Question

How much energy must be removed from a 125 g sample of benzene (C6H6) vapor at...

How much energy must be removed from a 125 g sample of benzene (C6H6) vapor at 425.0 K to make it a solid at 200.0 K? Use the following steps to get to your answer. You MUST show your work to receive any credit. The following physical data for benzene may be useful. The quiz will be due at the beginning of class on 2/17/16. ΔHvap = 33.9 kJ/mol ΔHfus = 9.8 kJ/mol Cliq = 1.73 J/g°C Cgas = c Csol = 1.51 J/g°C Tmelting = 279.0 K Tboiling = 353.0 K

3) How much energy must be removed to convert the gas to a liquid?

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
How much energy must be removed from a 125 g sample of benzene (C6H6) at 425.0...
How much energy must be removed from a 125 g sample of benzene (C6H6) at 425.0 K to liquefy the sample and lower the temperature to 335.0 K? The following physical data may be useful. ΔHvap = 33.9 kJ/mol ΔHfus = 9.8 kJ/mol Cliq = 1.73 J/g°C Cgas = 1.06 J/g°C Csol = 1.51 J/g°C Tmelting = 279.0 K Tboiling = 353.0 K (The answer is 67.7 kJ. Please show how you get the answer)
How much energy must be removed from a 125 g sample of benzene (molar mass= 78.11...
How much energy must be removed from a 125 g sample of benzene (molar mass= 78.11 g/mol) at 425.0 K to liquefy the sample and lower the temperature to 335.0 K? The following physical data may be useful. ΔHvap = 33.9 kJ/mol Cliq = 1.73 J/g°C Tmelting = 279.0 K ΔHfus = 9.8 kJ/mol Cgas = 1.06 J/g°C Tboiling = 353.0 K Csol = 1.51 J/g°C
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).
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.
Using the provided data, calculate the amount of heat, in kJ, required to warm 15.3 g...
Using the provided data, calculate the amount of heat, in kJ, required to warm 15.3 g of solid benzene, initially at -9. °C, to gaseous benzene at 93. °C. benzene molar mass 78.1118 g/mol melting point 5. °C boiling point 80. °C ΔHfus 9.9 kJ/mol ΔHvap at bp 30.7 kJ/mol Cs, solid 1.51 J/g⋅°C Cs, liquid 1.73 J/g⋅°C Cs, gas 1.33 J/g⋅°C A.10.5 kJ B.82.8 kJ C.87.5 kJ D.35.7 kJ E.46.2 kJ Please help I know what to do if...
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.
1. What quantity of energy, in joules, must be removed from a 134-g sample of C2H4(g)...
1. What quantity of energy, in joules, must be removed from a 134-g sample of C2H4(g) that is initially at 22.29°C to its condensation point (-103.77°C) and then change the gas to a liquid at that temperature? _______________ J Useful Information: The molecular weight of  C2H4 is 28.052 g/mol. The boiling point of  C2H4 is -103.77°C. The heat capacity of C2H4(g) is 1.529 J/gK The heat of vaporization of C2H4 is 13.53 kJ/mol.
Calculate the amount of energy necessary to warm 10.0 g of ice from 0.0° C to...
Calculate the amount of energy necessary to warm 10.0 g of ice from 0.0° C to 137.0° C. Express your answer in kJ. Do not enter units of measurement, do not enter the answer in scientific notation. The specific heat is 4.184 J/g∙°C for water and 1.99 J/g∙°C for steam. ΔHvap is 40.79 kJ/mol and ΔHfus is 6.01 kJ/mol.
part A How much heat energy, in kilojoules, is required to convert 69.0 g of ice...
part A How much heat energy, in kilojoules, is required to convert 69.0 g of ice at −18.0 ∘C to water at  25.0 ∘C ? Part B How long would it take for 1.50 mol of water at 100.0 ∘C to be converted completely into steam if heat were added at a constant rate of 22.0 J/s ? Specific heat of ice: sice=2.09 J/(g⋅∘C) Specific heat of liquid water: swater=4.18 J/(g⋅∘C) Enthalpy of fusion (H2O(s)→H2O(l)): ΔHfus=334 J/g Enthalpy of vaporization (H2O(l)→H2O(g)):...
How much heat must be removed from 100 g of water at 25.0°C to change it...
How much heat must be removed from 100 g of water at 25.0°C to change it into ice at -10.0°C? The specific heat of ice is 2090 J/kg · K, and the specific heat of water is 4186 J/kg · K. For water LF = 334,000 J/kg and LV = 2.256 × 106 J/kg.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT