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Assertion (A): Specific heat at constant pressure for an ideal gas is always greater than the specific heat at constant volume.
Reason (R): Heat added at constant volume is not utilized for doing any external work.
- a)Both A and R are individually true and R is the correct explanation of A
- b)Both A and R are individually true but R is NOT the correct explanation of A
- c)A is true but R is false
- d)A is false but R is true
Correct answer is option 'A'. Can you explain this answer?
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Assertion (A): Specific heat at constant pressure for an ideal gas is ...
Both A and R correct and R is the correct explanation of A
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Assertion (A): Specific heat at constant pressure for an ideal gas is ...
Specific heat at constant pressure for an ideal gas is always greater than the specific heat at constant volume. This statement is true and can be explained by the following reasoning:
Reasoning:
Heat added at constant volume is not utilized for doing any external work.
Explanation:
Specific heat is defined as the amount of heat energy required to raise the temperature of a substance by a certain amount. There are two types of specific heat for gases: specific heat at constant pressure (Cp) and specific heat at constant volume (Cv).
Specific heat at constant pressure (Cp) is the heat capacity of a substance when the pressure is kept constant during the process. It represents the ability of a substance to absorb heat energy when the volume changes.
On the other hand, specific heat at constant volume (Cv) is the heat capacity of a substance when the volume is kept constant during the process. It represents the ability of a substance to absorb heat energy when the pressure changes.
Assertion (A): Specific heat at constant pressure for an ideal gas is always greater than the specific heat at constant volume.
This assertion is true. The specific heat at constant pressure (Cp) is always greater than the specific heat at constant volume (Cv) for an ideal gas. This is because, during a constant pressure process, the gas is allowed to expand, and some of the heat energy is used to do work against the external pressure. This means that more heat energy is required to raise the temperature of the gas by a certain amount.
Reason (R): Heat added at constant volume is not utilized for doing any external work.
This reason is true and provides the correct explanation for Assertion (A). When heat is added to a gas at constant volume, the gas does not expand, and no external work is done. Therefore, all the heat energy added is used to increase the internal energy of the gas, resulting in a smaller increase in temperature compared to a constant pressure process. This is why the specific heat at constant volume (Cv) is always smaller than the specific heat at constant pressure (Cp) for an ideal gas.
In conclusion, both Assertion (A) and Reason (R) are individually true, and Reason (R) is the correct explanation of Assertion (A).
Reasoning:
Heat added at constant volume is not utilized for doing any external work.
Explanation:
Specific heat is defined as the amount of heat energy required to raise the temperature of a substance by a certain amount. There are two types of specific heat for gases: specific heat at constant pressure (Cp) and specific heat at constant volume (Cv).
Specific heat at constant pressure (Cp) is the heat capacity of a substance when the pressure is kept constant during the process. It represents the ability of a substance to absorb heat energy when the volume changes.
On the other hand, specific heat at constant volume (Cv) is the heat capacity of a substance when the volume is kept constant during the process. It represents the ability of a substance to absorb heat energy when the pressure changes.
Assertion (A): Specific heat at constant pressure for an ideal gas is always greater than the specific heat at constant volume.
This assertion is true. The specific heat at constant pressure (Cp) is always greater than the specific heat at constant volume (Cv) for an ideal gas. This is because, during a constant pressure process, the gas is allowed to expand, and some of the heat energy is used to do work against the external pressure. This means that more heat energy is required to raise the temperature of the gas by a certain amount.
Reason (R): Heat added at constant volume is not utilized for doing any external work.
This reason is true and provides the correct explanation for Assertion (A). When heat is added to a gas at constant volume, the gas does not expand, and no external work is done. Therefore, all the heat energy added is used to increase the internal energy of the gas, resulting in a smaller increase in temperature compared to a constant pressure process. This is why the specific heat at constant volume (Cv) is always smaller than the specific heat at constant pressure (Cp) for an ideal gas.
In conclusion, both Assertion (A) and Reason (R) are individually true, and Reason (R) is the correct explanation of Assertion (A).
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Assertion (A): Specific heat at constant pressure for an ideal gas is always greater than the specific heat at constant volume.Reason (R): Heat added at constant volume is not utilized for doing any external work.a)Both A and R are individually true and R is the correct explanation of Ab)Both A and R are individually true but R is NOT the correct explanation of Ac)A is true but R is falsed)A is false but R is trueCorrect answer is option 'A'. Can you explain this answer?
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ample number of questions to practice Assertion (A): Specific heat at constant pressure for an ideal gas is always greater than the specific heat at constant volume.Reason (R): Heat added at constant volume is not utilized for doing any external work.a)Both A and R are individually true and R is the correct explanation of Ab)Both A and R are individually true but R is NOT the correct explanation of Ac)A is true but R is falsed)A is false but R is trueCorrect answer is option 'A'. Can you explain this answer? tests, examples and also practice Mechanical Engineering tests.
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