A sample of hydrogen gas (3.2 L)at 3.5 atm and 25 °C was combined with 5.2 L of nitrogen gas at 7.3 atm and 25 °C at constant temperature in a 15.0 L flask.Assuming the initial pressure in the flask was 0.00 atm and the temperature upon mixing was 25 °C,what is the total pressure (atm)in the flask?
A)3.28
B)5.85
C)9.45
D)15.4
E)10.8

Question

Quizplus · Accepted Answer

The total pressure in the flask is the sum of the partial pressures of hydrogen and nitrogen. The partial pressure of hydrogen is 3.2 L * 3.5 atm / 15.0 L = 0.76 atm. The partial pressure of nitrogen is 5.2 L * 7.3 atm / 15.0 L = 2.52 atm. The total pressure is 0.76 atm + 2.52 atm = 3.28 atm.

A Sample of Hydrogen Gas (3