Hydrogen gas can have produced by the reaction between metallic aluminum and aqu

Question

Hydrogen gas can have 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. If 224 9 mL of gas with a total pressure 1.09 atm was collected via water displacement at 29.4 degree C, what is the partial pressure of hydrogen gas in the sample? How many grams of aluminum must have reacted to produce this quantity of hydrogen gas? The vapor pressure of water at 29.4 degree C is 30.75 torr.

Explanation / Answer

For the given reaction,

Partial pressure of hydrogen = 1.09 - 0.04 = 1.05 atm

moles of H2 = PV/RT = (1.09 - 0.04) x 0.2249/0.08205 x (273 + 29.4) = 0.0095 mols

mass of Al reacted = 0.0095 x 2 x 27/3 = 0.171 g

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