we use Pv=nRT. Everything here should be related to H2 (g) --> Chemical equation1Mg +2 HCl à MgCl2 +H2(g) From video : mass of Mg =.0407 g H2 gas volume = 38.2ml Temperature of room=24.0 +273=297k Total Pressure of the room = 30.01 in mmHg Calculations: find total pressure from barometer and convert it to mmHg, 1 in =2.54 cm and 25.4 mm 30.01 in mmHg x 25.4 mm Hg =762.3 mmHg total pressure of room 1in mmHg First step- convert g of Mg to mol of H2 0.0407g Mg x 1mol/24 gx 1molH2 = 0.00169mol 1mol Mg Second step: Total pressure of gas = Pressure of H2 + P of water 762.3 = p H2 + 22.4 FROM reference (canvas)=Pressure of water at 24 C= 22.4 mmHg n= 0.00169mol H2 Pressure of H2= 762.3-22.4= 739.854 x 1atm/760= 0.973 atm H2 Volume of H2= 38.2 ml /1000 =0.038L H2 Temp= 297K anwer this quesions with the information provide: Using PV=nRT, Find R=? (No R averge needed) à 0.973X0.0382=0.00169XRx 297 0.0372=0.50R Then, Percent error comparing your R from the experiment with theoretical value à 0.08206, and then find molar volume of this gas? to find molar volume at stp, put 1atm for pressure and for temp 273 K and n=1 in V=nRT,. then, find percent error of experiment molar volume from theoretical value of 22.4L P In general à Percent error =experimental value-theoretical value/theoretical valuex100
we use Pv=nRT. Everything here should be related to H2 (g) --> Chemical equation1Mg +2 HCl à MgCl2 +H2(g)
From video : mass of Mg =.0407 g
H2 gas volume = 38.2ml
Temperature of room=24.0 +273=297k
Total Pressure of the room = 30.01 in mmHg
Calculations: find total pressure from barometer and convert it to mmHg,
1 in =2.54 cm and 25.4 mm
30.01 in mmHg x 25.4 mm Hg =762.3 mmHg total pressure of room
1in mmHg
First step- convert g of Mg to mol of H2
0.0407g Mg x 1mol/24 gx 1molH2 = 0.00169mol
1mol Mg
Second step: Total pressure of gas = Pressure of H2 + P of water
762.3 = p H2 + 22.4 FROM reference (canvas)=Pressure of water at 24 C= 22.4 mmHg
n= 0.00169mol H2
Pressure of H2= 762.3-22.4= 739.854 x 1atm/760= 0.973 atm H2
Volume of H2= 38.2 ml /1000 =0.038L H2
Temp= 297K
anwer this quesions with the information provide:
Using PV=nRT, Find R=? (No R averge needed) à 0.973X0.0382=0.00169XRx 297 0.0372=0.50R
Then, Percent error comparing your R from the experiment with theoretical value à 0.08206, and then find molar volume of this gas? to find molar volume at stp, put 1atm for pressure and for temp 273 K and n=1 in V=nRT,. then, find percent error of experiment molar volume from theoretical value of 22.4L P
In general à Percent error =experimental value-theoretical value/theoretical valuex100
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