Ideal Gas Law Practice Worksheet Solve the following problems using the ideal gas law: 1) How many moles of gas does it take to occupy 120 liters at a pressure of

2.3 atmospheres and a temperature of 340 K? 2) If I have a 50 liter container that holds 45 moles of gas at a temperature of

200° C, what is the pressure inside the container? 3) It is not safe to put aerosol canisters in a campfire, because the pressure

inside the canisters gets very high and they can explode. If I have a 1.0 liter canister that holds 2 moles of gas, and the campfire temperature is 1400° C, what is the pressure inside the canister?

4) How many moles of gas are in a 30 liter scuba canister if the temperature

of the canister is 300 K and the pressure is 200 atmospheres? 5) I have a balloon that can hold 100 liters of air. If I blow up this balloon with

3 moles of oxygen gas at a pressure of 1 atmosphere, what is the temperature of the balloon?

12=8.21×10-2

pV= n RT

2 2

N=Ppf

,

=2-3 Atm ( 120L )

= 9.88751 - . MOI

8. 21 x 10-2 Latm ( 340k ) =

9.9MOI

3 K .MOI 2

5IS 't 3

P= 171¥ =45 mot ( 8.21×10-2 L - Atmlk - MOI ) ( 200+273 .

15k )It 50L

= 34.9610 - . - Atm = 30 Atm

1 3 5

P= nR =

2mm ( 8.21×10-2 L - atmlk - MOI ) ( 1400+273 .15k )

1. OL2

= 27473 .. - Atm = 300 Atm ISF

ISF I

n=p¥

,

=200 Atm ( 30L )

= 243.60 - - - mot

( 8.21×10-2 L - atmlk - MOI ) 300K

3 I= 200 mo )

ISF

ISF I

T= PV=

latin ( 100L )-

= 406.00 - - - KMR 3 moi ( 8.21×10-2 L - atmlk - MOI )

I 3=

400K

ISF

Solutions to the Ideal gas law practice worksheet: The ideal gas law states that PV = nRT, where P is the pressure of a gas, V is the volume of the gas, n is the number of moles of gas present, R is the ideal gas constant, and T is the temperature of the gas in Kelvins. Common mistakes: • Students express T in degrees celsius, rather than Kelvins. This can cause

huge problems, especially when the temperature is below freezing. • Students use the wrong value of R. You need to make sure that you have the

right value of R for the units you’re using. In this worksheet, R = 0.08206 L.atm/mol.K – some people prefer using units of KPa rather than atmospheres, resulting in huge errors if the wrong R is used.

1) 9.89 moles

2) 34.9 atm

3) 274.5 atm

4) 243.7 moles

5) 406.2 K (133.2° C – a very hot day to blow up balloons!)

Name _____________________________ Date ____________ Per ________ Gas Law Stoichiometry Worksheet

1) For the reaction 2 H2(g) + O2(g) ! 2 H2O(g), how many liters of water can be made from 5 L

of oxygen gas and an excess of hydrogen at STP?

2) How many liters of water can be made from 55 grams of oxygen gas and an excess of hydrogen at STP?

3) How many liters of water can be made from 55 grams of oxygen gas and an excess of

hydrogen at a pressure of 12.4 atm and a temperature of 850 C? 4) How many liters of water can be made from 34 grams of oxygen gas and an excess

amount of hydrogen gas at STP?

5) ____Na(s) + ___ Cl2(g) ___NaCl(s) a. Balance the above reaction. b. What volume of chlorine gas, measured at STP, is necessary for the complete

reaction of 4.81 g of sodium metal.

L 02 → LHZO1St

A A 3

I MOI 2h01 H2O 22.4L5L 02× - × - X -

= LOL H2O22.4L Imo I 02 IMO I 1St

3 as as

g 02 → L H2Oas 3

2 as

55g Oz ×I MOI 02 2 MOI H2O 22 . 4L

my L µzox x

32.0g 02 I MOI 02 I MOI 25 't

zA as

55802 -7 mo102→molHz0→LHzo^

z A as

nonstP055g02xlm0_0Zx2m0lH20-3.43n5mo1HzO@l2.c, atm 'S 358

-

' 5k

32.0902 lmol 02 2

3 A 5z

3 = 8.1513 - - - L H2O

✓ = nPy=

( 3.4375mA ) ( 8.21×10 -2L . Atmlmol . K ) (358.15k£ g. z < Azo124am 23

g 02-7 MOI 02 -7 MOI H2O -7 L H2O

•A A 3 Sfp

IMO I 02 2h01 H2O 22.4L34802 X

32 . go ,X X 47.6L H2O

I MOI 02 I MOI3 A A = 48L H2O

2

2 2

g Na → MOI Na → MOI C1z→ Lclz^

3 A 3 STPI MOI Na I Mol Clz 22.4L

4.81g Nax X X 2.3422 . - - Laz23.0g Na 2nd Na I MOI

as as3 = 2.34L Clz

3

6) ___C3H8(g) + ___O2(g) ___CO2(g) + ___H2O(g) a. Balance the above reaction.

b. What volume of oxygen gas at 25˚C and 1.04 atm is needed for the complete combustion of 5.53 g of propane?

7) ___ K2MnO4 (s) + ___Cl2(g) ___ KMnO4 (s)+ ___KCl(g) a. Balance the above reaction. b. What volume of Cl2(g), measured at STP, is needed to produce 10.0 g of KMnO4?

8) ___Mg3N2(s) + ___ H2O(l) ___MgO(s) + ___NH3(g) a. Balance the above reaction.

b. If 10.3 g of magnesium nitride is treated with 10.3 g of water, what volume of ammonia gas would be collected at 24˚C and 0.989 atm?

9) ___ Cl2(g) + ____ C2H2(g) ! _____ C2H2Cl4(l) a. Balance the above reaction. b. What volume of Cl2 will be needed to make 75.0 grams of C2H2Cl4 at 24°C and 773 mm Hg?

10) ____ C8H18(l) + ____ O2(g) ! ____ CO2(g) + ____ H2O(g)

a. Balance the above reaction. b. How many grams of water would be produced if 20.0 liters of O2 gas were burned at a temperature of -10.0°C and a pressure of 1.3 atm?

5 3 4PEART

5.53g c3Hq×

18h01

Cato

L€3mHo9→ozm°lC3H8→

Molo# Loz

X = 0.6284 - - - MOI 02

3 440gC3H8as

IMO C3H8 3

3g

5

y= nR¥=

30.6284

- - Mol ( 8.21×10-2 L - atmlk - mot ) ( 25+273 .15k¥14 .

, > go.co . . L

31.04atm

2 2 2

753.0L02

g KMn04 → mot KMn04 → MOI Clz Lazas

3FMOI KMn04 I mot Clz 22 - 4L

10.0g KMn04 × × X3 202.7g KMnO4 2 MOI KMn04 I MOI

4 A co

55254 . . L clz = 0.552L 9210.3g 10.3g 3

LR 3 3 2

ER

Omit . . .

for later

optional2

nonGC2H2Cl¢→ MOI C2HzCl4→ MOI Ck L Clz

asas

175.09

C2H2Cl4×tCd4×2¥= 0.8929 - - MOCK

3 168.0g czHzCl4 IMOI Cut 2014 3

4 as

✓ = HRT :-P = MR (24+2173.15) :-( 7173mm Hgx 7=21.415 .. - Lclz

33 5 3

17620mmHg

2 25 16 18 = 21 L U22

102 -7 MOI 02-7 MOI H2O -7g H2O2 3 A

n= 1¥ =L .3atM ( 20-04 pV=nRT

( 8.21×10-2 L - atmlk - MOI ) ( -10.0+273.1514=1.203 - - - mot 023 5 2

A 3

18 moi H2O 18.09 H2O= 15.596 . -

- 9h201. 203 --

. MOI 02 X XZ 25 Mol 02 I MOI H2O

es as = 16g H2O2