Question

A. DATA 170 Trial 1 1. Mass of magnesium. 2. Calibration of gas measuring tube 3. Volume of gas in tube (mL) 4. Barometric pressure (torr) TITLULUUUUUUUUUU 0878 8704 2 anh 88.2m6 67.0me 710. Bruly 770.13 multy 14 Leden 135mm 2oc zdce 198 tot 22c 220 5. Height of water in the gas measuring tube above the water in the beaker (mm) 6. Room temperature (°C) 7. Temperature of water 8. Water vapor pressure at the temperature of the water (torr) 19.8 toll 19.6 tord Postal B. CALCULATIONS Pwater 770 13-19.6% - 8o33 1. Calculate the pressure of the water column in the tube as a mercury equivalent (torr) untuITITI 2. Calculate the pressure of dry hydrogen (torr)

confused about the wording on the first two calculations and what to look for.

Answer 1

1)

Pressure of water column = 144 mm = 0.144 m

h = 0.144 m, g = 10 m/s² and density of water (d)= 1000kg/m³

Pressure of water column = h x d x g

= (0.144 m × 1000 × 10) Pa

= 1440 Pa

= 10.8 torr

Answer: 10.8 torr

2)

Hi you are correct, according to Dalton's law of partial pressure

P_total = P_gas + P_water

P_gas = P_total - P_water since 1 mmHg = 1 torr; 770.13 mmHg = 770.13 torr

P_gas = 770.13 torr - 19.8 torr = 750.33 torr which is equal to 750.33 mmHg

Answer: Pressure of dry hydrogen gas = 750.33 torr

Hope this helped you!

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