a. Calculate the moles of H2 produced from each trial b. Vol of gas was not at s
ID: 1065662 • Letter: A
Question
a. Calculate the moles of H2 produced from each trial
b. Vol of gas was not at standard temp and pressure. Convert the volume at the pressure and temperature of the experiment to a volume at standard temperature and pressure. (STP = 273. 15K, P = 1.00atm)
c. Using your answers from part a and b, calculate the molar volume of H2(g) (L/mol) at STP for each trial.
(For what ever reason, I am only able to put in a good value for mols of H2 into the computer, it keeps saying my calculations are incorrect for the rest. Trying to figure out what I am doing wrong)
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 above two measurements covnerted to mL) (L) .135444 LExplanation / Answer
Mg(s) + HCl(aq) Reaction
2Mg + 2HCl = MgCl2 + H2
PV= n RT
Here P = 0.0471atm
V= 0.135444 L
T= 295.7 K
n = PV/ RT
= 0.0006*0.135444 /0.08206* 295.7
= 3.35*10^-6 Moles
Trail 2:
2Mg + 2HCl = MgCl2 + H2
PV= n RT
Here P = 0.0471atm
V= 0.135444 L
T= 296.1K
n = PV/ RT
= 0.0471*0.135444 /0.08206* 296.1
= 2.63*10^-4Moles
Vol of gas was not at standard temp and pressure. Convert the volume at the pressure and temperature of the experiment to a volume at standard temperature and pressure. (STP = 273. 15K, P = 1.00atm)
mole of any gas at STP occupies 22.4 liters of volume
thus, 3.35*10^-6 Moles will occupies = 22.4 L / 1 mol* 3.35*10^-6 Moles
= 7.504*10^-5L
Now calculate the molar volume
Volume ; 7.504*10^-5L / number of mole s
= 22.4 L / mole
And 2.63*10^-4 Moles will occupies = 22.4 L / 1 mol* 2.63*10^-4 Moles
= 5.89*10^-3 L
Now calculate the molar volume
Volume ; 5.89*10^-3 L / number of mole s2.63*10^-4
= 22.4 L / mole
Mg(s) + HCl(aq) Reaction
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