1. The vapor pressure of liquid chloroform , CHCl 3 , is 100 . mm Hg at 283 K. A
ID: 477167 • Letter: 1
Question
1.
The vapor pressure of liquid chloroform, CHCl3, is 100. mm Hg at 283 K. A 0.384 g sample of liquidCHCl3 is placed in a closed, evacuated 400. mL container at a temperature of 283 K.
Assuming that the temperature remains constant, will all of the liquid evaporate? _____yes OR no
What will the pressure in the container be when equilibrium is reached? _______mm Hg
2.
The vapor pressure of liquid octane, C8H18, is 100. mm Hg at 339 K.
A sample of C8H18 is placed in a closed, evacuated 518 mL container at a temperature of 339 K. It is found that all of the C8H18 is in the vapor phase and that the pressure is 61.0 mm Hg. If the volume of the container is reduced to 373 mL at constant temperature, which of the following statements are correct?
Choose all that apply.
a. No condensation will occur.
b. Some of the vapor initially present will condense.
c. The pressure in the container will be 100. mm Hg.
d. Only octane vapor will be present.
e. Liquid octane will be present.
3.
The vapor pressure of liquid acetone, CH3COCH3, is 40.0 mm Hg at 264 K.
A sample of CH3COCH3 is placed in a closed, evacuated container of constant volume at a temperature of 402 K. It is found that all of the CH3COCH3 is in the vapor phase and that the pressure is 50.0 mm Hg. If the temperature in the container is reduced to 264 K, which of the following statements are correct?
Choose all that apply.
a. pressure in the container will be 40.0 mm Hg.
b. No condensation will occur.
c. Liquid acetone will be present.
d. Some of the vapor initially present will condense.
e. Only acetone vapor will be present.
Explanation / Answer
1.
The vapor pressure of liquid chloroform, CHCl3, is 100. mm Hg at 283 K. A 0.384 g sample of liquidCHCl3 is placed in a closed, evacuated 400. mL container at a temperature of 283 K.
Assuming that the temperature remains constant, will all of the liquid evaporate? _____yes OR no
What will the pressure in the container be when equilibrium is reached? _______mm Hg
Ideal gas equation is as follows:
PV= n RT
Here p = pressure,100 mmHg or 0.132 atm
V = volume 400 ml or 0.400 L, n= number of moles
R = gas constant, 0.08206 L atm K. -1 mol. -1.
and T = temperature, 283 K
Now calculate the moles of chloroform, CHCl3
n = PV/RT
= 0.132 atm * 0.400 L/ 0.08206 L atm K. -1 mol. -1 *283 K
= 2.27*10^-3 Moles
Molar mass of chloroform, CHCl3 = 119.38 g/mol
Amount of chloroform = number of moles * molar mass
= 2.27*10^-3 Moles *119.38 g/mol
= 0.271 g
Since this mass of chloroform is less than the total mass of chloroform thus there will not all the liquid evaporate.
Assuming that the temperature remains constant, will all of the liquid evaporate? __NO___yes OR no
What will the pressure in the container be when equilibrium is reached? ___100____mm Hg
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