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For the isothermal expansion of an ideal gas:
- a)E and H increases.
- b)E increases but H decreases.
- c)H increases and E decreases.
- d)E and H are unaltered.
Correct answer is 'D'. Can you explain this answer?
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Verified Answer
For the isothermal expansion of an ideal gas:a)E and H increases. b)E...
- Isothermal means the temperature does not change.
- Expansion means the volume has increased.
Therefore, isothermal expansion is the increase in volume under constant-temperature conditions.
In this situation, the gas does work, so the work is negatively-signed because the gas exerts energy to increase in volume.
During isothermal conditions, the change in internal energy ΔU is 0 for only an ideal gas, so efficient work done is entirely transformed into efficient heat flow.
Most Upvoted Answer
For the isothermal expansion of an ideal gas:a)E and H increases. b)E...
E depends upon the temp. of teh system (temp difference 0)H=U+PV==U +NRTSO U/E INTERNAL ENERGY IS AND CHANGE IN TEM PERATURE IS ALSO 0SO H =0
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For the isothermal expansion of an ideal gas:a)E and H increases. b)E...
E and H=0 bcoz: since for ideal gas E and H is function of temp. only and ∆T=0
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For the isothermal expansion of an ideal gas:a)E and H increases. b)E increases but H decreases.c)H increases and E decreases.d)E and H are unaltered.Correct answer is 'D'. Can you explain this answer?
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