Question

Enter your answer in the provided box. From the data below, calculate the total heat (in J) needed to convert 0.172 mol of gaseous ethanol at 300.0°C and 1 atm to liquid ethanol at 25.0°C and 1 atm: AH 40.5 kJ/mol b.p. at 1 atm: 78.5°C vap Cliquid 2.45 J/goC 1.43 J/goC Cgas

Answer 1

no of mol of ethanol gas taken(n) = 0.172 mol

mass of ethanol gas taken(m) = 0.172*46 = 7.912 g

heat released(q) = mgas*Cgas*DT1+n*DHvap+mliquid*Cliquid*DT2

mgas = 7.912 g

cgas = 1.43 j/g.c

DT1 = 300-78.5

n = 0.172 mol

DHvap = 40.5*10^3 j/mol

mliquid = 7.912 g

cliquid = 2.45 j/g.c

DT1 = 78.5-25

heat released(q) = 7.912*1.43*(300-78.5)+0.172*40.5*10^3+7.912*2.45*(78.5-25)

                 = 10509 joule

answer: 10509 joule