Question

Enter your answer in the provided box. From the data below, calculate the total heat (in...

Enter your answer in the provided box. From the data below, calculate the total heat (in J) needed to convert 0.602 mol of gaseous ethanol at 300.0°C and 1 atm to liquid ethanol at 25.0°C and 1 atm: b.p. at 1 atm: 78.5°C ΔH o vap : 40.5 kJ/mol cgas: 1.43 J/g·°C cliquid: 2.45 J/g·°C

Homework Answers

Answer #1

Q = mc∆T

Q = heat energy (Joules, J), m = mass of a substance (kg)

c = specific heat (units J/kg∙K), is a symbol meaning "the change in"

∆T = change in temperature (Kelvins, K)

gaseous ethanol going to get following 3 changes

1) As a gas the temperature reduces from  300.0°C to 78.5°C

2) Gas is converted to liquid

3) As a liquid the temperature redcues to 78.5°C to  25.0°C

Amount of heat needed

Q = 0.602 x 1.43 x (300-78.5) + 0.602 x 40500 /46.07 + 0.602 x 2.45 x (78.5 - 25 )

Q = 798.80 Joules

798.80 Joules of heat is required.

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