Answer to Question #201915 in Inorganic Chemistry for AG SERUMULA

Question #201915

Calculate the total amount of energy (in kJ) necessary to raise the temperature of 2.00 L of ethanol (density = 0.7849 g/cm3 ) from 18 0C to its boiling point (78.3 0C) and then to fully vaporize the liquid. Assume that it is a closed system where no heat exchange with the surroundings take place. (Given: Cethanol = 2.44 J/g·K; heat of vaporization of ethanol at 78.3 0C = 38.56 kJ/mol.)


1
Expert's answer
2021-06-02T06:31:34-0400

The value of heat is "q=mC\\Delta T"


"q=1569 \u00d72.44\u00d7(78.3-18)"


"q=230.967kJ"


Heat required to vaporize "=34.10 \u00d7\\Delta H _{vap}" =1315.23kJ


Hence proved.


Need a fast expert's response?

Submit order

and get a quick answer at the best price

for any assignment or question with DETAILED EXPLANATIONS!

Comments

No comments. Be the first!

Leave a comment

LATEST TUTORIALS
New on Blog
APPROVED BY CLIENTS