Question

The diagram below shows a gas sample being measured with an open-end mercury (Hg) manometer. If a barometer reads 730. 1 torr, what is the pressure of the gas in the flask (in atm) when Δh = 5.89 cm? (NOTE: 1 cm = 10 mm; 760 mmHg = 760 torr = 1 atm)

Answer 1

The pressure of the gas in the flask (in atm) when Δh = 5.89 cm is 1.04 atm

Data obtained from the question

The following data were obtained from the question:

• Atmospheric pressure (Pa) = 730.1 torr = 730.1 mmHg
• Change in height (Δh) = 5.89 cm
• Pressure due to Δh (PΔh) = 5.89 cmHg = 5.89 × 10 = 58.9 mmHg
• Pressure of gas (P) =?

How to determine the pressure of the gas

The pressure of the gas can be obtained as illustrated below:

P = Pa + PΔh

P = 730.1 + 58.9

P = 789 mmHg

Divide by 760 to express in atm

P = 789 / 760

P = 1.04 atm

Thus, the pressure of the gas when Δh = 5.89 cm is 1.04 atm

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