![\Delta H=[m\times c_{p,s}\times (T_{final}-T_{initial})]+n\times \Delta H_{fusion}+[m\times c_{p,l}\times (T_{final}-T_{initial})]+n\times \Delta H_{vap}+[m\times c_{p,g}\times (T_{final}-T_{initial})]](/tpl/images/0448/1498/e4ef0.png)
= enthalpy change = ?
= specific heat of solid ethanol= 0.97 J/gK
= specific heat of liquid ethanol = 2.31 J/gK
= enthalpy change for fusion = 5.02 KJ/mole = 5020 J/mole
= change in temperature ![\Delta H=[25.0 g\times 0.97J/gK\times (-114-(-135)K]+0.534mole\times 5020J/mole+[25.0g\times 2.31J/gK\times (-50-(-114))K]](/tpl/images/0448/1498/b9d5c.png)
  (1 KJ = 1000 J)Ethanol melts at -114 degree c. the enthalpy of fusion
is5.02kj/mol. the specific heat of soli...
Chemistry, 09.01.2020 06:31 JocelynC24
Ethanol melts at -114 degree c. the enthalpy of fusion
is5.02kj/mol. the specific heat of solid and liquid ethanol are
0.97jk/g-k and 2.31 j/g-k, respectively. how much heat(kj) is
needed toconvert 25.0 g of solid ethanol at -135 degree c to liquid
ethanolat -50 degree c?
Answers: 2
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