The vapor pressure of liquid chloroform, CHCl3, is 100. mm Hg at 283 K. A 0.380 g sample of liquid CHCl3 is placed in a closed, evacuated 380. mL container at a temperature of 283 K. Assuming that the temperature remains constant, will all of the liquid evaporate? yes/no
What will the pressure in the container be when equilibrium is reached? mm Hg

a

No

b

100 mm Hg

Explanation:

From the question we are told that

The vapor pressure of CHCl3, is

The temperature of CHCl3 is

The volume of the container is

The temperature of the container is

The mass of CHCl3 is m = 0.380 g

Generally the number of moles of CHCl3 present before evaporation started is mathematically represented as

Here M is the molar mass of CHCl3 with the value

=>

=>

Generally the number of moles of CHCl3 gas that evaporated is mathematically represented as

Here R is the gas constant with value

So

Given that the number of moles of  CHCl3 evaporated is less than the number of moles of CHCl3  initially present , then it mean s that not all the liquid evaporated

At equilibrium the temperature of CHCl3 will be equal to the pressure of  air so the pressure at equilibrium is  100 mmHg

altitude, density, pressure

air gets less dense the higher the altitude and also the air pressure is less as altitude rises.