Reference no: EM13196872
This week's experiment involves the determination of the molar mass of aluminum by measuring the amount of hydrogen gas liberated when a sample of aluminum is treated with excess hydrochloric acid.
In the reaction between aluminum and hydrochloric acid, how many moles of hydrogen gas would be liberated when 3.498E-2 grams of aluminum are treated with excess hydrochloric acid?
Moles of hydrogen gas liberated = mol
The atmospheric pressure was measured to be 0.9667 atm and the room temperature was 20.00oC. At this temperature, the vapor pressure of water is 17.50 torr. What would be the volume of the number of moles of hydrogen just calculated under these conditions? Enter the answer in mL.
Volume of hydrogen gas = mL
The syringe used in this experiment is calibrated to 60 mL. However, there is a 'dead volume' at the needle end of the syringe that is uncalibrated. This volume equals 1.20 mL. Bearing in mind that the syringe is upside down, what would the reading on the syringe be that corresponded to the volume you have just calculated?
Reading on the syringe = mL
Suppose that you have completed this week's experiment and have determined that the molar mass of aluminum is 22.33 g mol-1. What is the percent error of your experimental result?
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