A typical air sample in the lings contains oxygen at 100 mm Hg, nitrogen at 573 mm Hg, carbon dioxide at 40mm Hg and water at 47 mm Hg. What is the total pressure on the sample in mm Hg?

Dalton's law: total pressure is the sum of the partial pressures.

So do I have to do any conversions, say to moles or just take the sum of the values as is since the answer has to be in mm Hg?

To find the total pressure on the air sample, we need to sum up the partial pressures of all the gases present.

Given the partial pressures of oxygen, nitrogen, carbon dioxide, and water, we can find the total pressure by adding them together.

1. Start by adding the partial pressures of all the gases:
Total pressure = Partial pressure of oxygen + Partial pressure of nitrogen + Partial pressure of carbon dioxide + Partial pressure of water

2. Substitute the given values:
Total pressure = 100 mm Hg + 573 mm Hg + 40 mm Hg + 47 mm Hg

3. Calculate the sum:
Total pressure = 760 mm Hg

Therefore, the total pressure on the air sample is 760 mm Hg.