Kinetic Molecular Theory - MCAT Chemical and Physical Foundations of Biological Systems
Card 1 of 21
Phase diagrams are used to depict changes in the properties of a solution at different temperatures and pressures. Below is a phase diagram of a polar solution.
In section 3, as the temperature increases, the velocity of the molecules in a(n) manner.
Phase diagrams are used to depict changes in the properties of a solution at different temperatures and pressures. Below is a phase diagram of a polar solution.
In section 3, as the temperature increases, the velocity of the molecules in a(n) manner.
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This question asks you how the velocity of the molecules changes with increasing temperature. From molecular kinteics, we know that temperature is proportional to kinetic energy.
We can see that as temperature rises, the kinetic energy rises, however, the question asks us how the velocity changes. Now, we need to know how kinetic energy and velocity are related. We can pull this relationship from Newtonian mechanics.
If we simplify, we can see that 
. Velocity increases with increasing temperature, but in an indirectly proportional manner.
This question asks you how the velocity of the molecules changes with increasing temperature. From molecular kinteics, we know that temperature is proportional to kinetic energy.
We can see that as temperature rises, the kinetic energy rises, however, the question asks us how the velocity changes. Now, we need to know how kinetic energy and velocity are related. We can pull this relationship from Newtonian mechanics.
If we simplify, we can see that
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At room temperature which of the following equimolar gases has the fastest effusion rate?
At room temperature which of the following equimolar gases has the fastest effusion rate?
Tap to reveal answer
According to Graham's law, the rate of effusion of a gas is inversely proportional to the square root of the mass: 
.
The gas with the lowest molecular weight will effuse the fastest. 
has the lowest molecular weight of the given gasses, with a value of 
.
According to Graham's law, the rate of effusion of a gas is inversely proportional to the square root of the mass:
The gas with the lowest molecular weight will effuse the fastest.
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Consider a helium atom and a molecule of carbon monoxide both at a temperature of 
. Which of the following accurately describes the velocity of the carbon monoxide molecule in relation to the velocity of the helium atom?
Consider a helium atom and a molecule of carbon monoxide both at a temperature of
Tap to reveal answer
Since both molecules are at the same temperature, the value of the temperature is irrelevant. The difference in velocity between the two molecules depends on the difference in their molar masses. The molar mass of a helium atom is 
, and the molar mass of a carbon monoxide molecule is 
.
Graham's Law describes the relationship between gas particle mass and velocity:
Using the molar masses of the particles in question, we can determine their relationship.
Since both molecules are at the same temperature, the value of the temperature is irrelevant. The difference in velocity between the two molecules depends on the difference in their molar masses. The molar mass of a helium atom is
Graham's Law describes the relationship between gas particle mass and velocity:
Using the molar masses of the particles in question, we can determine their relationship.
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Phase diagrams are used to depict changes in the properties of a solution at different temperatures and pressures. Below is a phase diagram of a polar solution.
In section 3, as the temperature increases, the velocity of the molecules in a(n) manner.
Phase diagrams are used to depict changes in the properties of a solution at different temperatures and pressures. Below is a phase diagram of a polar solution.
In section 3, as the temperature increases, the velocity of the molecules in a(n) manner.
Tap to reveal answer
This question asks you how the velocity of the molecules changes with increasing temperature. From molecular kinteics, we know that temperature is proportional to kinetic energy.
We can see that as temperature rises, the kinetic energy rises, however, the question asks us how the velocity changes. Now, we need to know how kinetic energy and velocity are related. We can pull this relationship from Newtonian mechanics.
If we simplify, we can see that . Velocity increases with increasing temperature, but in an indirectly proportional manner.
This question asks you how the velocity of the molecules changes with increasing temperature. From molecular kinteics, we know that temperature is proportional to kinetic energy.
We can see that as temperature rises, the kinetic energy rises, however, the question asks us how the velocity changes. Now, we need to know how kinetic energy and velocity are related. We can pull this relationship from Newtonian mechanics.
If we simplify, we can see that
← Didn't Know|Knew It →
At room temperature which of the following equimolar gases has the fastest effusion rate?
At room temperature which of the following equimolar gases has the fastest effusion rate?
Tap to reveal answer
According to Graham's law, the rate of effusion of a gas is inversely proportional to the square root of the mass: .
The gas with the lowest molecular weight will effuse the fastest. has the lowest molecular weight of the given gasses, with a value of .
According to Graham's law, the rate of effusion of a gas is inversely proportional to the square root of the mass:
The gas with the lowest molecular weight will effuse the fastest.
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Consider a helium atom and a molecule of carbon monoxide both at a temperature of . Which of the following accurately describes the velocity of the carbon monoxide molecule in relation to the velocity of the helium atom?
Consider a helium atom and a molecule of carbon monoxide both at a temperature of
Tap to reveal answer
Since both molecules are at the same temperature, the value of the temperature is irrelevant. The difference in velocity between the two molecules depends on the difference in their molar masses. The molar mass of a helium atom is , and the molar mass of a carbon monoxide molecule is .
Graham's Law describes the relationship between gas particle mass and velocity:
Using the molar masses of the particles in question, we can determine their relationship.
Since both molecules are at the same temperature, the value of the temperature is irrelevant. The difference in velocity between the two molecules depends on the difference in their molar masses. The molar mass of a helium atom is
Graham's Law describes the relationship between gas particle mass and velocity:
Using the molar masses of the particles in question, we can determine their relationship.
← Didn't Know|Knew It →
Phase diagrams are used to depict changes in the properties of a solution at different temperatures and pressures. Below is a phase diagram of a polar solution.
In section 3, as the temperature increases, the velocity of the molecules in a(n) manner.
Phase diagrams are used to depict changes in the properties of a solution at different temperatures and pressures. Below is a phase diagram of a polar solution.
In section 3, as the temperature increases, the velocity of the molecules in a(n) manner.
Tap to reveal answer
This question asks you how the velocity of the molecules changes with increasing temperature. From molecular kinteics, we know that temperature is proportional to kinetic energy.
We can see that as temperature rises, the kinetic energy rises, however, the question asks us how the velocity changes. Now, we need to know how kinetic energy and velocity are related. We can pull this relationship from Newtonian mechanics.
If we simplify, we can see that . Velocity increases with increasing temperature, but in an indirectly proportional manner.
This question asks you how the velocity of the molecules changes with increasing temperature. From molecular kinteics, we know that temperature is proportional to kinetic energy.
We can see that as temperature rises, the kinetic energy rises, however, the question asks us how the velocity changes. Now, we need to know how kinetic energy and velocity are related. We can pull this relationship from Newtonian mechanics.
If we simplify, we can see that
← Didn't Know|Knew It →
At room temperature which of the following equimolar gases has the fastest effusion rate?
At room temperature which of the following equimolar gases has the fastest effusion rate?
Tap to reveal answer
According to Graham's law, the rate of effusion of a gas is inversely proportional to the square root of the mass: .
The gas with the lowest molecular weight will effuse the fastest. has the lowest molecular weight of the given gasses, with a value of .
According to Graham's law, the rate of effusion of a gas is inversely proportional to the square root of the mass:
The gas with the lowest molecular weight will effuse the fastest.
← Didn't Know|Knew It →
Consider a helium atom and a molecule of carbon monoxide both at a temperature of . Which of the following accurately describes the velocity of the carbon monoxide molecule in relation to the velocity of the helium atom?
Consider a helium atom and a molecule of carbon monoxide both at a temperature of
Tap to reveal answer
Since both molecules are at the same temperature, the value of the temperature is irrelevant. The difference in velocity between the two molecules depends on the difference in their molar masses. The molar mass of a helium atom is , and the molar mass of a carbon monoxide molecule is .
Graham's Law describes the relationship between gas particle mass and velocity:
Using the molar masses of the particles in question, we can determine their relationship.
Since both molecules are at the same temperature, the value of the temperature is irrelevant. The difference in velocity between the two molecules depends on the difference in their molar masses. The molar mass of a helium atom is
Graham's Law describes the relationship between gas particle mass and velocity:
Using the molar masses of the particles in question, we can determine their relationship.
← Didn't Know|Knew It →
Phase diagrams are used to depict changes in the properties of a solution at different temperatures and pressures. Below is a phase diagram of a polar solution.
In section 3, as the temperature increases, the velocity of the molecules in a(n) manner.
Phase diagrams are used to depict changes in the properties of a solution at different temperatures and pressures. Below is a phase diagram of a polar solution.
In section 3, as the temperature increases, the velocity of the molecules in a(n) manner.
Tap to reveal answer
This question asks you how the velocity of the molecules changes with increasing temperature. From molecular kinteics, we know that temperature is proportional to kinetic energy.
We can see that as temperature rises, the kinetic energy rises, however, the question asks us how the velocity changes. Now, we need to know how kinetic energy and velocity are related. We can pull this relationship from Newtonian mechanics.
If we simplify, we can see that . Velocity increases with increasing temperature, but in an indirectly proportional manner.
This question asks you how the velocity of the molecules changes with increasing temperature. From molecular kinteics, we know that temperature is proportional to kinetic energy.
We can see that as temperature rises, the kinetic energy rises, however, the question asks us how the velocity changes. Now, we need to know how kinetic energy and velocity are related. We can pull this relationship from Newtonian mechanics.
If we simplify, we can see that
← Didn't Know|Knew It →
At room temperature which of the following equimolar gases has the fastest effusion rate?
At room temperature which of the following equimolar gases has the fastest effusion rate?
Tap to reveal answer
According to Graham's law, the rate of effusion of a gas is inversely proportional to the square root of the mass: .
The gas with the lowest molecular weight will effuse the fastest. has the lowest molecular weight of the given gasses, with a value of .
According to Graham's law, the rate of effusion of a gas is inversely proportional to the square root of the mass:
The gas with the lowest molecular weight will effuse the fastest.
← Didn't Know|Knew It →
Consider a helium atom and a molecule of carbon monoxide both at a temperature of . Which of the following accurately describes the velocity of the carbon monoxide molecule in relation to the velocity of the helium atom?
Consider a helium atom and a molecule of carbon monoxide both at a temperature of
Tap to reveal answer
Since both molecules are at the same temperature, the value of the temperature is irrelevant. The difference in velocity between the two molecules depends on the difference in their molar masses. The molar mass of a helium atom is , and the molar mass of a carbon monoxide molecule is .
Graham's Law describes the relationship between gas particle mass and velocity:
Using the molar masses of the particles in question, we can determine their relationship.
Since both molecules are at the same temperature, the value of the temperature is irrelevant. The difference in velocity between the two molecules depends on the difference in their molar masses. The molar mass of a helium atom is
Graham's Law describes the relationship between gas particle mass and velocity:
Using the molar masses of the particles in question, we can determine their relationship.
← Didn't Know|Knew It →
Phase diagrams are used to depict changes in the properties of a solution at different temperatures and pressures. Below is a phase diagram of a polar solution.
In section 3, as the temperature increases, the velocity of the molecules in a(n) manner.
Phase diagrams are used to depict changes in the properties of a solution at different temperatures and pressures. Below is a phase diagram of a polar solution.
In section 3, as the temperature increases, the velocity of the molecules in a(n) manner.
Tap to reveal answer
This question asks you how the velocity of the molecules changes with increasing temperature. From molecular kinteics, we know that temperature is proportional to kinetic energy.
We can see that as temperature rises, the kinetic energy rises, however, the question asks us how the velocity changes. Now, we need to know how kinetic energy and velocity are related. We can pull this relationship from Newtonian mechanics.
If we simplify, we can see that . Velocity increases with increasing temperature, but in an indirectly proportional manner.
This question asks you how the velocity of the molecules changes with increasing temperature. From molecular kinteics, we know that temperature is proportional to kinetic energy.
We can see that as temperature rises, the kinetic energy rises, however, the question asks us how the velocity changes. Now, we need to know how kinetic energy and velocity are related. We can pull this relationship from Newtonian mechanics.
If we simplify, we can see that
← Didn't Know|Knew It →
At room temperature which of the following equimolar gases has the fastest effusion rate?
At room temperature which of the following equimolar gases has the fastest effusion rate?
Tap to reveal answer
According to Graham's law, the rate of effusion of a gas is inversely proportional to the square root of the mass: .
The gas with the lowest molecular weight will effuse the fastest. has the lowest molecular weight of the given gasses, with a value of .
According to Graham's law, the rate of effusion of a gas is inversely proportional to the square root of the mass:
The gas with the lowest molecular weight will effuse the fastest.
← Didn't Know|Knew It →
Consider a helium atom and a molecule of carbon monoxide both at a temperature of . Which of the following accurately describes the velocity of the carbon monoxide molecule in relation to the velocity of the helium atom?
Consider a helium atom and a molecule of carbon monoxide both at a temperature of
Tap to reveal answer
Since both molecules are at the same temperature, the value of the temperature is irrelevant. The difference in velocity between the two molecules depends on the difference in their molar masses. The molar mass of a helium atom is , and the molar mass of a carbon monoxide molecule is .
Graham's Law describes the relationship between gas particle mass and velocity:
Using the molar masses of the particles in question, we can determine their relationship.
Since both molecules are at the same temperature, the value of the temperature is irrelevant. The difference in velocity between the two molecules depends on the difference in their molar masses. The molar mass of a helium atom is
Graham's Law describes the relationship between gas particle mass and velocity:
Using the molar masses of the particles in question, we can determine their relationship.
← Didn't Know|Knew It →
Phase diagrams are used to depict changes in the properties of a solution at different temperatures and pressures. Below is a phase diagram of a polar solution.
In section 3, as the temperature increases, the velocity of the molecules in a(n) manner.
Phase diagrams are used to depict changes in the properties of a solution at different temperatures and pressures. Below is a phase diagram of a polar solution.
In section 3, as the temperature increases, the velocity of the molecules in a(n) manner.
Tap to reveal answer
This question asks you how the velocity of the molecules changes with increasing temperature. From molecular kinteics, we know that temperature is proportional to kinetic energy.
We can see that as temperature rises, the kinetic energy rises, however, the question asks us how the velocity changes. Now, we need to know how kinetic energy and velocity are related. We can pull this relationship from Newtonian mechanics.
If we simplify, we can see that . Velocity increases with increasing temperature, but in an indirectly proportional manner.
This question asks you how the velocity of the molecules changes with increasing temperature. From molecular kinteics, we know that temperature is proportional to kinetic energy.
We can see that as temperature rises, the kinetic energy rises, however, the question asks us how the velocity changes. Now, we need to know how kinetic energy and velocity are related. We can pull this relationship from Newtonian mechanics.
If we simplify, we can see that
← Didn't Know|Knew It →
At room temperature which of the following equimolar gases has the fastest effusion rate?
At room temperature which of the following equimolar gases has the fastest effusion rate?
Tap to reveal answer
According to Graham's law, the rate of effusion of a gas is inversely proportional to the square root of the mass: .
The gas with the lowest molecular weight will effuse the fastest. has the lowest molecular weight of the given gasses, with a value of .
According to Graham's law, the rate of effusion of a gas is inversely proportional to the square root of the mass:
The gas with the lowest molecular weight will effuse the fastest.
← Didn't Know|Knew It →
Consider a helium atom and a molecule of carbon monoxide both at a temperature of . Which of the following accurately describes the velocity of the carbon monoxide molecule in relation to the velocity of the helium atom?
Consider a helium atom and a molecule of carbon monoxide both at a temperature of
Tap to reveal answer
Since both molecules are at the same temperature, the value of the temperature is irrelevant. The difference in velocity between the two molecules depends on the difference in their molar masses. The molar mass of a helium atom is , and the molar mass of a carbon monoxide molecule is .
Graham's Law describes the relationship between gas particle mass and velocity:
Using the molar masses of the particles in question, we can determine their relationship.
Since both molecules are at the same temperature, the value of the temperature is irrelevant. The difference in velocity between the two molecules depends on the difference in their molar masses. The molar mass of a helium atom is
Graham's Law describes the relationship between gas particle mass and velocity:
Using the molar masses of the particles in question, we can determine their relationship.
← Didn't Know|Knew It →
Phase diagrams are used to depict changes in the properties of a solution at different temperatures and pressures. Below is a phase diagram of a polar solution.
In section 3, as the temperature increases, the velocity of the molecules in a(n) manner.
Phase diagrams are used to depict changes in the properties of a solution at different temperatures and pressures. Below is a phase diagram of a polar solution.
In section 3, as the temperature increases, the velocity of the molecules in a(n) manner.
Tap to reveal answer
This question asks you how the velocity of the molecules changes with increasing temperature. From molecular kinteics, we know that temperature is proportional to kinetic energy.
We can see that as temperature rises, the kinetic energy rises, however, the question asks us how the velocity changes. Now, we need to know how kinetic energy and velocity are related. We can pull this relationship from Newtonian mechanics.
If we simplify, we can see that . Velocity increases with increasing temperature, but in an indirectly proportional manner.
This question asks you how the velocity of the molecules changes with increasing temperature. From molecular kinteics, we know that temperature is proportional to kinetic energy.
We can see that as temperature rises, the kinetic energy rises, however, the question asks us how the velocity changes. Now, we need to know how kinetic energy and velocity are related. We can pull this relationship from Newtonian mechanics.
If we simplify, we can see that
← Didn't Know|Knew It →
At room temperature which of the following equimolar gases has the fastest effusion rate?
At room temperature which of the following equimolar gases has the fastest effusion rate?
Tap to reveal answer
According to Graham's law, the rate of effusion of a gas is inversely proportional to the square root of the mass: .
The gas with the lowest molecular weight will effuse the fastest. has the lowest molecular weight of the given gasses, with a value of .
According to Graham's law, the rate of effusion of a gas is inversely proportional to the square root of the mass:
The gas with the lowest molecular weight will effuse the fastest.
← Didn't Know|Knew It →