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Physical Chemistry

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29 Jan 2008 12:08:28 IST

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521

tell which is correct?

None

one mole of monoatomic ideal gas at 300 k expands adiabatically against a constant external prssure of of 1 atm frm a vol. of10litres to a vol. of 20litres calculate enthalpy change for d process

if we calculate change in internal energy frm 1st law of t.d.: it comes out 2 be

-1013 j & change in enthalpy as H=U+P(CHANGE IN VOLUME) DEN THE ASWER COMES 2 B ZERO

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GAURAV

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29 Jan 2008 12:09:57 IST

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HOWEVER IF WE USE H=

U EN ANSWER COMES DIFFERENT TELL HW?

GAURAV

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9 Feb 2008 12:26:43 IST

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any eperts plz answer it

Ranjeet Panda

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9 Feb 2008 12:34:03 IST

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E=W+Q
Since Q=0 (adiabatic)

E=W=10 Lit atm.
(Convert units)

Ranjeet Panda

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9 Feb 2008 12:36:37 IST

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Sorry perhaps i am incorrect

chetan

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9 Feb 2008 12:55:40 IST

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H =

U + P

V
      = 0    + 1.013*10⁵N/m²* (20-10)*10^-3
      = 1013J

Bipin Dubey

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24 Feb 2008 11:01:40 IST

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since T is constant

U=0 (for an ideal gas).

H = U + PV

H =

U + P

V (since P is constant)

Put the values you'll get 1013 J.

GAURAV

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3 Mar 2008 12:30:24 IST

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but man at constant temp change inenhalpy must be zero as delta t is zero

GAURAV

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3 Mar 2008 12:30:51 IST

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sorrry dats is enthalpy

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