The vapor pressure of liquid iodomethane, CH3I, is 100. mm Hg at 266 K. A 0.453 g sample of liquid CH3I is placed in a closed, evacuated 370. mL container at a temperature of 266 K.a.Assuming that the temperature remains constant, will all of the liquid evaporate? _(yes/no)b.What will the pressure in the container be when equilibrium is reached? ____ mm Hg

The vapor pressure is the pressure of the vapor that is in equilibrium with the liquid. At a constant temperature, some molecules of the liquid will vaporize, and then will do pressure at the surface of the liquid.

If the pressure at the container is higher then the vapor pressure, the liquid will evaporate.

a. Let's calculate the pressure at the container by the ideal gas law:

PV = nRT

Where P is the pressure, V is the volume, n is the number of moles, R is the gas constant (62,364 mmHg.mL/mol.K), and T is the temperature.

The molar mass of CH₃I is 142 g/mol

n = mass/ molar mass

n = 0.453/142

n = 0.0032 mol

P*370 = 0.0032*62,364*266

370P = 53,084.24

P = 143.5 mmHg

So, all the liquid will evaporate.

b. Because all liquid evaporates, when the equilibrium is reached, the pressure is the gas pressure: 143.5 mmHg.