Question

Hydrogen gas bubbled through water is collected into an inverted tube at a temperature of 21.0 °C. The pressure of the collected mixed gas is adjusted to atmospheric pressure which is measured as 755 torr. What is the partial pressure, in mmHg, of the hydrogen gas in the mixture? Use partial pressure of water table below. How many grams of hydrogen are contained in the inverted tube if the volume of the mixed gas is 34.5 ml? Partial Pressure of Water Vapor Related to Temp: Temperature (°C) Przo vapor (mmHg) 18.0 15.477 19.0 16.477 20.0 17.535 18.650 22.0 19.827

Answer 1

6 Total pressure of mixed Gas = 755 toor = 755 mm Hg At 21°c (h2 gas + H20 vapour) partial pressure of H₂O at 21°C = 18.650 mm Hg Partial pressure of tho + Partial pressure of H2= 755 mmily Partial pressure of Hz Gas = 755 mmily - 18.650mming Partial pressure of He Ceas = 736 35 mm Hg = 0.96888 a ton. asm Volume of a = 34.5 mL & Pressure of H2=0-96888 Temperature -21°c= 294k ana mole of Ha-Gas Using Ideal Gas Equation - [PV=nes where - R= Universal Ceas Lonstre (0096888 afm) (34.54) = n x 0.082057 akmal x 292 K molk n = 0.96888 X 345 .. mol 0.082057 x 294 X1000 1000 → n = 0.00138 mole. Moles of Hydrogen Gas = 0·00138 mole.

3 Мая б, к, ih o-ool 39 wee Mass= molar mass x Mole Mass= 2.015889/mol X 0.0013.8m) Mass of H2 = -0.00 278 g Ang Dalton's Gas law was used to correctly determine the partial pressure of Hydrogen in the sample 6 Ideal gas law was used to correctly determine the number of moles of fly drogen in the sample. 6.2.01588 g/mol was used to determine the mass in grams of Hydrogen in the sample.