If 575 grams of frozen ethonal are warmed to the freezing point of ethanol, how much heat is required to melt all of this frozen ethanol, CH3CH2OH, at the freezing point? The molar heat of vaporization of ethanol= 4.95 kj/mol

Please help I dont understand, i'll be grateful to the person who answers :((

1 Answer
1s2s2p
Feb 9, 2018

#6.19*10^4J=61.9kJ#

Explanation:

#DeltaE=L_mDeltan#, where:

  • #DeltaE# = change in energy (#J#)
  • #L_m# = molar heat of vaporization (#kJcolor(white)(l)mol^(-1)#)
  • #Deltan# = change in moles (#mol#)

#n("CH"_3"CH"_2"OH")=(m("CH"_3"CH"_2"OH"))/(M_r("CH"_3"CH"_2"OH"))=575/46=12.5mol#

#DeltaE=12.5*4.95=61.875kJ=6.19*10^4J#

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