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*H= -(1.00 mol)(40.656kJ/mol)

= -40.7 kJ

* since q=H (@ constant pressure)

there for q= -40.7 kJ

*w=nRT

=(1.00 mol)(8.315 J/mol.K)(373K)

= 3.1 kJ

* U= H-nRT

= (-40.7kJ)-(1.00 mol)(8.315 J/mol.K)(373K)

= -43.8kJ

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11y ago
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10y ago

Q = ( m ) ( Cp ) ( 100 - 67 ) + ( m ) ( h sub fg )

h sub fg = 40.7 kJ / mole ) 1000 J / kJ ) ( 1 mole / 18.105 g )

h sub fg = 2259 J / g

Q = ( 1.0 g ) ( 4.184 J/g - Cdeg ) ( 33 C deg ) + ( 1.0 g ) ( 2259 J/g )

Q = 138.1 J + 2259 J = 2397 J = 2.397 kJ <--------------

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15y ago

well you have not mentioned the complete unit...it is 49.79 kJ/mol or also 2.766 kJ/gram

just divide 49 Kj/mol by 18 g/mol (which is the molar mass of water) and have your answer.

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14y ago

1mol/4.68e10times40.79

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11y ago

no

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Anonymous

Lvl 1
4y ago

40.79J

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Q: A sample of 1mol of water is condensed isothermally and reversibly to liquid water at 100 degreethe standard enthalpy of vaporization of water is 40.656kj per mole find work and heat?
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