Question

12. A container holds 0.52 moles of chlorine gas, 0.38 moles of hydrogen gas, and 0.47 moles

of argon gas. If the total pressure of the gases is 5.8 atm, what is the partial pressure of each
gas?

Answer 1

The partial pressures of chlorine gas, hydrogen gas, and argon gas in the container are 2.16 atm, 1.60 atm, and 1.96 atm respectively.

Step-by-step explanation:

The partial pressure of a gas in a mixture is proportional to the number of moles of that gas present. So, the partial pressure of chlorine gas (PC) can be calculated as:

PC = (0.52 moles of chlorine / (0.52 + 0.38 + 0.47)) * 5.8 atm = 0.52 * 5.8 / 1.37 = 2.16 atm

Similarly, the partial pressure of hydrogen gas (PH) can be calculated as:

PH = (0.38 moles of hydrogen / (0.52 + 0.38 + 0.47)) * 5.8 atm = 0.38 * 5.8 / 1.37 = 1.60 atm

And the partial pressure of argon gas (PA) can be calculated as:

PA = (0.47 moles of argon / (0.52 + 0.38 + 0.47)) * 5.8 atm = 0.47 * 5.8 / 1.37 = 1.96 atm

So, the partial pressures of chlorine gas, hydrogen gas, and argon gas in the container are 2.16 atm, 1.60 atm, and 1.96 atm respectively.