Question

The reaction of metallic aluminum with aqueous hydrochloric acid produces hydrogen gas.

2Al(s)+6HCl(aq) → 2AlCl₃(aq)+3H₂(g)

Hydrogen gas produced by this reaction is typically collected via water displacement, during which time the hydrogen gas becomes saturated with water vapor. A 266.1mL sample of gas with a total pressure 149 kPa was collected via water displacement at 29.4℃. Calculate the partial pressure of hydrogen gas in the sample. The vapor pressure of water at 29.4℃ is 4.10 kPa.

Calculate the mass of aluminum that reacted to produce this quantity of hydrogen gas.

Answer 1

Augwer'- qalis) +6 HCl (29) 2AlCl3 (20) + 3Hala @ Pastral pressure of M2 ; PH2 = 149 kPa - 4 . 10 kPa = 144.9 kpa lansevel © Now I kPa = 0.00967atm 194-9 KPaz 0.00967 atm x 194-9 kpg TKPG PH₂ = 1.43 atm T= 302-4K (29.40 ) va 0.2661 L na PU ( from ideal gas equation) " H2 DT = 1.43 atm x 0.26612 0.0821 Latm mort Klx 302.4k 0.0153 mel MH2 = Now 3 moles of H₂ = 2 mol of Al -0.0153 me of the = 2 mel at AI XG-01S3 mo at the 0 3 moles of H2 = 0.0102 mol OLA) mar of Al = malex melar man pl 2 0.0102 mol x 27gmest = 0.276 g Cansever!