| Mass of flask, stopper, and 5mL of water (g) | 102.945 | g |
| Mass of flask, stopper, and filled with water (g) | 238.389 | g |
| Volume of gas space in flask (the difference between the abovetwo measurements covnerted to mL) (L) | .135444 | L |
Mg(s) + HCl(aq) Reaction | Trail 1 | Trial 2 |
| Mass of Mg(g) | 0.008 | 0.007 |
| Initial Pressure (atm) | 0.9974 | 0.9945 |
| Max Pressure (atm) | 0.9980 | 0.007 |
| Pressure Change (atm) | 0.0006 | 0.0471 |
| Temp (K) | 295.7 | 296.1 |
a. Calculate the moles of H2 produced from each trial
b. Vol of gas was not at standard temp and pressure. Convert thevolume at the pressure and temperature of the experiment to avolume at standard temperature and pressure. (STP = 273. 15K, P =1.00atm)
c. Using your answers from part a and b, calculate the molarvolume of H2(g) (L/mol) at STP for each trial.
(For what ever reason, I am only able to put in a goodvalue for mols of H2 into the computer, it keeps saying mycalculations are incorrect for the rest. Trying to figure out whatI am doing wrong)
