One end of an open-ended manometer is connected to a canister of unknown gas. The atmospheric pressure is 1.03 atm. The mercury level is 18.6 mm higher in the U-Tube on the side open to the atmosphere than on the side attached to the canister. What is the pressure of gas in mm Hg?
1.03 atm = ??mm
??mm + 18.6 mm = ??
To determine the pressure of the gas in the canister, you need to calculate the pressure difference between the two ends of the manometer. Here's how you can approach the problem:
1. Start by converting the atmospheric pressure from atm to mm Hg. Since 1 atm is equivalent to 760 mm Hg, the atmospheric pressure is:
1.03 atm * 760 mm Hg/atm = 783.8 mm Hg
2. The mercury level on the side open to the atmosphere is 18.6 mm higher than the side connected to the canister. This means that the pressure of the gas in the canister must be lower than the atmospheric pressure.
3. Subtract the height difference (18.6 mm) from the atmospheric pressure (783.8 mm Hg):
783.8 mm Hg - 18.6 mm = 765.2 mm Hg
Therefore, the pressure of the gas in the canister, as measured by the manometer, is approximately 765.2 mm Hg.