What is the vapor pressure of a 34.6 g sample of ethanol
(C2H5OH) in 120.0 mL...
What is the vapor pressure of a 34.6 g sample of ethanol
(C2H5OH) in 120.0 mL of water if the vapor pressure of water is
24.4 mmHg and the density is 0.9945 g/mL?
Problem 11.93
The vapor pressure of ethanol (C2H5OH) at 19 ∘C is 40.0 torr . A
0.800 g sample of ethanol is placed in a 2.80 L container at 19 ∘C
.
Part A
If the container is closed and the ethanol is allowed to reach
equilibrium with its vapor, how many grams of liquid ethanol
remain?
Express your answer to two significant figures and include the
appropriate units.
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The vapor pressure of ethonal (C2H5OH) is 672torr at
75°C. The vapor pressure of water is 289torr at the same
temperature.
Ethonal and water forms solution that behave like ideal solution.
Calc vapor pressure of ethonal and water above the solution at
75°C.
The
density of an aqueous solution containing 15.0% ethanol (C2H5OH) by
mass is 0.974 g/mL.
A) calculate the molality of this solution. B) calculate the
solutions molarity.
C) what volume of the solution would contain 0.108 mole of
ethanol?
A 21.8 g sample of ethanol
(C2H5OH, 46.07 g/mol) is burned in a bomb
calorimeter, according to the following reaction equation. If the
temperature of the rises from 13.0 °C to 79.3 °C, what is the heat
capacity of the calorimeter?
C2H5OH(l) + 3
O2(g) →2 CO2(g) + 3
H2O(g)
ΔH°rxn = –1235 kJ
The vapor pressure of ethanol (CH3CH2OH) at 20c is 44 mm Hg, and
the vapor pressure of Methanol (CH3OH) at the same temperature is
94 mm Hg. A mixture of 30.0 g of Methanol and 45.0 g ethanol is
prepared and can be assumed to behave ideally. Anwser the following
questions concerning this mixture.
A) Which component is more volatile?
A2) Determine the mole fraction of both components of the liquid
mixture?
B) Calculate the vapor pressure of methanol and...
At
35.0degrees, the vapour pressure of pure ethanol (C2H5OH) is
100.0mmHg and the vapour pressure of pure acetone (CH3COCH3) is
360.0 mmHg
a) a solution is formed from 25.0g of ethanol and 15.0g of
acetone. Assume ideal behaviour and calculate the vapour pressure
of each component above this solution.
b) calculate the mole fraction of acetone in the vapour
pressure in equilibrium with the solution in part a).
c) Name a method that can be used to separate these two...
The vapor pressure of ethanol is 1.00 × 102 mmHg at 34.90°C.
What is its vapor pressure at 50.66°C? (ΔHvap for ethanol is 39.3
kJ/mol.)
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A vapor composed of 0.65 mole fraction ethanol and 0.35 mole
fraction acetic acid at 120.0 mmHg (absolute), is in equilibrium
with a liquid phase also composed of ethanol and acetic acid.
Assume that the liquid is an ideal solution and apply Raoult's law
to find the following.
What is the temperature of the liquid____oC?
What are the mole fractions of the liquid pahse?
XE=___mol ethanol/mol
XA=___ mol acetic acid/mol
What is the vapor pressure of an ideal solution of ethanol if 1
mile of glycerin is placed in 4 moles of ethanol at 40?C? Pure
ethanol has a vapor pressure of 135.3 torr.
The equilibrium vapor pressure of ethanol at 298.15 K is 0.078
atm. Will ethanol gas at 0.05 atm and 298.15 K spontaneously
condense to liquid ehtanol? First answer this by thinking about it
qualitatively. Then support it with a calculation. Use the change
in entropy of the system and calculate the change in entropy of the
surroundings, and the change in entropy of the universe for the
condensation of one mole of ethanol gas at 0.05 atm and 298.15 K...