The partial pressures of the gases in a mixture are 0.875 atm O2, 0.0553 atm N2, and 0.00652 atm Ar. What is the total pressure of the mixture?

A. 0.813 atm

B. 0.937 atm

C. 0.000315 atm

D. 0.875 atm

2.73 atm = P. B. P. = P. + P. = 2.73 atm + (745 torr *.) = 2.73 + 0.980 = 3.71 atm. 3. Helium is collected over water at 25°C and 1.00 atm total pressure ... 1 atm. 760 torr. = 3.12 L. 4. A. In a mixture of the two gases, the partial pressures of CH4 (g) and O2 (g) are 0.175 atm and 0.250 atm, respectively. What is the mole fraction

B. 0.937 atm

The total pressure of a gas mixture is simply the sum of the partial pressures of each gas within the mixture. So let's add them together: 0.875 atm + 0.0553 atm + 0.00652 atm = 0.93682 atm.

Since we only have 3 significant figures in our data, round the result to 3 figures, giving 0.937 atm, which exactly matches option "B" which is the correct answer.