34.9 grams of hydrogen gas and 17.7 grams of methane gas are combined in a reaction vessel with a total pressure at 2.92 atm.What is the partial pressure (atm)of hydrogen gas?

Question

Quizplus · Accepted Answer

To determine the partial pressure of hydrogen gas, we need to use the mole fraction of hydrogen gas in the mixture.

First, we need to determine the number of moles of each gas present:

n(H2) = 34.9 g / 2.016 g/mol = 17.3 mol
n(CH4) = 17.7 g / 16.04 g/mol = 1.10 mol

Next, we need to calculate the total number of moles in the mixture:

n(total) = n(H2) + n(CH4) = 18.4 mol

Now we can calculate the mole fraction of hydrogen gas:

X(H2) = n(H2) / n(total) = 17.3 mol / 18.4 mol = 0.940

Finally, we can use the mole fraction to determine the partial pressure of hydrogen gas:

P(H2) = X(H2) * P(total) = 0.940 * 2.92 atm = 2.75 atm

Therefore, the answer is D) 2.75.

349 Grams of Hydrogen Gas and 17