This 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 32.26 miligrams of aluminum are treated with excess hydrochloric acid?
The atmospheric pressure was measured to be 0.9247 atm and the room temperature was 19.00oC. At this temperature, the vapor pressure of water is 16.50 torr. What would be the volume of the number of moles of hydrogen just calculated under these conditions? in 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?
Suppose that you have completed this week's experiment and have determined that the molar mass of aluminum is 22.35 g mol-1. What is the percent error of your experimental result?