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For an ideal gas, which one of the following statements does not hold true?
- a)The speed of all gas molecules is same
- b)The kinetic energies of all gas molecules are not same
- c)The potential energy of the gas molecules is zero
- d)There is no interactive force between the molecules.
Correct answer is option 'A'. Can you explain this answer?
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Verified Answer
For an ideal gas, which one of the following statements does not hold ...
In an ideal gas, at any particular time, different particles in the gas have different speeds and hence different kinetic energies. This assumption is reasonable because as the particles collide, we expect their speed to change. Even if the initial speed of all the particles was the same, the molecular collisions will disrupt this uniformity. Hence statement 1 is incorrect and 2 is correct.
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For an ideal gas, which one of the following statements does not hold ...
Introduction:
In this question, we are asked to identify which statement about an ideal gas does not hold true. An ideal gas is a theoretical concept used in physics and chemistry to simplify the behavior of gases under certain conditions. It is important to understand the properties and characteristics of an ideal gas to apply the ideal gas law and other gas laws in various scientific calculations.
Statement Analysis:
Let's analyze each statement to determine if it holds true for an ideal gas.
a) The speed of all gas molecules is the same:
This statement is not true for an ideal gas. In an ideal gas, the gas molecules have a distribution of speeds. According to the Maxwell-Boltzmann distribution, the speeds of gas molecules in a sample follow a probability distribution. The distribution is characterized by an average speed, but individual gas molecules can have different speeds.
b) The kinetic energies of all gas molecules are not the same:
This statement is true for an ideal gas. The kinetic energy of a gas molecule depends on its mass and speed. Since the speeds of gas molecules in an ideal gas can vary, their kinetic energies will also vary. The kinetic energy of a gas molecule is given by the equation KE = (1/2)mv^2, where m is the mass and v is the velocity of the molecule.
c) The potential energy of the gas molecules is zero:
This statement is true for an ideal gas. In an ideal gas, the gas molecules are assumed to have negligible volume and do not interact with each other. Therefore, there is no potential energy associated with the interaction between gas molecules. The potential energy of an ideal gas is considered to be zero.
d) There is no interactive force between the molecules:
This statement is true for an ideal gas. In an ideal gas, the gas molecules are assumed to have no interactive forces between them. This means that there are no attractive or repulsive forces acting between the gas molecules. The absence of interactive forces allows the gas molecules to move independently of each other and exhibit ideal gas behavior.
Conclusion:
Based on the analysis, the statement that does not hold true for an ideal gas is "a) The speed of all gas molecules is the same." In an ideal gas, the speeds of gas molecules follow a distribution, and individual gas molecules can have different speeds.
In this question, we are asked to identify which statement about an ideal gas does not hold true. An ideal gas is a theoretical concept used in physics and chemistry to simplify the behavior of gases under certain conditions. It is important to understand the properties and characteristics of an ideal gas to apply the ideal gas law and other gas laws in various scientific calculations.
Statement Analysis:
Let's analyze each statement to determine if it holds true for an ideal gas.
a) The speed of all gas molecules is the same:
This statement is not true for an ideal gas. In an ideal gas, the gas molecules have a distribution of speeds. According to the Maxwell-Boltzmann distribution, the speeds of gas molecules in a sample follow a probability distribution. The distribution is characterized by an average speed, but individual gas molecules can have different speeds.
b) The kinetic energies of all gas molecules are not the same:
This statement is true for an ideal gas. The kinetic energy of a gas molecule depends on its mass and speed. Since the speeds of gas molecules in an ideal gas can vary, their kinetic energies will also vary. The kinetic energy of a gas molecule is given by the equation KE = (1/2)mv^2, where m is the mass and v is the velocity of the molecule.
c) The potential energy of the gas molecules is zero:
This statement is true for an ideal gas. In an ideal gas, the gas molecules are assumed to have negligible volume and do not interact with each other. Therefore, there is no potential energy associated with the interaction between gas molecules. The potential energy of an ideal gas is considered to be zero.
d) There is no interactive force between the molecules:
This statement is true for an ideal gas. In an ideal gas, the gas molecules are assumed to have no interactive forces between them. This means that there are no attractive or repulsive forces acting between the gas molecules. The absence of interactive forces allows the gas molecules to move independently of each other and exhibit ideal gas behavior.
Conclusion:
Based on the analysis, the statement that does not hold true for an ideal gas is "a) The speed of all gas molecules is the same." In an ideal gas, the speeds of gas molecules follow a distribution, and individual gas molecules can have different speeds.
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For an ideal gas, which one of the following statements does not hold true?a)The speed of all gas molecules is sameb)The kinetic energies of all gas molecules are not samec)The potential energy of the gas molecules is zerod)There is no interactive force between the molecules.Correct answer is option 'A'. Can you explain this answer?
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