Thermodynamics - Physics
Card 0 of 192
A gas in a closed container is heated with 
of energy, causing the lid of the container to rise 
with 
of force. What is the total change in energy of the system?
A gas in a closed container is heated with
For this problem, use the first law of thermodynamics. The change in energy equals the increase in heat energy minus the work done.
We are not given a value for work, but we can solve for it using the force and distance. Work is the product of force and displacement.
Now that we have the value of work done and the value for heat added, we can solve for the total change in energy.
For this problem, use the first law of thermodynamics. The change in energy equals the increase in heat energy minus the work done.
We are not given a value for work, but we can solve for it using the force and distance. Work is the product of force and displacement.
Now that we have the value of work done and the value for heat added, we can solve for the total change in energy.
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A gas in a closed container is heated, causing the lid of the container to rise. The gas performs 
of work to raise the lid, such that is has a final total energy of 
. How much heat energy was added to the system?
A gas in a closed container is heated, causing the lid of the container to rise. The gas performs
For this problem, use the first law of thermodynamics. The change in energy equals the increase in heat energy minus the work done.
We are given the amount of work done by the gas and the total energy of the system. Using these values, we can solve for the heat added.
For this problem, use the first law of thermodynamics. The change in energy equals the increase in heat energy minus the work done.
We are given the amount of work done by the gas and the total energy of the system. Using these values, we can solve for the heat added.
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A gas in a closed container is heated with 
of energy, causing the lid of the container to rise. If the change in energy of the system is 
, how much work was done by the system?
A gas in a closed container is heated with
For this problem, use the first law of thermodynamics. The change in energy equals the increase in heat energy minus the work done.
We are given the total change in energy and the original amount of heat added. Using these values, we can solve for the work done by the system.
For this problem, use the first law of thermodynamics. The change in energy equals the increase in heat energy minus the work done.
We are given the total change in energy and the original amount of heat added. Using these values, we can solve for the work done by the system.
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Which of the following represents the first law of thermodynamics?
Which of the following represents the first law of thermodynamics?
The first law of thermodynamics is another wording of the law of conservation of energy. Effectively it states that energy cannot be created or destroyed, but it can change forms.
This means that, in the given situation of the ball rolling down the hill, the total initial energy equals the final kinetic energy plus heat.
The zeroth law of thermodynamics states that if a system is in equilibrium with two other systems, then the two other systems are in equilibrium with each other.
The second law of thermodynamics states that the entropy of a closed system will always increase.
The third law of thermodynamics states that absolute zero is the temperature at which entropy is zero.
The first law of thermodynamics is another wording of the law of conservation of energy. Effectively it states that energy cannot be created or destroyed, but it can change forms.
This means that, in the given situation of the ball rolling down the hill, the total initial energy equals the final kinetic energy plus heat.
The zeroth law of thermodynamics states that if a system is in equilibrium with two other systems, then the two other systems are in equilibrium with each other.
The second law of thermodynamics states that the entropy of a closed system will always increase.
The third law of thermodynamics states that absolute zero is the temperature at which entropy is zero.
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According to the first law of thermodynamics, in an isothermal process __________.
According to the first law of thermodynamics, in an isothermal process __________.
According to the first law of thermodynamics, change in internal energy of a closed system is given by the difference between the heat energy added to the system and the work done by the system:
In an isothermal process, temperature is constant. Temperature is a measure of internal energy of the system. If temperature is constant, then there is no fluctuation of internal energy.
It can be implied that heat added to the system is equal to work done by the system.
According to the first law of thermodynamics, change in internal energy of a closed system is given by the difference between the heat energy added to the system and the work done by the system:
In an isothermal process, temperature is constant. Temperature is a measure of internal energy of the system. If temperature is constant, then there is no fluctuation of internal energy.
It can be implied that heat added to the system is equal to work done by the system.
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A glass of cold water is placed in a sealed room. After an infinite amount of time, what will happen?
A glass of cold water is placed in a sealed room. After an infinite amount of time, what will happen?
The second law of thermodynamics states that closed systems constantly move towards a state of thermal equilibrium. Since we are looking at a closed system, that means we must be moving towards a state of equilibrium. The only way that happens is if the air cools and the water warms, until they both reach a new final temperature.
Looking at this question in terms of heat transfer, we can infer that the glass of water will warm up, but there must be a transfer of heat to the glass in order for this to occur. The heat comes from the air, causing it to cool as the glass warms.
The second law of thermodynamics states that closed systems constantly move towards a state of thermal equilibrium. Since we are looking at a closed system, that means we must be moving towards a state of equilibrium. The only way that happens is if the air cools and the water warms, until they both reach a new final temperature.
Looking at this question in terms of heat transfer, we can infer that the glass of water will warm up, but there must be a transfer of heat to the glass in order for this to occur. The heat comes from the air, causing it to cool as the glass warms.
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An object can never reach absolute zero in a finite number of steps. Which of these laws supports this statement?
An object can never reach absolute zero in a finite number of steps. Which of these laws supports this statement?
The third law of thermodynamics states that it is impossible to decrease the temperature of a system to absolute zero in a finite number of steps. To do so would require that the entropy of the system also reaches zero, suggesting that the atoms cease vibrating in the material and it has zero net energy. Such a process is not possible.
The third law of thermodynamics states that it is impossible to decrease the temperature of a system to absolute zero in a finite number of steps. To do so would require that the entropy of the system also reaches zero, suggesting that the atoms cease vibrating in the material and it has zero net energy. Such a process is not possible.
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Gas A is in thermal equilibrium with gases B and C. Which of the following is a valid conclusion?
Gas A is in thermal equilibrium with gases B and C. Which of the following is a valid conclusion?
The zeroth law of thermodynamics states that if two systems are in thermal equilibrium with a third system, they are in equilibrium with each other. If gas A is in equilibrium with gas B and gas C, then gas be and gas C must be in thermal equilibrium with each other.
The zeroth law of thermodynamics states that if two systems are in thermal equilibrium with a third system, they are in equilibrium with each other. If gas A is in equilibrium with gas B and gas C, then gas be and gas C must be in thermal equilibrium with each other.
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Three substances are added to a mug to make coffee: the coffee, which is 
, the milk, which is 
, and the sugar, which is in thermal equilibrium with the coffee. Describe the thermal state of the sugar.
Three substances are added to a mug to make coffee: the coffee, which is
The zeroth law of thermodynamics states that if two objects are in thermodynamic equilibrium with a third object, then they must be in thermodynamic equilibrium with each other. In this question, the coffee is in equilibrium with both the milk and the sugar, allowing us to conclude that the milk and sugar must be in equilibrium with each other.
The second law of thermodynamics states that the entropy of the universe is always increasing, and is not relevant to this particular scenario.
The zeroth law of thermodynamics states that if two objects are in thermodynamic equilibrium with a third object, then they must be in thermodynamic equilibrium with each other. In this question, the coffee is in equilibrium with both the milk and the sugar, allowing us to conclude that the milk and sugar must be in equilibrium with each other.
The second law of thermodynamics states that the entropy of the universe is always increasing, and is not relevant to this particular scenario.
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System A is in equilibrium with system C.
System B is in equilibrium with system C.
System A is in equilibrium with system B according to which law of thermodynamics?
System A is in equilibrium with system C.
System B is in equilibrium with system C.
System A is in equilibrium with system B according to which law of thermodynamics?
The zeroth law of thermodynamics states that if two separate systems are in equilibrium with a third system, then they are in equilibrium with each other. The zeroth law of thermodynamics is essentially equivalent to the transitive property of mathematics.
If 
and 
, then 
.
The first law of thermodynamics states that internal energy changes due to heat flow. Mathematically, this law is presented as 
.
The second law of thermodynamics states that the entropy (or disorder) of the universe is always increasing. Certain systems exist in which there is a local decrease in entropy, but these processes are always balanced by an increase of entropy outside of the system.
The third law of thermodynamics states that absolute zero is the state in which a system has zero entropy. Essentially, this means that it is impossible to reach absolute zero (at least with modern technology).
The zeroth law of thermodynamics states that if two separate systems are in equilibrium with a third system, then they are in equilibrium with each other. The zeroth law of thermodynamics is essentially equivalent to the transitive property of mathematics.
If
The first law of thermodynamics states that internal energy changes due to heat flow. Mathematically, this law is presented as
The second law of thermodynamics states that the entropy (or disorder) of the universe is always increasing. Certain systems exist in which there is a local decrease in entropy, but these processes are always balanced by an increase of entropy outside of the system.
The third law of thermodynamics states that absolute zero is the state in which a system has zero entropy. Essentially, this means that it is impossible to reach absolute zero (at least with modern technology).
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An ideal gas is inside of a tube at 
. If the pressure remains constant, but the volume decreases from 
to 
, what will be the final temperature in the tube?
An ideal gas is inside of a tube at
For this problem, use Charles's Law:
In this formula, 
is the volume and 
is the temperature. Charles's Law allows us to set up a proportion for changes in volume and temperature, as long as pressure remains constant. Since we are dealing with a proportion, the units for temperature are irrelevant and we do not need to convert to Kelvin.
Using the given values, we should be able to solve for the final temperature.
Cross multiply.
For this problem, use Charles's Law:
In this formula,
Using the given values, we should be able to solve for the final temperature.
Cross multiply.
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An ideal gas is inside of a container with a pressure of 
. If it starts with a volume of 
and is compressed to 
, what is the new pressure if the temperature remains constant?
An ideal gas is inside of a container with a pressure of
We will need to use Boyle's Law to solve:
Boyle's Law allows us to set up a relationship between the changes in pressure and volume under conditions with constant temperature. Since the equation is a proportion, we do not need to convert any units.
We can use the given values to solve for the new pressure.
We will need to use Boyle's Law to solve:
Boyle's Law allows us to set up a relationship between the changes in pressure and volume under conditions with constant temperature. Since the equation is a proportion, we do not need to convert any units.
We can use the given values to solve for the new pressure.
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An ideal gas is compressed from 
to 
at constant temperature. If the initial pressure was 
, what is the new pressure?
An ideal gas is compressed from
For this problem, use Boyle's Law:
Boyle's Law allows us to set up a proportion between the pressure and volume at a constant temperature.
Using the values given, we can solve for the final pressure.
For this problem, use Boyle's Law:
Boyle's Law allows us to set up a proportion between the pressure and volume at a constant temperature.
Using the values given, we can solve for the final pressure.
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A balloon in a hot room is submerged in a bucket of cold water. What will happen to this balloon?
A balloon in a hot room is submerged in a bucket of cold water. What will happen to this balloon?
The volume of air in the balloon will increase when exposed to hotter temperatures, and decrease when exposed to colder temperatures. If we look at the ideal gas law, we can see that temperature and volume have a direct relationship. As one goes down, so does the other, assuming all other factors remain constant.
We can also look at Charles's law of volumes:
The balloon is sealed, so the amount of gas in the balloon will not change, and the elasticity of the balloon means that pressure will also remain constant. As temperature decreases, volume must also decrease. Suppose that the temperature is halved in our question. The result would be half the volume, according to Charles's law.
By this logic, we can conclude that the balloon will shrink when placed in the cold water.
The volume of air in the balloon will increase when exposed to hotter temperatures, and decrease when exposed to colder temperatures. If we look at the ideal gas law, we can see that temperature and volume have a direct relationship. As one goes down, so does the other, assuming all other factors remain constant.
We can also look at Charles's law of volumes:
The balloon is sealed, so the amount of gas in the balloon will not change, and the elasticity of the balloon means that pressure will also remain constant. As temperature decreases, volume must also decrease. Suppose that the temperature is halved in our question. The result would be half the volume, according to Charles's law.
By this logic, we can conclude that the balloon will shrink when placed in the cold water.
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Why does adding heat cause a gas to expand?
Why does adding heat cause a gas to expand?
Heat is a form of energy. Adding heat to a gaseous system will increase the energy of the molecules, causing them to move faster and collide more frequently. This increased velocity results in the expansion of the gas.
Heat is a form of energy. Adding heat to a gaseous system will increase the energy of the molecules, causing them to move faster and collide more frequently. This increased velocity results in the expansion of the gas.
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The temperature of an ideal gas is raised from 
to 
. If the volume remains constant, what was its initial pressure if the final pressure is 
?
The temperature of an ideal gas is raised from
For this problem, use Gay-Lussac's law to set up a direct proportion between pressure and temperature. Note that this law only applies when volume is constant.
Plug in our given values and solve for the initial pressure.
For this problem, use Gay-Lussac's law to set up a direct proportion between pressure and temperature. Note that this law only applies when volume is constant.
Plug in our given values and solve for the initial pressure.
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A 
disc of copper is dropped into a 
glass of water. If the copper was at 
and the water was at 
, what is the new temperature of the mixture?
A
The relationship between mass and temperature, when two masses are mixed together, is:
Using the given values for the mass and specific heat of each compound, we can solve for the final temperature.
We need to work to isolate the final temperature.
Distribute into the parenthesis using multiplication.
Combine like terms.
The relationship between mass and temperature, when two masses are mixed together, is:
Using the given values for the mass and specific heat of each compound, we can solve for the final temperature.
We need to work to isolate the final temperature.
Distribute into the parenthesis using multiplication.
Combine like terms.
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of soup at 
cools down to 
after 
. If the specific heat of the soup is 
, how much energy does the soup release into the room?
The formula for heat energy is:
We are given the initial and final temperatures, mass, and specific heat. Using these values, we can find the heat released. Note that the time is irrelevant to this calculation.
That means that the soup "lost" 
of energy. This is the amount that it released into the room. The value is negative for the soup, the source of the heat, but positive for the room, which receives it.
The formula for heat energy is:
We are given the initial and final temperatures, mass, and specific heat. Using these values, we can find the heat released. Note that the time is irrelevant to this calculation.
That means that the soup "lost"
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of soup at 
cools down after 
. If the specific heat of the soup is 
, and it released 
of energy into the room, what is the final temperature of the soup?
The formula for heat energy is:
We are given the initial temperature, mass, specific heat, and heat released. Using these values, we can find the final temperature. Note that the time is irrelevant to this calculation. Since heat is released from the soup, the net change in the soup's energy is negative. Since the soup is cooling, we expect our answer to be less than 
.
The formula for heat energy is:
We are given the initial temperature, mass, specific heat, and heat released. Using these values, we can find the final temperature. Note that the time is irrelevant to this calculation. Since heat is released from the soup, the net change in the soup's energy is negative. Since the soup is cooling, we expect our answer to be less than
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of soup cools down to 
after 
. If the specific heat of the soup is 
, and it released 
of energy into the room, what was the initial temperature of the soup?
The formula for heat energy is:
We are given the final temperature, mass, specific heat, and heat released. Using these values, we can find the initial temperature. Note that the time is irrelevant to this calculation. Since heat is released from the soup, the net change in the soup's energy is negative. Since the soup is cooling, we expect our answer to be greater than 
.
The formula for heat energy is:
We are given the final temperature, mass, specific heat, and heat released. Using these values, we can find the initial temperature. Note that the time is irrelevant to this calculation. Since heat is released from the soup, the net change in the soup's energy is negative. Since the soup is cooling, we expect our answer to be greater than
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