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If the gas at constant temperature and pressure expands, then its
Options
(a) internal energy increases
(b) internal energy remains the same
(c) internal energy decreases
(d) entropy increases and then decreases
Correct Answer:
internal energy remains the same
Explanation:
For an ideal gas, the internal energy depends upon temperature. As expansion takes place at constant temperature and pressure so internal energy of the gas remains constant, i.e. ΔE = 0.
Related Questions: - Choose isosteres from the following.
- Which of the following metals reacts with water
- An ideal gas, obeying kinetic theory of gases can not be liquefied, because
- The number of primary, secondary and tertiary carbons in 3,4-dimethylheptane
- The two polypeptide chains present in insulin contain which of the following number
Topics: States of Matter Gases and Liquids
(80)
Subject: Chemistry
(2512)
Important MCQs Based on Medical Entrance Examinations To Improve Your NEET Score
- Choose isosteres from the following.
- Which of the following metals reacts with water
- An ideal gas, obeying kinetic theory of gases can not be liquefied, because
- The number of primary, secondary and tertiary carbons in 3,4-dimethylheptane
- The two polypeptide chains present in insulin contain which of the following number
Topics: States of Matter Gases and Liquids (80)
Subject: Chemistry (2512)
Important MCQs Based on Medical Entrance Examinations To Improve Your NEET Score
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Internal energy at any state is a function of number of moles n and the temperature. If the the volume expansion takes place at constant temperature and pressure we see that using the gas equation PV=nRT, we get V∝n and thus the number of moles of gas are increasing(may be the gas is being introduces by an external agent), thus internal energy is increasing.
The internal energy remains same because internal energy directly depends upon temperatures and the temp is constant so internal energy also remains same