Calculate the amount of energy released when 120.0g of diethyl ether (MW = 74.12 g/mol) is cooled from 53.0 C to 10.0 C ?
boiling point = 26.02 KJ/mol
specific heat capacity, (CH3)2 O(I) 3.74 J/(g.k)
specific heat capacity, (CH3)2 O(g) 2.35 J/(g.k)
Apply heat equation...
boiling point of diethyl ether = 34.6°C
therefore
expect change of phase from 53°C --> 34.6°C change, then 34.6°C to 10°C
note that this:
We require 2 type of heat, latent heat and sensible heat
Sensible heat (CP): heat change due to Temperature difference
Latent heat (LH): Heat involved in changing phases (no change of T)
Then
Q1 = mvapor * Cpvapor * (Tboiling - Tinitial)
Q2 = mvapor * Latent heat of condensation
Q3 = mvapor * Cpliquid * (Tfinal - Tboiling)
substitute
Q1 = 120* 3.74* (34.6- 53) = -8257.92
Q2 = 120* (-26.02*10^3) / 74.12 = -42126.28
Q3 = 120* 2.35* (10- 34.6) = -6937.2
Qtotal = q1+q2+q3 = -(8257.92 +42126.28+6937.2) = -57321.4 J
heat released = 57321.4 J = 57.321 kJ
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