Edited Invalid date
6.8 Kinetic Molecular Theory: -- Part 1
The ratio of rates is what you know about the mass of nitrogen.
The units of the answer are correct.
The answer seems reasonable for the mass of the gas.
You can conclude from the answer that the gas is probably xenon, which has a molar mass of 131.29 g>mol.
A glass tube has an equal number of moles.
The tube has the same number of moles as before.
The tube has more moles of helium than argon.
The tube has more moles of argon than helium.
A mole of ideal gas has a volume of 22.41 L. Most of these gases have a volume that is close to 22.41 L, meaning that they act like ideal gases.
The molar volumes of several gases are close to 22.41 L, which indicates that their departures from ideal behavior are small.
These assumptions are valid for most gases.
At higher pressures or lower temperatures, these assumptions break down.
The volume of the particles themselves occupies a significant portion of the total gas volume.
The volume of argon is almost the same as that of an ideal gas.
The ideal gas law predicts as a gas.
At high pressure, the particle size becomes significant.
0.0562 is the number of atoms or molecule that compose a substance.
The molecule have a lot of energy.
They don't affect the collision much.
An analogy to billiard balls can be used to understand this difference.
Imagine two balls coated in a substance that makes them sticky.
The balls bounce off one another as if the sticky substance was not there, if they collide at high speeds.
The sticky substance would have an effect if the two balls collide.
The balls might not bounce off one another.
The effect of these weak attractions between particles is a decrease in the number of collisions with the surfaces of the container and a decrease in the pressure compared to that of an ideal gas.
The pressure of the xenon gas is almost the same as that of an ideal gas.
The xenon atoms spend more time interacting with each other and less time colliding with the walls, making the pressure less than predicted by the ideal gas law.
At low temperature, intermolecular forces become significant.
Real gases are different from ideal gas behavior.
The behavior of helium is a positive deviation from the ideal behavior.
The volume is 1mol ing.
The effects of the ideal gas law are combined.
The temperature at which these curves were calculated was 500 K.
The curves should be ranked in order of temperature.
The initial volume of the gas sample is 0.500 L.
A gas sample has a volume of 178 mL.
A sample of gas contains oxygen and nitrogen.
chlorine gas reacts with aluminum to form a metal.
A gas sample occupies 663 mL at 25 degC and 1.00 atm.
A sample of Xe takes 75 seconds to leave a container.
37 seconds is the time it takes for an unknown gas to effuse out of a container.
Gas pressure is the force per unit area that results from gas particles The total of the measure pressure, including Hg, torr, Pa, and psi, is the property of the mixture.
When other variables are constant, the simple gas laws express relationships between pairs of vari ables.
The volume of a gas is related to the pressure in the reaction.
The quantities can be converted to moles based on the temperature.
Avogadro's law states that the volume of a gas is directly proportional to the amount in moles.
The ideal gas law can be used to find one of the four variables giv molar volume at STP.
The amount in moles and the amount in liters can be calculated using it.
The mean free path of a gas particle is determined by the relative rates of diffusion or effusion.
There is a model for gases.
View flashcards and assignments made for the note
Getting your flashcards
Privacy & Terms