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

Chemistry
Tutor: None Selected Time limit: 1 Day

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

Thank you for the opportunity to help you with your question!

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


Please let me know if you need any clarification. I'm always happy to answer your questions.
Jun 2nd, 2015

Studypool's Notebank makes it easy to buy and sell old notes, study guides, reviews, etc.
Click to visit
The Notebank
...
Jun 2nd, 2015
...
Jun 2nd, 2015
Dec 6th, 2016
check_circle
Mark as Final Answer
check_circle
Unmark as Final Answer
check_circle
Final Answer

Secure Information

Content will be erased after question is completed.

check_circle
Final Answer