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The internal energy of an ideal gas is a function of
- a)pressure only
- b)absolute temperature only
- c)pressure and volume
- d)pressure, volume and temperature
Correct answer is option 'B'. Can you explain this answer?
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The internal energy of an ideal gas is a function ofa)pressure onlyb)a...
Internal Energy of an Ideal Gas
Internal energy of an ideal gas is a function of absolute temperature only. This can be explained by the following points:
Definition of Internal Energy
Internal energy is the sum of all microscopic forms of energy of a system. For an ideal gas, internal energy is solely determined by the motion of its molecules, which is directly related to temperature.
Microscopic Explanation
In an ideal gas, molecules move randomly in all directions. As temperature increases, the average kinetic energy of the molecules also increases. This results in higher internal energy of the gas.
Mathematical Relationship
According to the ideal gas law, the internal energy of an ideal gas is directly proportional to its absolute temperature. The equation for internal energy of an ideal gas is given by U = nCvT, where U is the internal energy, n is the number of moles, Cv is the molar specific heat at constant volume, and T is the absolute temperature.
Pressure and Volume
While pressure and volume do affect the state of an ideal gas, they do not directly determine the internal energy of the gas. Internal energy is a function of temperature, which is a measure of the average kinetic energy of the gas molecules.
Therefore, the internal energy of an ideal gas is solely dependent on the absolute temperature, making option 'B' the correct choice.
Internal energy of an ideal gas is a function of absolute temperature only. This can be explained by the following points:
Definition of Internal Energy
Internal energy is the sum of all microscopic forms of energy of a system. For an ideal gas, internal energy is solely determined by the motion of its molecules, which is directly related to temperature.
Microscopic Explanation
In an ideal gas, molecules move randomly in all directions. As temperature increases, the average kinetic energy of the molecules also increases. This results in higher internal energy of the gas.
Mathematical Relationship
According to the ideal gas law, the internal energy of an ideal gas is directly proportional to its absolute temperature. The equation for internal energy of an ideal gas is given by U = nCvT, where U is the internal energy, n is the number of moles, Cv is the molar specific heat at constant volume, and T is the absolute temperature.
Pressure and Volume
While pressure and volume do affect the state of an ideal gas, they do not directly determine the internal energy of the gas. Internal energy is a function of temperature, which is a measure of the average kinetic energy of the gas molecules.
Therefore, the internal energy of an ideal gas is solely dependent on the absolute temperature, making option 'B' the correct choice.
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The internal energy of an ideal gas is a function ofa)pressure onlyb)absolute temperature onlyc)pressure and volumed)pressure, volume and temperatureCorrect answer is option 'B'. Can you explain this answer?
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