Question

How much heat energy is required to convert 81.5 g of solid ethanol at -114.5 °C...

How much heat energy is required to convert 81.5 g of solid ethanol at -114.5 °C to gasesous ethanol at 194.1 °C? The molar heat of fusion of ethanol is 4.60 kJ/mol and its molar heat of vaporization is 38.56 kJ/mol. Ethanol has a normal melting point of -114.5 °C and a normal boiling point of 78.4 °C. The specific heat capacity of liquid ethanol is 2.45 J/g·°C and that of gaseous ethanol is 1.43 J/g·°C.

Homework Answers

Answer #1

moles of ethanol = 81.5/46 = 1.77 moles.

a. heat to convert solid to liquid at -114.5 degrees celcius

q = deltaHfusion* moles

    = 4.6*1.77 = 8.142 KJ

b. heat liquid ethanol from -114.5 degrees celcius to 78.4 degrees celcius

q = msdeltaT

   = 81.5*2.45*(78.4-(-114.5))

   = 38517 J

c. heat to convert liquid to vapor

q = deltaHvaporization*moles

   = 38.56 *1.77

   = 68.25 KJ

d. heat steam from 78.4 degrees celcius to 194.1 degrees celcius

q = msdeltaT

   = 81.5*1.43*(194.1-78.4)

   =13484.3 J

Total energy = 8.142 KJ + 38.517 KJ + 68.25 KJ + 13.484 KJ

                     = 128.393 KJ

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
How much heat energy is required to convert 21.1 g of solid ethanol at -114.5 °C...
How much heat energy is required to convert 21.1 g of solid ethanol at -114.5 °C to gaseous ethanol at 191.5 °C? The molar heat of fusion of ethanol is 4.60 kJ/mol and its molar heat of vaporization is 38.56 kJ/mol. Ethanol has a normal melting point of -114.5 °C and a normal boiling point of 78.4 °C. The specific heat capacity of liquid ethanol is 2.45 J/g·°C and that of gaseous ethanol is 1.43 J/g·°C. ________kJ
How much energy (in kilojoules) is released when 22.0 g of ethanol vapor at 97.5 ∘C...
How much energy (in kilojoules) is released when 22.0 g of ethanol vapor at 97.5 ∘C is cooled to -12.5 ∘C? Ethanol has mp = -114.5 ∘C, bp = 78.4 ∘C, ΔHvap = 38.56 kJ/mol and ΔHfusion = 4.60 kJ/mol. The molar heat capacity is 113 J/(K⋅mol) for the liquid and 65.7 J/(K⋅mol) for the vapor.
How much heat energy is required to convert 32.1 g of solid iron at 26 °C...
How much heat energy is required to convert 32.1 g of solid iron at 26 °C to liquid iron at 1538 °C? The molar heat of fusion of iron is 13.8 kJ/mol. Iron has a normal melting point of 1538 °C. The specific heat capacity of solid iron is 0.449 J/g·°C.
How much energy (in kilojoules) is released when 29.0 g of ethanol vapor at 88.0 ∘C...
How much energy (in kilojoules) is released when 29.0 g of ethanol vapor at 88.0 ∘C is cooled to -10.0 ∘C? Express your answer to two significant figures. q = ______________ kJ Ethanol has mp = -114.5 ∘C, bp = 78.4 ∘C, ΔHvap = 38.56 kJ/mol and ΔHfusion = 4.60 kJ/mol. The molar heat capacity is 113 J/(K⋅mol) for the liquid and 65.7 J/(K⋅mol) for the vapor.
What amount of thermal energy (in kJ) is required to convert 220 g of ice at...
What amount of thermal energy (in kJ) is required to convert 220 g of ice at -18 °C completely to water vapour at 248 °C? The melting point of water is 0 °C and its normal boiling point is 100 °C. The heat of fusion of water is 6.02 kJ mol-1 The heat of vaporization of water at its normal boiling point is 40.7 kJ mol-1 The specific heat capacity of ice is 2.09 J g-1 °C-1 The specific heat...
What amount of thermal energy (in kJ) is required to convert 216 g of ice at...
What amount of thermal energy (in kJ) is required to convert 216 g of ice at -30 °C completely to water vapour at 198 °C? The melting point of water is 0 °C and its normal boiling point is 100 °C. The heat of fusion of water is 6.02 kJ mol-1 The heat of vaporization of water at its normal boiling point is 40.7 kJ mol-1 The specific heat capacity of ice is 2.09 J g-1 °C-1 The specific heat...
Ethanol (C2H5OH) melts at -114 ∘C and boils at 78 ∘C. The enthalpy of fusion of...
Ethanol (C2H5OH) melts at -114 ∘C and boils at 78 ∘C. The enthalpy of fusion of ethanol is 5.02 kJ/mol, and its enthalpy of vaporization is 38.56 kJ/mol. The specific heat of solid and liquid ethanol are 0.97 J/g⋅K are 2.3 J/g⋅Krespectively. A. How much heat is required to convert 40.5 g of ethanol at 36 ∘C to the vapor phase at 78 ∘C? B. How much heat is required to convert 40.5 g of ethanol at -161 ∘C to...
Ethanol (C2H5OH) melts at -114 ∘C and boils at 78 ∘C. The enthalpy of fusion of...
Ethanol (C2H5OH) melts at -114 ∘C and boils at 78 ∘C. The enthalpy of fusion of ethanol is 5.02 kJ/mol, and its enthalpy of vaporization is 38.56 kJ/mol. The specific heat of solid and liquid ethanol are 0.97 J/g⋅K are 2.3 J/g⋅K respectively. Q: A) How much heat is required to convert 36.5 g of ethanol at 35 ∘C to the vapor phase at 78 ∘C? B) How much heat is required to convert 36.5 g of ethanol at -167...
How much heat is required to convert 22.8 g of liquid benzene (C6H6) at 58 ∘C...
How much heat is required to convert 22.8 g of liquid benzene (C6H6) at 58 ∘C to gaseous benzene at 100 ∘C? The boiling point of benzene is 80.1 ∘C and Cm [C6H6(l)] = 136.0 J/(mol⋅∘C), and ΔHvap = 30.72 kJ/mol, Cm [C6H6(g)] = 82.4 J/(mol⋅∘C).
From the data below, calculate the total heat (in J) needed to convert 0.896 mol of...
From the data below, calculate the total heat (in J) needed to convert 0.896 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 ΔH0vap :40.5 kJ/mol cgas:1.43 J/g·°C cliquid:2.45 J/g·°C