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Find internal energy
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Asked by ashutosharnold1998 | 03 Nov, 2019, 20:22: PM
Given:
For the change:
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ΔH = H1+ H2
n = 1 mole
T = 100 °C
H1 = nCdT
= 1× (-4.2)×18×100
= -7560 J/mol
= -7.56 kJ/mol
H2 = -6 kJ/mol
ΔH = -7.56 + (-6)
ΔH = -13.56 kJ/mol
In the process the volume change is negligible
Therefore, ΔH = ΔU +PΔV
ΔV =0
Change in internal energy = -13.56 kJ/mol
Answered by Varsha | 05 Nov, 2019, 11:47: AM
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