Question

Calculate the final volume of one mole of an ideal gas initially at 0°C and 1 atm pressure, if it absorbs 100 cal heat during a reversible isothermal expansion.


Please tell fast..​

Answer 1

Answer:

The gas is in the standard temperature and pressure condition i.e. at S.T.P

Therefore,

Vi=22.4dm3

Vf=?

As given that the expansion is isothermal and reversible 

∴ΔU=0

Now from first law of thermodynamics,

ΔU=q+w

∵ΔU=0

∴q=–w

Given that the heat is absorbed.

∴q=1000cal

⇒w=−q=−1000cal

Now,

Work done in a reversible isothermal expansion is given by-

w=−nRTln(ViVf)

Given:-

T=0℃=273K

n=1 mol

∴1000=−nRTln(ViVf)

⇒1000=−1×2.303×2×273×log(22.4Vf)

⇒log(22.4Vf)=−2.303×273×21000

⇒

Explanation:

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