The hydrogen gas formed in a chemical reaction is collected over water at 30 deg
ID: 904491 • Letter: T
Question
The hydrogen gas formed in a chemical reaction is collected over water at 30 degrees Celsius at a total pressure of 732 mmHg. What is the partial pressure of the Hydrogen gas collected in this way? If the total volume of gas collected is 722mL, what mass of hydrogen gas is collected? The hydrogen gas formed in a chemical reaction is collected over water at 30 degrees Celsius at a total pressure of 732 mmHg. What is the partial pressure of the Hydrogen gas collected in this way? If the total volume of gas collected is 722mL, what mass of hydrogen gas is collected?Explanation / Answer
vapor pressure of water at 30 deg.c =31.7 mm Hg
Total pressure =saturation pressure of water+ partial pressure of hydrogen
732= 31.7 + partial pressure of pressure of hydrogen
Partial pressure of hydrogen =732-31.7 =700.3 mm Hg
From PV= nRT
P =700.3 =700.3/760 atm =0.921447 atm
V= 722 m; =722/1000 L =0.722 L
R= 0.08206 atm.L/gmole.K
T= 30+273.15= 303.15 K
n= mass/molecularr weigght= M/2 Where (M =Molecular weight)
n= PV/RT = M/2 = 0.921447*0.722/(0.08206*303.15) = 0.026744
M =0.026744*2=0.053487 gm
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