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If all of the following flasks are the same size, at the same temperature, and contain the same number of molecules, in which flask will the pressure be highest?
-All have the same pressure
-Flask 4
-Flask 2
-Flask 3
-Flask 1
All have the same pressure, because pressure is a function of the number of molecules, temperature, and volume, but does not depend on the identity of the gas.
100
At 17 °C, a 0.80 mole sample of a gas exerts a pressure of 1.2 atmospheres. What is the volume of the container?
15.87L
100
How do gas molecules move?
Randomly because of collisions
100
What is Pressure
The amount of force exerted from the collision on the sides of a container.
Flask 1 because as the volume decreases the pressure increases because there are more collisions per unit of surface area within the container.
200
How many moles of oxygen must be placed in a 3.00 liter container in order to exert a pressure of 2.00 atmospheres at 25 °C?
0.245 moles
200
What is Diffusion?
Molecules going from areas of high concentration to low concentration.
200
What does PTV stand for?
Pressure, Temperature, Volume
200
What is this gas law also known as: P1V1/T1=P2V2/T2
Combined Gas Law
300
Which of the following gases move the fastest when at the same temperature, and contain the same number of molecules, and have the same volume?
He, Ne, Ar, Kr
He
300
What is the pressure exerted by 5.00 moles of nitrogen gas contained in a 30.0 Liter container at 25.0 °C?
4.07 atm
300
Do larger or smaller molecules diffuse faster?
Smaller molecules
300
If Pressure is held constant and Temperature increases, what happens to the volume?
What is the Ideal Gas Law, and what units have to be used?
PV=nRT
atm,Liters,moles,Ideal Gas Constant, and Kelvin
400
Do molecules move faster or slower in high pressure?
They move slower in high pressure.
400
If temperature is held constant and volume increases, what happens to the pressure?
It decreases.
400
Which Gas Law is this: P1/T1=P2/T2
Gay-Lussac's Law
500
Which of the following gases would have the slowest rate of diffusion, assuming all of the gases are at the same temperature?
H,Cl,F,Se
Se
500
A 500 mL metal cylinder holding 0.100 moles of helium gas is known to rupture at a pressure of 10 atmospheres. At what temperature, in °C, will the container fail?
336 C
500
What is diffusion
I is blank
500
What are different ways to effect the number of collisions (effect the pressure)? Name 2.
1) Increase the temperature, makes the molecules move faster and collide more
2) Decreasing the volume gives less space for the molecules to move, so more collisions occur.
3) Adding more particles will increase the chance of collisions.
4)Increasing pressure will make the particles bounce off more and collide more.
500
If a gas has a pressure of 432.5 Kpa, in a 8120 mL container, and at a temperature of 74C, how many moles of gas are in the container?