Question

A substance has the following properties:

Heat capacities:


1.34 J/g oC (solid)
3.02 J/g oC (liquid)
2.55 J/g oC (gas)


Heat of Fusion = 4.23 kJ/mole
Heat of Vaporization = 23.5 kJ/mole
Melting Point = -30.0 oC
Boiling Point = 88.5 oC
Molar Mass = 96.3 g/mole

How much energy (in kJ) would be needed to heat 5.55 g of this substance from -19.0 to 19.0oC?

Enter the E1 - E5 energies and the total energy in the spaces below. Recall that

E1 is the energy absorbed by the solid up to the final temperature or melting point (whichever is reached first)

Answer 1

E2 is the energy absorbed when the solid is converted to a liquid
E3 is the energy absorbed by the liquid up to the final temperature or boiling point (whichever is reached first)
E4 is the energy absorbed when the liquid is converted to a gas
E5 is the energy absorbed by the gas.

One or more of the energies may be 0 kJ.



E1 (in kJ) - report answer to 2 decimal places (Tol: ± 0)
E2 (in kJ) - report answer to 2 decimal places (Tol: ± 0)
E3 (in kJ) - report answer to 2 decimal places (Tol: ± 0.01)
E4 (in kJ) - report answer to 2 decimal places (Tol: ± 0)
E5 (in kJ) - report answer to 2 decimal places (Tol: ± 0)
Etotal (in kJ) (Tol: ± 0.01)

Answer 2

@ganeshie8 @Abhisar @Luigi0210

Answer 3

so far what I can see
Melting Point = -30.0 oC
Boiling Point = 88.5 oC
your transition from -19C to +19C will be in liquid phase without change states
only you will need to calculate E3 with the 3.02 J/g oC (liquid)
E=m x C x delta T
The C is in J/gC, your final result has to be converted to kJ
The molar mass I don't know if you need to convert in kJ/mol or you just can express your results as kJ/g.
All the others E values are 0kJ