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The familiar "ether" used as an anesthetic agent is diethyl ether, C4H10O. Its heat of...

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user8876431 | eNotes Newbie

Posted March 23, 2013 at 3:36 PM via web

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The familiar "ether" used as an anesthetic agent is diethyl ether, C4H10O. Its heat of vaporization is +26.5 kJ/mol at its boiling point. How much energy in kilojoules is required to convert 100 mL of diethyl ether at its boiling point from liquid to vapor if its density is 0.7138 g/mL?

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jerichorayel | College Teacher | (Level 1) Senior Educator

Posted March 23, 2013 at 5:42 PM (Answer #1)

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Transforming one mole of ether from liquid to vapor requires 26.5 kilojoules. To solve this problem, first we need to find the amount of moles of ether to be vaporized. To solve this first, we need to get the amount of ether in mass then convert it to moles using the molar mass of ether.

mL -> grams

`100 mL * (0.7138 grams Ether)/(1 mL)`

= 71.38 grams ether

Grams -> moles

`71.38 grams Ether * (1 mol e Ether)/(74.12 grams Ether)`

= 0.9630 moles ether

Moles -> amount of heat (in kJ)

`0.9630 mol es Ether * (26.5 kJ)/(1 mol e Ether)`

= 25.52037 = 25.5 kJ heat needed to convert 100mL liquid ether to vapor.

 

 

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