A gas mixture contains oxygen and argon at partial pressures of 0.60 atm and 425 mmhg. If nitrogen gas added to the sample increases the total pressure to 1250 torr, what is the partial pressure in torr?
To find the partial pressure of nitrogen gas, we need to utilize Dalton's Law of Partial Pressures, which states that the total pressure of a gas mixture is equal to the sum of the partial pressures of each individual gas.
In this case, we have oxygen, argon, and nitrogen gases. We are given the partial pressures of oxygen and argon, which are 0.60 atm and 425 mmHg, respectively. However, the total pressure is given in torr, so we need to convert the partial pressures of oxygen and argon to torr.
Converting 0.60 atm to torr:
1 atm = 760 torr
0.60 atm × 760 torr/atm = 456 torr
Converting 425 mmHg to torr:
1 mmHg = 1 torr
425 mmHg × 1 torr/mmHg = 425 torr
Now, let's use Dalton's Law of Partial Pressures to find the partial pressure of nitrogen gas:
Total pressure = Partial pressure of oxygen + Partial pressure of argon + Partial pressure of nitrogen
1250 torr = 456 torr + 425 torr + Partial pressure of nitrogen
To find the partial pressure of nitrogen, we can rearrange the equation:
Partial pressure of nitrogen = Total pressure - Partial pressure of oxygen - Partial pressure of argon
Partial pressure of nitrogen = 1250 torr - 456 torr - 425 torr
Partial pressure of nitrogen = 369 torr
Therefore, the partial pressure of nitrogen gas is 369 torr.
What's the partial pressure in torr OF WHAT? nitrogen?
PAr + PO2 + PN2 = total pressure
Solve for PN2.