Question

Pure Benzene (C6H6) has a melting point of 5.5 degrees C. Delta Hof fusion for benzene...

Pure Benzene (C6H6) has a melting point of 5.5 degrees C. Delta Hof fusion for benzene is 9.87 kj/mol; specific heat for liquidbenzene is 1.63 J/g X degrees). A. Calculate the number of joules required to melt 57.4 g ofbenzene at 5.5 degrees C. B. Calculate the number of joules required to raise the temperatureof 57.4 g of liquid benzene from 5.5 degrees C. to 45.0 degreesC.

Homework Answers

Answer #1

mP of benzene = 5.5 c

DHfus of benzene = 9.87 kj/mol

specific heat for liquidbenzene = 1.63 J/g.c

A. heat required to melt = n*DHfus

              = (57.4/78)*9.87

              = 7.26 kj

B. heat required to heat = n*DHfus + mass of C6H6*Specific heat of C6H6*DT

      = (57.4/78)*9.87 + 57.4 *1.63*10^-3*(45-5.5)

   = 10.95 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
Using the following data, Compound Melting Point (C) delta H fusion (kJ/mol) Boiling Point (C) delta...
Using the following data, Compound Melting Point (C) delta H fusion (kJ/mol) Boiling Point (C) delta H vap (kJ/mol) HF -83.11 4.577 19.54 25.18 HCl -114.3 1.991 -84.9 17.53 HBr -86.96 2.406 -67.0 19.27 Hl -50.91 2.871 -35.38 21.16 calculate ?Sfus and ?Svap for HF. Determine the entropy change when 3.30 mol of HF(g) condenses at atmospheric pressure.
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).
) Pure benzene, C6H6, has a density of 0.8765 g/ml, a freezing point of 5.45oC and...
) Pure benzene, C6H6, has a density of 0.8765 g/ml, a freezing point of 5.45oC and a boiling point of 80.2oC. Its freezing point depression constant, Kf, is 5.07oC/m. A solution was made by taking 24.20 grams of an unknown non-electrolyte and dissolving it in 125.0 grams of benzene. The measured freezing point of the solution was -1.65oC. Calculate the molecular weight of the unknown substance. 258 g/mole 145 g/mole 138 g/mole 272 g/mole 595 g/mol
A substance has a melting point of 20°C and a heat of fusion of 2.6×104 J/kg....
A substance has a melting point of 20°C and a heat of fusion of 2.6×104 J/kg. The boiling point is 150°C and the heat of vaporization is 5.2×104 J/kg at a pressure of 1.0 atm. The specific heats for the solid, liquid, and gaseous phases are 600 J/(kg·K), 1000 J/(kg·K), and 400 J/(kg·K), respectively. The quantity of heat required to raise the temperature of 3.0 kg of the substance from 3°C to 118°C, at a pressure of 1.0 atm, is...
Question Part Submissions Used Mercury has the following physical properties: normal melting point = -39°C, normal...
Question Part Submissions Used Mercury has the following physical properties: normal melting point = -39°C, normal boiling point = 357°C, heat of fusion = 2.33 kJ/mol, heat of vaporization = 284 J/g, specific heat = 0.139 J/g·°C. Calculate ΔH for the conversion of 171 g of solid mercury at its freezing point to mercury vapor at its boiling point. Note that the heat of vaporization is in atypical units of J/g. To calculate that value, simply multiply so that units...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT