A metal bulb is filled with 10.2 g of CHCl3 and 0.322 g of CH4 (two gases). What is the total pressure in the bulb if the temperature is 345◦C and the volume is 50.0 mL? 1. 0.107 atm 2. 192 atm 3. 107 atm 4. 1450 atm 5. 12,030 atm 6. There is no pressure because the metal bulb exerts more force than the gas does. 7. 12.1 atm

3. 107 atm

Explanation:

First, we will calculate the moles of each gas by dividing its mass by its molar mass.

nCHCl₃ = 10.2 g / (119.38 g/mol) = 0.0854 mol

nCH₄ = 0.322 g / (16.04 g/mol) = 0.0201 mol

The total number of moles is 0.0854 mol + 0.0201 mol = 0.1055 mol.

The absolute temperature is 345°C + 273.15 = 618 K

We can find the pressure of the gaseous mixture using the ideal gas equation.

P * V = n * R * T

P = n * R * T / V

P = 0.1055 mol * 0.08206 atm. L/mol. K * 618 K / 0.0500 L

P = 107 atm