Given:

Number Unit Mass of flask, stopper, and 5mL of water= 97.906 g

Mass of flask, stopper, and filled with water =233.658 g

Volume of gas space in flask (the difference between the above two measurements covnerted to mL) =0.13 L

Trial 1: Mg(s)+HCl (aq)

Mg + HCl reaction

Mass of Mg 0.008 g

Initial Pressure= 1.0387 atm

Maximum Pressure=1.0427 atm

Change in pressure= -0.0405 atm

Temperature of water bath=294.1 Kelvin

NaHCO3(s) + HCl(aq) reaction

Mass of NaHCO3=0.050 g

Mass of system before reaction =117.581

Mass of system after reaction=117.566

Mass Change= -0.015 g

Initial Pressure=1.0553 atm

Maximum Pressure=1.0028atm

Change in Pressure=0.0525 atm

Temperature of water bath=292.8 Kelvin

Q1. Based on the mass of Mg used, calculate the moles of H2(g) theoretically produced in trial 1.

Q2. The volume of hydrogen gas produced was not at standard temperature and pressure. Convert the volume at the pressure and temperature of the experiment to a volume at standard temperature and pressure: STP (T=273.15K and P= 1.00 atm) for trial 1.

Q3. Using your answers in #1 and #2, calculate the molar volume of H2 (g) (L.mol) at STP.

Q4. Calculate the % error of your calculated molar volume at STP with the accepted molar volume of an ideal gas at STP (22.4L/mol).

NaHCO3(aq)+HCL(aq)

Q5. From the P, V, and Tdata, calculate the actual moles of CO2 produced in each trial.

Q6. With your result from the pervious question and your data, calculate the molar mass of CO2 (g)

Q7. Calculate % error of your calculated molar mass of CO2.