Use the following data for ethanol (C2H5OH) to determine the amount of heat (in

Question

Use the following data for ethanol (C2H5OH) to determine the amount of heat (in kJ) required to convert all 75 g of ethanol at 9 °C completely into the vapor phase at 78 °C. Enter your answer to one (1) decimal place.
MP = –114 °C BP = 78 °C Hfus = 5.06 kJ/mol Hvap = 38.56 kJ/mol Csolid = 0.97 J/gK Cliquid = 2.3 J/gK Use the following data for ethanol (C2H5OH) to determine the amount of heat (in kJ) required to convert all 75 g of ethanol at 9 °C completely into the vapor phase at 78 °C. Enter your answer to one (1) decimal place.
MP = –114 °C BP = 78 °C Hfus = 5.06 kJ/mol Hvap = 38.56 kJ/mol Csolid = 0.97 J/gK Cliquid = 2.3 J/gK Use the following data for ethanol (C2H5OH) to determine the amount of heat (in kJ) required to convert all 75 g of ethanol at 9 °C completely into the vapor phase at 78 °C. Enter your answer to one (1) decimal place.
MP = –114 °C BP = 78 °C Hfus = 5.06 kJ/mol Hvap = 38.56 kJ/mol Csolid = 0.97 J/gK Cliquid = 2.3 J/gK

Explanation / Answer

The ethanol will be in liquid phase at 9°C.

So to take it to 78°C we require msT amount of heat i.e. 75×2.3×(78-9) i.e 11.9kJ.

To take it into vapour phase we will need nH amout of heat where n is number of moles of ethanol i.e. 75/46 =1.63 moles.

So heat will be 1.63×38.56 i.e. 62.85kJ.

So total heat will be 62.85+11.9=74.8kJ

Related Questions

Navigate

• Browse (All)
• Browse U
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.