Kinetic Molecular Theory - AP Physics 2
Card 1 of 12
What is the average molecular kinetic energy of a gas at a temperature of 
?
What is the average molecular kinetic energy of a gas at a temperature of
Tap to reveal answer
We know that the expression for average kinetic energy is:
Where average velocity of a gas is:
Plugging this into our expression for kinetic energy, we get:
Plugging in our values, we get:
We know that the expression for average kinetic energy is:
Where average velocity of a gas is:
Plugging this into our expression for kinetic energy, we get:
Plugging in our values, we get:
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A mixture of methane 
and oxygen 
is held at a constant temperature of 
and a pressure of 
. What is the ratio of the average velocity of methane to that of oxygen?
A mixture of methane
Tap to reveal answer
For gases at equal temperatures, we know that they both have the same average kinetic energy:
Note that 
is the molecular weight of each molecule, and 
is the average velocity of each molecule. Then rearranging for the ratio of velocities:
Then taking the square root of each side:
Now all we need is the molecular weight of each molecule:
Plugging these in, we get:
For gases at equal temperatures, we know that they both have the same average kinetic energy:
Note that
Then taking the square root of each side:
Now all we need is the molecular weight of each molecule:
Plugging these in, we get:
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What is the ratio of the rate of effusion of carbon dioxide 
to nitrogen 
?
What is the ratio of the rate of effusion of carbon dioxide
Tap to reveal answer
We can use Graham's law to solve this problem, which states that the ratio of effusion between to gasses is the square root of the inverse of the gases' molecular masses:
Therefore, in this problem we get:
Now we just need to determine the molecular masses of the two gasses, starting with carbon dioxide:
Plugging these in:
We can use Graham's law to solve this problem, which states that the ratio of effusion between to gasses is the square root of the inverse of the gases' molecular masses:
Therefore, in this problem we get:
Now we just need to determine the molecular masses of the two gasses, starting with carbon dioxide:
Plugging these in:
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What is the average molecular kinetic energy of a gas at a temperature of ?
What is the average molecular kinetic energy of a gas at a temperature of
Tap to reveal answer
We know that the expression for average kinetic energy is:
Where average velocity of a gas is:
Plugging this into our expression for kinetic energy, we get:
Plugging in our values, we get:
We know that the expression for average kinetic energy is:
Where average velocity of a gas is:
Plugging this into our expression for kinetic energy, we get:
Plugging in our values, we get:
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A mixture of methane and oxygen is held at a constant temperature of and a pressure of . What is the ratio of the average velocity of methane to that of oxygen?
A mixture of methane
Tap to reveal answer
For gases at equal temperatures, we know that they both have the same average kinetic energy:
Note that is the molecular weight of each molecule, and is the average velocity of each molecule. Then rearranging for the ratio of velocities:
Then taking the square root of each side:
Now all we need is the molecular weight of each molecule:
Plugging these in, we get:
For gases at equal temperatures, we know that they both have the same average kinetic energy:
Note that
Then taking the square root of each side:
Now all we need is the molecular weight of each molecule:
Plugging these in, we get:
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What is the ratio of the rate of effusion of carbon dioxide to nitrogen ?
What is the ratio of the rate of effusion of carbon dioxide
Tap to reveal answer
We can use Graham's law to solve this problem, which states that the ratio of effusion between to gasses is the square root of the inverse of the gases' molecular masses:
Therefore, in this problem we get:
Now we just need to determine the molecular masses of the two gasses, starting with carbon dioxide:
Plugging these in:
We can use Graham's law to solve this problem, which states that the ratio of effusion between to gasses is the square root of the inverse of the gases' molecular masses:
Therefore, in this problem we get:
Now we just need to determine the molecular masses of the two gasses, starting with carbon dioxide:
Plugging these in:
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What is the average molecular kinetic energy of a gas at a temperature of ?
What is the average molecular kinetic energy of a gas at a temperature of
Tap to reveal answer
We know that the expression for average kinetic energy is:
Where average velocity of a gas is:
Plugging this into our expression for kinetic energy, we get:
Plugging in our values, we get:
We know that the expression for average kinetic energy is:
Where average velocity of a gas is:
Plugging this into our expression for kinetic energy, we get:
Plugging in our values, we get:
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A mixture of methane and oxygen is held at a constant temperature of and a pressure of . What is the ratio of the average velocity of methane to that of oxygen?
A mixture of methane
Tap to reveal answer
For gases at equal temperatures, we know that they both have the same average kinetic energy:
Note that is the molecular weight of each molecule, and is the average velocity of each molecule. Then rearranging for the ratio of velocities:
Then taking the square root of each side:
Now all we need is the molecular weight of each molecule:
Plugging these in, we get:
For gases at equal temperatures, we know that they both have the same average kinetic energy:
Note that
Then taking the square root of each side:
Now all we need is the molecular weight of each molecule:
Plugging these in, we get:
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What is the ratio of the rate of effusion of carbon dioxide to nitrogen ?
What is the ratio of the rate of effusion of carbon dioxide
Tap to reveal answer
We can use Graham's law to solve this problem, which states that the ratio of effusion between to gasses is the square root of the inverse of the gases' molecular masses:
Therefore, in this problem we get:
Now we just need to determine the molecular masses of the two gasses, starting with carbon dioxide:
Plugging these in:
We can use Graham's law to solve this problem, which states that the ratio of effusion between to gasses is the square root of the inverse of the gases' molecular masses:
Therefore, in this problem we get:
Now we just need to determine the molecular masses of the two gasses, starting with carbon dioxide:
Plugging these in:
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What is the average molecular kinetic energy of a gas at a temperature of ?
What is the average molecular kinetic energy of a gas at a temperature of
Tap to reveal answer
We know that the expression for average kinetic energy is:
Where average velocity of a gas is:
Plugging this into our expression for kinetic energy, we get:
Plugging in our values, we get:
We know that the expression for average kinetic energy is:
Where average velocity of a gas is:
Plugging this into our expression for kinetic energy, we get:
Plugging in our values, we get:
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A mixture of methane and oxygen is held at a constant temperature of and a pressure of . What is the ratio of the average velocity of methane to that of oxygen?
A mixture of methane
Tap to reveal answer
For gases at equal temperatures, we know that they both have the same average kinetic energy:
Note that is the molecular weight of each molecule, and is the average velocity of each molecule. Then rearranging for the ratio of velocities:
Then taking the square root of each side:
Now all we need is the molecular weight of each molecule:
Plugging these in, we get:
For gases at equal temperatures, we know that they both have the same average kinetic energy:
Note that
Then taking the square root of each side:
Now all we need is the molecular weight of each molecule:
Plugging these in, we get:
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What is the ratio of the rate of effusion of carbon dioxide to nitrogen ?
What is the ratio of the rate of effusion of carbon dioxide
Tap to reveal answer
We can use Graham's law to solve this problem, which states that the ratio of effusion between to gasses is the square root of the inverse of the gases' molecular masses:
Therefore, in this problem we get:
Now we just need to determine the molecular masses of the two gasses, starting with carbon dioxide:
Plugging these in:
We can use Graham's law to solve this problem, which states that the ratio of effusion between to gasses is the square root of the inverse of the gases' molecular masses:
Therefore, in this problem we get:
Now we just need to determine the molecular masses of the two gasses, starting with carbon dioxide:
Plugging these in:
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