Answer :
Using Dalton's Law of Partial Pressures, the partial pressure of hydrogen gas and helium gas in a container holding 2.00 moles each, with a total pressure of 4.00 atm, would be 2.00 atm for each gas.
If a container holds 2.00 moles of hydrogen gas and 2.00 moles of helium gas, and the total pressure is 4.00 atm, the partial pressure of each of the gases can be determined using Dalton's Law of Partial Pressures. This law states that in a mixture of non-reacting gases, the total pressure exerted is equal to the sum of the partial pressures of individual gases. Since there are equal moles of hydrogen and helium, their partial pressures will be equal under the same conditions.
Therefore, the partial pressure of hydrogen gas (PH2) and the partial pressure of helium gas (PHe) can be calculated as follows:
Ptotal = PH2 + PHe
Ptotal = 4.00 atm = PH2 + PH2 (because the moles are equal, the pressures will be the same)
Hence, PH2 = PHe
= 4.00 atm / 2
= 2.00 atm for each gas.
