Kinetic Molecular Theory - AP Chemistry
Card 1 of 78
Which of the following is not an assumption of the kinetic molecular theory of gases?
Which of the following is not an assumption of the kinetic molecular theory of gases?
Tap to reveal answer
The kinetic molecular theory of gases states that the average kinetic energy of gas particles is proportional to temperature, and it is the same for all gases at a given temperature. This is the opposite of what is stated in the answer choice.
The kinetic molecular theory of gases states that the average kinetic energy of gas particles is proportional to temperature, and it is the same for all gases at a given temperature. This is the opposite of what is stated in the answer choice.
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Two moles of nitrogen gas are kept in a glass container. The temperature of the gas is 400K.
What is the kinetic energy of the gas?
Two moles of nitrogen gas are kept in a glass container. The temperature of the gas is 400K.
What is the kinetic energy of the gas?
Tap to reveal answer
Using the equation 
, n being the number of moles, R being 8.314, and T being the temperature in Kelvin, we can find the kinetic energy of two moles of gas in a container.
Using the equation
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Why does a higher temperature result in a faster reaction?
Why does a higher temperature result in a faster reaction?
Tap to reveal answer
The temperature of a system can be manipulated to increase the reaction rate. The temperature affects the rate of the reaction because as temperature increases, so does the average kinetic energy. This means that molecules (reactants) are moving around more quickly, resulting in more frequent molecular collisions, resulting in an increased rate of product formation.
The temperature of a system can be manipulated to increase the reaction rate. The temperature affects the rate of the reaction because as temperature increases, so does the average kinetic energy. This means that molecules (reactants) are moving around more quickly, resulting in more frequent molecular collisions, resulting in an increased rate of product formation.
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Which of the following statements in not an assumption made in kinetic molecular theory?
Which of the following statements in not an assumption made in kinetic molecular theory?
Tap to reveal answer
The average kinetic energy is considered to be a sole function of temperature; pressure is not a factor. All of the other statements are assumptions of kinetic molecular theory.
The average kinetic energy is considered to be a sole function of temperature; pressure is not a factor. All of the other statements are assumptions of kinetic molecular theory.
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The reaction 
obeys the rate law 
What are the units of the rate constant, 
?
The reaction
What are the units of the rate constant,
Tap to reveal answer
Recall that 
and that 
and 
are both molar concentrations. Then,
Dividing both sides by 
gives
Recall that
Dividing both sides by
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Consider the following first order reaction
Where k is the rate constant.
and the initial concentrations of A and B are
What is the percent conversion after 500 seconds? Round to the nearest percent.
Consider the following first order reaction
Where k is the rate constant.
and the initial concentrations of A and B are
What is the percent conversion after 500 seconds? Round to the nearest percent.
Tap to reveal answer
For a first order reaction,
Integrating both sides gives
Where 
is an integration constant.
Solving for 
gives
Initially 
there are 3 mols of 
. Using this we find that
At 
,
Percent conversion is calculated as follows:
For a first order reaction,
Integrating both sides gives
Where
Solving for
Initially
At
Percent conversion is calculated as follows:
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Which of the following is not an assumption of the kinetic molecular theory of gases?
Which of the following is not an assumption of the kinetic molecular theory of gases?
Tap to reveal answer
The kinetic molecular theory of gases states that the average kinetic energy of gas particles is proportional to temperature, and it is the same for all gases at a given temperature. This is the opposite of what is stated in the answer choice.
The kinetic molecular theory of gases states that the average kinetic energy of gas particles is proportional to temperature, and it is the same for all gases at a given temperature. This is the opposite of what is stated in the answer choice.
← Didn't Know|Knew It →
Two moles of nitrogen gas are kept in a glass container. The temperature of the gas is 400K.
What is the kinetic energy of the gas?
Two moles of nitrogen gas are kept in a glass container. The temperature of the gas is 400K.
What is the kinetic energy of the gas?
Tap to reveal answer
Using the equation , n being the number of moles, R being 8.314, and T being the temperature in Kelvin, we can find the kinetic energy of two moles of gas in a container.
Using the equation
← Didn't Know|Knew It →
Why does a higher temperature result in a faster reaction?
Why does a higher temperature result in a faster reaction?
Tap to reveal answer
The temperature of a system can be manipulated to increase the reaction rate. The temperature affects the rate of the reaction because as temperature increases, so does the average kinetic energy. This means that molecules (reactants) are moving around more quickly, resulting in more frequent molecular collisions, resulting in an increased rate of product formation.
The temperature of a system can be manipulated to increase the reaction rate. The temperature affects the rate of the reaction because as temperature increases, so does the average kinetic energy. This means that molecules (reactants) are moving around more quickly, resulting in more frequent molecular collisions, resulting in an increased rate of product formation.
← Didn't Know|Knew It →
Which of the following statements in not an assumption made in kinetic molecular theory?
Which of the following statements in not an assumption made in kinetic molecular theory?
Tap to reveal answer
The average kinetic energy is considered to be a sole function of temperature; pressure is not a factor. All of the other statements are assumptions of kinetic molecular theory.
The average kinetic energy is considered to be a sole function of temperature; pressure is not a factor. All of the other statements are assumptions of kinetic molecular theory.
← Didn't Know|Knew It →
The reaction obeys the rate law
What are the units of the rate constant, ?
The reaction
What are the units of the rate constant,
Tap to reveal answer
Recall that and that and are both molar concentrations. Then,
Dividing both sides by gives
Recall that
Dividing both sides by
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Consider the following first order reaction
Where k is the rate constant.
and the initial concentrations of A and B are
What is the percent conversion after 500 seconds? Round to the nearest percent.
Consider the following first order reaction
Where k is the rate constant.
and the initial concentrations of A and B are
What is the percent conversion after 500 seconds? Round to the nearest percent.
Tap to reveal answer
For a first order reaction,
Integrating both sides gives
Where is an integration constant.
Solving for gives
Initially there are 3 mols of . Using this we find that
At ,
Percent conversion is calculated as follows:
For a first order reaction,
Integrating both sides gives
Where
Solving for
Initially
At
Percent conversion is calculated as follows:
← Didn't Know|Knew It →
Which of the following is not an assumption of the kinetic molecular theory of gases?
Which of the following is not an assumption of the kinetic molecular theory of gases?
Tap to reveal answer
The kinetic molecular theory of gases states that the average kinetic energy of gas particles is proportional to temperature, and it is the same for all gases at a given temperature. This is the opposite of what is stated in the answer choice.
The kinetic molecular theory of gases states that the average kinetic energy of gas particles is proportional to temperature, and it is the same for all gases at a given temperature. This is the opposite of what is stated in the answer choice.
← Didn't Know|Knew It →
Two moles of nitrogen gas are kept in a glass container. The temperature of the gas is 400K.
What is the kinetic energy of the gas?
Two moles of nitrogen gas are kept in a glass container. The temperature of the gas is 400K.
What is the kinetic energy of the gas?
Tap to reveal answer
Using the equation , n being the number of moles, R being 8.314, and T being the temperature in Kelvin, we can find the kinetic energy of two moles of gas in a container.
Using the equation
← Didn't Know|Knew It →
Why does a higher temperature result in a faster reaction?
Why does a higher temperature result in a faster reaction?
Tap to reveal answer
The temperature of a system can be manipulated to increase the reaction rate. The temperature affects the rate of the reaction because as temperature increases, so does the average kinetic energy. This means that molecules (reactants) are moving around more quickly, resulting in more frequent molecular collisions, resulting in an increased rate of product formation.
The temperature of a system can be manipulated to increase the reaction rate. The temperature affects the rate of the reaction because as temperature increases, so does the average kinetic energy. This means that molecules (reactants) are moving around more quickly, resulting in more frequent molecular collisions, resulting in an increased rate of product formation.
← Didn't Know|Knew It →
Which of the following statements in not an assumption made in kinetic molecular theory?
Which of the following statements in not an assumption made in kinetic molecular theory?
Tap to reveal answer
The average kinetic energy is considered to be a sole function of temperature; pressure is not a factor. All of the other statements are assumptions of kinetic molecular theory.
The average kinetic energy is considered to be a sole function of temperature; pressure is not a factor. All of the other statements are assumptions of kinetic molecular theory.
← Didn't Know|Knew It →
The reaction obeys the rate law
What are the units of the rate constant, ?
The reaction
What are the units of the rate constant,
Tap to reveal answer
Recall that and that and are both molar concentrations. Then,
Dividing both sides by gives
Recall that
Dividing both sides by
← Didn't Know|Knew It →
Consider the following first order reaction
Where k is the rate constant.
and the initial concentrations of A and B are
What is the percent conversion after 500 seconds? Round to the nearest percent.
Consider the following first order reaction
Where k is the rate constant.
and the initial concentrations of A and B are
What is the percent conversion after 500 seconds? Round to the nearest percent.
Tap to reveal answer
For a first order reaction,
Integrating both sides gives
Where is an integration constant.
Solving for gives
Initially there are 3 mols of . Using this we find that
At ,
Percent conversion is calculated as follows:
For a first order reaction,
Integrating both sides gives
Where
Solving for
Initially
At
Percent conversion is calculated as follows:
← Didn't Know|Knew It →
Which of the following is not an assumption of the kinetic molecular theory of gases?
Which of the following is not an assumption of the kinetic molecular theory of gases?
Tap to reveal answer
The kinetic molecular theory of gases states that the average kinetic energy of gas particles is proportional to temperature, and it is the same for all gases at a given temperature. This is the opposite of what is stated in the answer choice.
The kinetic molecular theory of gases states that the average kinetic energy of gas particles is proportional to temperature, and it is the same for all gases at a given temperature. This is the opposite of what is stated in the answer choice.
← Didn't Know|Knew It →
Two moles of nitrogen gas are kept in a glass container. The temperature of the gas is 400K.
What is the kinetic energy of the gas?
Two moles of nitrogen gas are kept in a glass container. The temperature of the gas is 400K.
What is the kinetic energy of the gas?
Tap to reveal answer
Using the equation , n being the number of moles, R being 8.314, and T being the temperature in Kelvin, we can find the kinetic energy of two moles of gas in a container.
Using the equation
← Didn't Know|Knew It →