how many joules are required to convert 10g of solid ethyl alcohol at 180.3 cm to the vapor state at the boiling point 78.3 c

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31-10-2022
Chemistry

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how many joules are required to convert 10g of solid ethyl alcohol at 180.3 cm to the vapor state at the boiling point 78.3 c

Answer :

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kjuli1766 kjuli1766 · Answer 1 · 2022-11-03T11:08:25-04:00

The total heat required is 15.83kJ.

Solution:

Mass m = 10 g

The initial temperature of ethyl alcohol = -180.3 deg C

Melting point of ethyl alcohol= -117.3 deg C

Specific heat of ethyl alcohol (solid ) = 0.971 J/g deg C

The heat is required to increase the temperature up to the melting point

Q1 = mC delta T

Q1 = 10 g X 0.971 J/g deg C X (-117.3 degC - (-180.3degC))

Q1 = 611.73 J

The heat required to melt the ethyl alcohol (at a constant temperature)

Q2 =m X[tex]H_{fus}[/tex]

Q2 =10g X 218J/g

Q2 =2180 J

boiling point of ethyl alcohol = 78.3 deg C

melting point =-117.3 deg C

Specific heat of ethyl alcohol (liquid) = 2.30 J/g deg C

The heat is required to increase the temperature up to the boiling point

Q3 = mC delta T

Q3 = 10 g X 2.30 J/g deg C X (78.3 deg C - (-117.3 deg C))

Q3 = 4498.8 J

The heat required to convert liquid ethyl alcohol into vapor (at constant temperature)

Q4 =m X Hvap

Q4 =10g X854 J/g

Q4 =8540 J

The heat is required to increase the temperature up to the boiling point

Total Heat required = Q1 +Q2 +Q3+Q4

=611.73 J+2180 J+4498.8 J+8540 J

Total Heat required=15830.53 J= 15.83kJ

The energy required to change the temperature of 1 gram of hydrogen by 1 degree is basically defined by the specific heat of the water. The amount of energy is 4.184 J. The heat required to turn 25 grams of water into steam is 56425 joules or 13500 calories. A related example shows how the energy is calculated as water changes from solid ice to vapor.

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