What is the basic concept of gas pressure?

Dalton's Law of Partial Pressure and Gas Mixtures Explained

Interactive Video
•
Physics, Chemistry, Science
•
9th - 12th Grade
•
Hard

Patricia Brown
FREE Resource
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10 questions
Show all answers
1.
MULTIPLE CHOICE QUESTION
30 sec • 1 pt
Gas molecules exert force only when heated.
Gas molecules exert force on each other.
Gas molecules do not exert any force.
Gas molecules exert force on the walls of the container.
2.
MULTIPLE CHOICE QUESTION
30 sec • 1 pt
According to Dalton's Law, what is the total pressure in a container with a mixture of gases?
The average pressure of all gases.
The pressure of the gas with the highest temperature.
The pressure of the gas with the highest volume.
The sum of the partial pressures of each individual gas.
3.
MULTIPLE CHOICE QUESTION
30 sec • 1 pt
What is the formula for the partial pressure of a gas according to Dalton's Law?
Partial pressure = Mole fraction of the gas x Total pressure
Partial pressure = Mole fraction of the gas / Total pressure
Partial pressure = Total pressure - Mole fraction of the gas
Partial pressure = Total pressure / Number of gases
4.
MULTIPLE CHOICE QUESTION
30 sec • 1 pt
In the derivation of Dalton's Law, what cancels out when dividing equation two by equation one?
The volume and the gas constant
The pressure
The temperature
The number of moles
5.
MULTIPLE CHOICE QUESTION
30 sec • 1 pt
How do you calculate the mole fraction of a gas in a mixture?
Number of moles of the gas divided by total number of moles
Total number of moles minus number of moles of the gas
Total number of moles divided by number of moles of the gas
Number of moles of the gas multiplied by total number of moles
6.
MULTIPLE CHOICE QUESTION
30 sec • 1 pt
What is the total pressure of a gas mixture containing 4 grams of hydrogen and 32 grams of oxygen at 298 Kelvin?
12.22 atmosphere
6.11 atmosphere
18.349 atmosphere
5 atmosphere
7.
MULTIPLE CHOICE QUESTION
30 sec • 1 pt
How is the partial pressure of hydrogen gas calculated in the given numerical problem?
By subtracting the mole fraction of hydrogen from the total pressure
By dividing the total pressure by the number of moles of hydrogen
By multiplying the mole fraction of hydrogen by the total pressure
By adding the mole fraction of hydrogen to the total pressure
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