1.53 g of aluminum metal is placed in a Erlenmeyer flask with 1.5 M sulfuric acid. The hydrogen gas produced from the reaction is collected over water as seen in the diagram below.
The aluminum is allowed to react with the sulfuric acid until it stops reacting. There is still some unreacted aluminum left in the reaction flask. The gas in the collection flask is brought to the same atmospheric pressure as the surroundings, 765.25 torr and a temperature of 24.0 oC. The vapor pressure of water at 24.0 oC is 22.4 torr. The collected gas is found to have a volume of 350 mL.
Answer the following three questions based on this scenario.
What is the partial pressure of the hydrogen in the collection flask?
How many moles of hydrogen gas are contained in the collection flask?
What mass of aluminum reacted? (hint: You need to determine the balanced equation for the reaction to do this problem.)
? g Al
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1.53 g of aluminum metal is placed in a Erlenmeyer flask with 1.5 M sulfuric acid....
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