Question
In: Chemistry
Ethanol has a heat of vaporization of 38.56 kJ/mol and a normal boiling point of 78.4...
Ethanol has a heat of vaporization of 38.56 kJ/mol and a normal boiling point of 78.4 ∘C.
What is the vapor pressure of ethanol at 12 ∘C?
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
Ethanol has a heat of vaporization of 38.56kJ/mol and a normal boiling point of 78.4 ℃
Ethanol has a heat of vaporization of 38.56kJ/mol and a normal boiling point of 78.4 ℃ .
What is the vapor pressure of ethanol at 17 ℃?
Express your answer using two significant figures. Units in torr
Butane (C4H10) has a heat of vaporization of 22.44 kJ/mol and a normal boiling point of...
Butane (C4H10) has a heat of vaporization of 22.44 kJ/mol and a
normal boiling point of -0.4 ∘C. A 250 mL sealed flask contains
0.65 g of butane at −22∘C.
How much butane is present as a liquid at the boiling point?
If the butane is warmed to 25 ∘C, how much is present as a
liquid?
Butane (C4H10) has a heat of vaporization of 22.44 kJ/mol and a normal boiling point of...
Butane (C4H10) has a heat of vaporization of 22.44 kJ/mol and a
normal boiling point of -0.4 ∘C. A 250 mL sealed flask contains 0.6
g of butane at −22∘C. How much butane is present as a liquid at the
boiling point? If the butane is warmed to 25 ∘C, how much is
present as a liquid?
The standard enthalpy of vaporization of Freon-11, CFCl3, is 25.21 kJ/mol at its normal boiling point...
The standard enthalpy of vaporization of Freon-11, CFCl3, is
25.21 kJ/mol at its normal boiling point of 17°C. What is the
change of entropy for 1 mol of liquid Freon-11 when it vaporizes at
its normal boiling point?
For the process Cl2(g) → 2Cl(g), Question 18 options: ΔH is +
and ΔS is + for the reaction. ΔH is + and ΔS = 0 for the reaction.
ΔH is – and ΔS is – for the reaction. ΔH is –...
A) methanol has a normal boiling point of 64.6°C and a heat of vaporization H of...
A) methanol has a normal boiling point of 64.6°C and a heat of
vaporization H of 35.2 kJ/mol. What is the vapor pressure of
methanol at 12.0°C
B) How much energy in kJ is needed to heat 5.00 g of ice from
-10.0°C to 30.0°C? the heat of fusion of water is 6.02 kJ/mol, and
the molar heat capacity is 36.6 J/mol K for ice and 75.3 J/mol K
for liquid water
The normal boiling point of ethanol, C2H5OH, is 78.3 °C, and its molar enthalpy of vaporization...
The normal boiling point of ethanol, C2H5OH, is 78.3 °C, and its
molar enthalpy of vaporization is 38.56 kJ/mol. What is the change
in entropy in the system when 68.3 g of C2H5OH(g)2at 1 atm
condenses to liquid at the normal boiling point?
Ethanol boils at 73.30 degrees Celsius at atmospheric pressure. The heat of vaporization, ΔΗvapis 39.3 kJ/mol....
Ethanol boils at 73.30 degrees Celsius at atmospheric pressure.
The heat of vaporization, ΔΗvapis 39.3 kJ/mol. The
melting point at atmospheric pressure is -114.10 degrees Celsius.
The triple point is at pressure 0.00043 Pa and temperature -123.00
degrees Celsius. The density of liquid Ethanol at 25.0 degrees
Celsius is 0.783 gr/cm3.
What is the vapor pressure of liquid ethanol at 30.00 degrees
Celsius?
The heat of fusionΔΗmeltis 4.9 kJ/mol. Calculate the
change in volume brought about by a transition from...
Ethanol has a normal boiling point of 78.3 degrees celcius. Why is the normal boiling point...
Ethanol has a normal boiling point of 78.3 degrees celcius. Why
is the normal boiling point higher than methanol but lower than
iso-propanol (Normal boiling point = 82.3, heat of vaporization =
45.4)? Would you expect the heat of vaporization of ethanol to
follow the same trend? Explain.
AND
Calculate the heat of vaporixation of cyclohexane using the
normal boiling point of 80.7 degrees celcius. The vapor pressure of
cyclohexane at 25.0 degrees celcius is 0.132 atm.
Water has an unusually high specific heat, melting point, boiling point, and heat of vaporization as...
Water has an unusually high specific heat, melting point, boiling
point, and heat of vaporization as compared to compounds of similar
molar mass. Explain why.
Please show all work with the correct answer. Thank
you!!!!
Estimate the heat of vaporization of diethyl ether at its normal boiling point using Trouton’s rule...
Estimate the heat of vaporization of diethyl ether at its normal
boiling point using Trouton’s rule and Chen’s rule and compare the
results with a tabulated value of this quantity. Calculate the
percentage error that results from using each estimation. Then
estimate ΔH^v at 100°C using Watson’s correlation.
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