From the data below, calculate the total heat (in J) needed to convert 0.602 moles of gaseous ethanol at 300.0 Celsius and 1 atm to liquid ethanol at 25.0 celsius and 1 atm: b.p. at 1 atm 78.5 celsius, ΔHvap: 40.5 Kj/mol, Cethanol (g) 1.43 j/g c, Cethanol(l) 2.45 j/g c

Question

From the data below, calculate the total heat (in J) needed to convert 0.602 moles of gaseous ethanol at 300.0 Celsius and 1 atm to liquid ethanol at 25.0 celsius and 1 atm: b.p. at 1 atm 78.5 celsius, ΔHvap: 40.5 Kj/mol,  Cethanol (g) 1.43 j/g c, Cethanol(l) 2.45 j/g c

aaronq · Answer

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$q_3=m*C_{(g)}*\Delta T$

$q_2=\Delta H_{vap}*n_{Et}$

$q_1=m*C_{(l)}*\Delta T$

$T_q=q_1+q_2+q_3$

Note that the heat capacities given are in "$J/g*C^{\;o}$" and $\Delta H_{vap}$ in "kJ/mol".