1.

Calculate the maximum work done when pressure on 10 g of hydrogen is reduced from 20 to 1 atm at a constant temperature of 273 K. The gas behaves ideally. Will there be any change in internal energy ? Also, calculate 'q'.

Answer»

Solution :We have,
`W=-2.303"nRT"log.(p_(1))/(p_(2))` …(Eqn. 4a)
n=number of moles of hydrogen`=("wt.in grams")/("mol.wt.")=(10)/(2)=5 "moles" `
Thus `W=-2.303xx5xx2xx273xxlog.(20)/(1)`
`=-8180 "CALORIES"`
Further, the CHANGE in state of the SYSTEM is from a GAS to a gas and THEREFORE, at constant temperature, internal energy will not change, i.e.,
`DeltaU=0`
Again, `q=DeltaU-W`
`0-(-8180)=8180 "calories"`.


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