Transcript Practicing the Ideal Gas Law - x10Hosting

PV = nRT
R = 0.0821 Latm/molK = 8.315 dm3kPa/molK
Ideal Gas Law & Gas Stoichiometry
1) Work out each problem on scratch paper.
2) Click ANSWER to check your answer.
3) Click NEXT to go on to the next problem.
EXIT
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QUESTION #1
How many grams of CO2 are
produced from 75 L of CO at 35°C
and 96.2 kPa?
2CO + O2  2CO2
ANSWER
EXIT
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ANSWER #1
Find the new molar volume:
n = 1 mol
V=?
P = 96.2 kPa
T = 35°C = 308 K
R = 8.315 dm3kPa/molK
V = 26.6 dm3/mol
BACK TO PROBLEM
EXIT
PV = nRT
CONTINUE...
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ANSWER #1 (con’t)
3
2CO
4
75 L
+ O2

2CO2
?g
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75 L
CO
1 mol
CO
2 mol
CO2
44.01
g CO2
26.6 L 2 mol
CO
CO
1 mol
CO2
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EXIT
= 120 g
CO2
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QUESTION #2
How many moles of oxygen will
occupy a volume of 2.5 L at 1.2
atm and 25°C?
ANSWER
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ANSWER #2
n=?
V = 2.5 L
P = 1.2 atm
T = 25°C = 298 K
R = 0.0821 Latm/molK
PV = nRT
n = 0.12 mol
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QUESTION #3
What volume will 56.0 grams of
nitrogen (N2) occupy at 96.0 kPa
and 21°C?
ANSWER
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ANSWER #3
V=?
n = 56.0 g = 2.00 mol
P = 96.0 kPa
T = 21°C = 294 K
R = 8.315 dm3kPa/molK
PV = nRT
V = 50.9 dm3
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QUESTION #4
What volume of NH3 at STP is
produced if 25.0 g of N2 is reacted
with excess H2?
N2 + 3H2  2NH3
ANSWER
EXIT
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ANSWER #4
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N2
4
25.0 g
+ 3H2

NH3
?L
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25.0 g
N2
1 mol
N2
2 mol
NH3
22.4 L
NH3
28.02 g 1 mol
N2
N2
1 mol
NH3
BACK TO PROBLEM
EXIT
= 40.0 L
NH3
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QUESTION #5
What volume of hydrogen is
produced from 25.0 g of water at
27°C and 1.16 atm?
2H2O  2H2 + O2
ANSWER
EXIT
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ANSWER #5
Find the new molar volume:
n = 1 mol
V=?
P = 1.16 atm
T = 27°C = 300. K
R = 0.0821 Latm/molK
BACK TO PROBLEM
EXIT
PV = nRT
V = 21.2 L/mol
CONTINUE...
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ANSWER #5 (con’t)
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2H2O
4

25.0 g
2H2 + O2
?L
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25.0 g
H2O
1 mol
H2O
2 mol
H2
21.2 L
H2
18.02 g 2 mol
H2O
H2O
1 mol
H2
BACK TO PROBLEM
EXIT
= 29.4
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L
H2
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QUESTION #6
How many atmospheres of pressure
will be exerted by 25 g of CO2 at
25°C and 0.500 L?
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ANSWER
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ANSWER #6
P=?
n = 25 g = 0.57 mol
T = 25°C = 298 K
V = 0.500 L
R = 0.0821 Latm/molK
PV = nRT
P = 28 atm
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QUESTION #7
How many grams of CaCO3 are
required to produce 45.0 dm3 of CO2
at 25°C and 2.3 atm?
CaCO3 + 2HCl  CO2 + H2O + CaCl2
ANSWER
EXIT
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ANSWER #7
Find the new molar volume:
n = 1 mol
V=?
P = 2.3 atm
T = 25°C = 298 K
R = 0.0821 Latm/molK
BACK TO PROBLEM
EXIT
PV = nRT
V = 11 L/mol
CONTINUE...
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ANSWER #7
CaCO3 + 2HCl  CO2 + H2O + CaCl2
?g
45.0 dm3
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45.0dm3
CO2
1 mol 1 mol 100.09 g
CO2 CaCO3 CaCO3
11 dm3 1 mol 1 mol
CO2
CO2 CaCO3
BACK TO PROBLEM
EXIT
= 410 g
CaCO3
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QUESTION #8
Find the number of grams of CO2 that
exert a pressure of 785 torr at 32.5 L
and 32°C.
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ANSWER
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ANSWER #8
n=?
P = 785 torr = 1.03 atm
V = 32.5 L
T = 32°C = 305 K
R = 0.0821 Latm/molK
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BACK TO PROBLEM
EXIT
PV = nRT
n = 1.34 mol

59.0 g CO2
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