Question

27.1 g of solid ethanol (MW = 46.07 g/mol) at -135.0 C (COLD!) is warmed up...

27.1 g of solid ethanol (MW = 46.07 g/mol) at -135.0 C (COLD!) is warmed up to room temperature (23.0 C). Here are some relevant physical data: Phase Cs (J/gC) Phase change temperature and enthalpy Gas 1.70 J/gC boiling pt: 78.4 C; Hvap: 38.6.7 kJ/mol Liquid 2.44 J/gC freezing pt: -114.1 C; Hfus: 4.9 kJ/mol Solid 2.42 J/gC a) What physical state will this sample of ethanol be at 23.0 C? _________________

b) Calculate the total energy (in kJ) required in the process described above.   

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
Ethanol, C2H5OH, (MW 46.06 g/mol) melts at -114 °C. The enthalpy of fusion is 5.02 kJ/mol....
Ethanol, C2H5OH, (MW 46.06 g/mol) melts at -114 °C. The enthalpy of fusion is 5.02 kJ/mol. The specific heats of solid and liquid ethanol are 0.97 J/g-K and 2.3 J/g-K, respectively. How much heat (kJ) is needed to convert 20.0 g of solid ethanol at -135 °C to liquid ethanol at -50 °C? please show work
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 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.
calculate the amount of heat (in kl) required to raise the temperature of 79 g sample...
calculate the amount of heat (in kl) required to raise the temperature of 79 g sample of ethanol from 298 k to 385 k. the specific heat capacity of ethanol 2.42 J/g C.the boiling point of ethanol and delta Hvap are given 78.4 C and 38.56 KJ/mol **16.6 IS WRONG SOULTION TO THIS QUESTION Please Help
A 0.66 g sample of ethanol (MW = 33.0 g/mol) is burned in a bomb calorimeter...
A 0.66 g sample of ethanol (MW = 33.0 g/mol) is burned in a bomb calorimeter that has a heat capacity of 4.31 kJ/oC. The temperature of the calorimeter increases by 6.35oC. Calculate the molar heat of combustion of ethanol using the data from this experiment. Since this experiment is carried out under conditions of constant volume, we are measuring ∆E. Your answer should be in kJ/mol and entered to 3 sig. fig. ΔE =
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⋅Krespectively. A) How much heat is required to convert 26.5 g of ethanol at 34 ∘C to the vapor phase at 78 ∘C? B) How much heat is required to convert 26.5 g of ethanol at -160 ∘C to...
When 1.020 g of ethanol (C2H6O, 46.07 g/mol) was burned in a bomb calorimeter containing 2400....
When 1.020 g of ethanol (C2H6O, 46.07 g/mol) was burned in a bomb calorimeter containing 2400. g of water, the temperature of the water rose from 22.46 to 25.52ºC.   The specific heat of water is 4.18 J/g-°C. What is the enthalpy of combustion of 1 mol of ethanol? What is the heat capacity of the calorimeter?
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...
A 12.30-g block of solid gold at 63.62 °C is immersed in a 23.29-g pool of...
A 12.30-g block of solid gold at 63.62 °C is immersed in a 23.29-g pool of liquid ethanol with a temperature of 12.25 °C. When thermal equilibrium is reached, what is the temperature of the gold and ethanol? Specific heat capacities: gold = 0.129 J/g °C; ethanol = 2.44 J/g °C ________°C
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT