Hydrogen gas produced by this reaction is typically collected via water displace
ID: 498014 • Letter: H
Question
Hydrogen gas produced by this reaction is typically collected via water displacement, during which time the hydrogen gas becomes saturated with water vapor. If 227.9 mL of gas with a total pressure 1.26 atm was collected via water displacement at 29.4 °C, what is the partial pressure of hydrogen gas in the sample?
Hydrogen gas can produced by the reaction between metallic aluminum and aqueous hydrochloric acid Hydrogen gas produced by this reaction is typically collected via water displacement, during which time the hydrogen gas becomes saturated with water vapor. 227.9 mL of with pressure 1.26 atm was via water displacement at 29.4 what is the partial pressure of hydrogen the sample? Number 30.8 atm How many grams of aluminum must have reacted to produce this quantity of hydrogen gas? The vapor pressure of water at 29.4 °C is 30.75 torr Number 5.08Explanation / Answer
Vapor pressure of water at 29.4 deg,c = 30.75 Torr = 0.04 atm, partial pressure of hydrogen = total pressure- saturation partial pressure = 1.26-0.04= 1.22 atm
V=227.9 ml =0.2279 L, P=1.22 atm, T=29.4deg.c= 29.4+273=302.4K, R= 0.0821 L.atm/mole.K
n= PV/RT = 1.22*0.2279/(0.0821*302.4)= 0.011 moles of Hydrogen
as per the reaction given, 3 moles of H2 requires 2 mole of Al
0.011 moles of H2 requires 0.011*2/3= 0.0073 moles, Mass of Aluminium= moles* atomic weight= 0.0073*27= 0.1971 gm
Related Questions
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.