For copper, Cu, the heat of fusion at its normal melting point of 1083 °C is 13.

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For copperCu, the heat of fusion at its normal melting point of 1083 °C is 13.0kJ/mol.


The entropy change when 2.34 moles of solid Cu melts at 1083 °C, 1 atm is  J/K.
Jun 2nd, 2015

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DATA:

Temperature= 1083C0 = 1356K

Heat of fusion (L)= 13.0KJ/mol

Moles of Cu= 2.34mol

Change in entropy(∆S)=?

SOLUTION:

MASS OF COPPER

L= Q/m

Q=L*m

Mass of Cu= moles of Cu*molecular mass of Cu

  = 2.34*63.546

  = 148.697g

Q=L*m

Q= 1300*148.697

Q= 1.9330*105J

FOR CHANGE IN ENTROPY

Q = T∆S

∆S= Q/T

∆S=1.9330*105/1356

∆S= 142.5516J/K


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Jun 2nd, 2015

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