Work done in expansion of an ideal gas from 4 `dm^(3) ` to `6 dm^(3)`against a constant external pressure of 2.5 atm was usedup to heat1 mole of water at `20^(@)C`. Calculate the final temperature of water ( Given `:` specific heat of water `=4.184 Jg^(-1)K^(-1))`.

Work done in expansion of an ideal gas from 4 `dm^(3) ` to `6 dm^(3)`a

1.	Work done in expansion of an ideal gas from 4 `dm^(3) ` to `6 dm^(3)`against a constant external pressure of 2.5 atm was usedup to heat1 mole of water at `20^(@)C`. Calculate the final temperature of water ( Given `:` specific heat of water `=4.184 Jg^(-1)K^(-1))`.
Answer» As work is being against constant external pressure, the process is irreversible . Hence, ` w= - P _(ext)DeltaV = - 2.5 atm ( 6-4) dm^(3) = - 5L atm ` `( 1 dm^(3) = 1L)` `= - 5 xx 101.3 J = - 506.5 J ` `( 1L atm = 101.3J )` For isothermal expansion of an ideal gas , `DeltaU =0`so that`q= - w=506 .5 J` This heat is used up to heat 1 mole of water. Applying the reaction ` q= m xxc xx DeltaT` `= 506. 5 =18 xx4.184 xxDeltaT` or`DeltaT=6.725^(@)` `:.` Final temperature`=20 +6.725 ^(@) C =26.725^(@) C`

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Work done in expansion of an ideal gas from 4 `dm^(3) ` to `6 dm^(3)`against a constant external pressure of 2.5 atm was usedup to heat1 mole of water at `20^(@)C`. Calculate the final temperature of water ( Given `:` specific heat of water `=4.184 Jg^(-1)K^(-1))`.

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