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An unknown mass of aluminum is added to HCl solution. The aluminum metal is completely dissolved in the solution and generates hydrogen gas. See the balanced equation for the gas evolution reaction:
2 Al(s) + 6 HCl(aq) ---> 2 AlCl3(aq) + 3 H2(g)
The following data is collected:
Mass of Al sample: unknown g
Volume of gas collected 45.38 mL
Barometric pressure 754.8 mmHg
Temperature 23.5OC
Vapor pressure of H2O at 23.5OC 21.65 mmHg
Hydrogen gas is collected over water. The reaction proceeds until all the amount of aluminum is consumed in the gas-evolution reaction (aluminum is the limiting reactant).
(a) Calculate the mole number of the hydrogen gas generated in the reaction:
- Convert the volume of the collected gas to L: 45.38 mL = ___________ L
- Calculate the pressure exerted by H2 gas (= dry hydrogen gas):
Pressure of the dry hydrogen gas
= barometric pressure −vapor pressure of H2O(g)
= 754.8 mmHg − 21.65 mmHg
= _________ mmHg
- Determine the pressure of dry hydrogen gas in atm:
__________ mmHg = ___________ atm
- Convert the temperature to kelvin unit: 23.5OC = ________ K
Use theideal gas law to calculate the mole number of hydrogen gas collected: n=PVRT
mole number of hydrogen gas collected = _____________ mol
(b) Use stoichiometry to determine the mass of Al that reacted in this experiment.
mass of Al = ____________ g
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