 1 atm, 1 L, and 1 K that was changed to 2 atm and 6 K.
What is 3 L?
200
R constant for RMSV
What is 8.3145?
200
the molar mass of a gas at 34 degreec C and 1.75 atm with a density of 3.4g/L. Molar mass= [(3.40 g/L)(0.08206 L atm/K mol)(307 K)]/1.75 atm
What is 48.94527314 g/mol (molar mass)?
300
The collisions of the particles with the walls of the container (b/c the particles are in constant motion).
What is the cause of the pressure exerted by a gas?
300
the temperature of 12 g of H2 at 4 atm and with a volume of 3 L.
What is 24.37241043 degrees Kelvin?
300
the end volume of a gas at 2.35 atm, 6.42 L, and 336 K that was cooled to 326 K.
What is 6.228928571 L?
300
the molar mass of a gas at 100 K and 6.7834 atm with a density of 4.791 kg/L.
What is 5795.758174 g/mol? hehe, Did you forget to convert the 4.791 kg/L into 4791 g/L?
400
Are assumed to exert no forces on each other.
What are the particles?
400
62 g of SO2 at 562 K ad with a volume of 26.21 L.
What is 1.818122616 atm?
400
the end temperature of a gas that started at 60 atm, 60 L, and 24 K and was changed to 30 atm and 50 L.
What is 10 K?
500
The postulates (all 4) of the Kinetic Molecular Theory.
What are these statements?:

1. The volume of the particles of a gas can be assumed negligible (zero).

2. The particles are in constant motion. The collisions of the particles with the walls of the container are the cause of the pressure exerted by the gas.

3. The particles are assumed to exert no forces on each other.

4. The average kinetic energy of gas particles is assumed to be directly proportional to the Kelvin temperature of the gas.

500
the mass of NO2 (mm=46.005) at 10.62 atm, 12.62 L, and 265 K.
What is 283.538162249895 g?
500
the end pressure of a gas that started at 10 atm, 10 L, and 156 K and was changed to 11 L and 223.08 K.
What is 13 atm?