Copyright Sautter 2003 SOLVING GAS LAW PROBLEMS BOYLES LAW CHARLES LAW GAY-LUSSACS LAW THE COMBINED GAS LAW THE IDEAL GAS LAW DALTONS LAW GRAHAMS LAW.

Copyright Sautter 2003

SOLVING GAS LAW PROBLEMS

• BOYLE’S LAW

• CHARLES LAW

• GAY-LUSSAC’S LAW

• THE COMBINED GAS LAW

• THE IDEAL GAS LAW

• DALTON’S LAW

• GRAHAM’S LAW OF DIFFUSION

GAS LAW FORMULAE• BOYLE’S LAW:

P1 x V1 = P2 x V2

• CHARLES LAW:

V1 / T1 = V2 / T2

• GAY-LUSSAC’S LAW:

P1 / T1 = P2 / T2• KELVIN = 273 + DEGREES CELSIUS

• COMBINED GAS LAW

(P1 x V1 ) / T1 = (P2 x V2 ) / T2

• DALTON’S LAW

P TOTAL = PGAS A + P GAS B + P GAS C + P …….

GAS LAW FORMULAE (CONT’D)

• DALTON’S LAW (CONT’D)

• PGAS A = (N GAS A / N TOTAL) x PTOTAL

• AVOGADRO’S HYPOTHESIS “EQUAL VOLUMES OF DIFFERENT GASES,

AT THE SAME TEMPERATURE AND PRESSURE, CONTAIN EQUAL MOLES”

UNIVERSAL GAS LAW P x V = N x R x T

GAS LAW FORMULAE (CONT’D)• GRAHAM’S LAW OF DIFFUSION

v2 / v1 = ( m1 / m2)1/2

v = average molecular velocity

m = molecular mass

ONE MOLE OF ANY GAS OCCUPIES 22.4 LITERS AT STP CONDITIONS

Liters divide by 22.4 moles

Liters multiply by 22.4 moles

SOLVING BOYLE’S LAW PROBLEMS• WHAT IS THE VOLUME OF 500 ML OF NEON GAS AT 2.0 ATMS OF

PRESSURE WHEN ITS PRESSURE IS CHANGED TO 2090 MM OF HG ?

• SOLUTION:

P1 x V1 = P2 x V2 , P1 = 2.0 ATM V1 = 500 ML,

P2 = 2090 MM / 760 = 2.75 ATM

V2 = ( P1 x V1) / P2

V2 = (2.0 x 500) / 2.75 = 364 ML

NOTE: BOYLE’S LAW IS INVERSE, AS PRESSURE INCREASES, VOLUME DECREASES.

SOLVING BOYLE’S LAW PROBLEMS

• IF 6.0 LITERS OF OXYGEN AT 1140 MM OF HG IS REDUCED TO A VOLUME OF 2000 ML, WHAT IS THE NEW PRESSURE OF THE GAS ?

• SOLUTION:

P1 x V1 = P2 x V2 , P1 = 1140 MM V1 = 6.0 L,

V2 = 2000 ML / 1000 = 2.0 L

P2 = ( P1 x V1) / V2

P2 = (1140 x 6.0) / 2.0 = 3420 MM OF HG

SOLVING CHARLES LAW PROBLEMS

• WHAT IS THE VOLUME OF HYDROGEN WHEN 300 ML ARE HEATED FROM 35 CELSIUS TO 80 CELSIUS ?

• SOLUTION:

V1 / T1 = V2 / T2 , V1 = 300 ML

• KELVIN = 273 + DEGREES CELSIUS

• T1 = (35 +273) = 308 K, T2 = (80 + 273) = 353 K

• V2 = (V1 x T2 ) / T1

• V2 = (300 x 353) / 308 = 344 ml

SOLVING CHARLES LAW PROBLEMS• A 500 ml sample of carbon dioxide is reduced to 350 ml by cooling.

If the original temperature has 300 K, what is the new temperature in degrees Celsius ?

• SOLUTION:

V1 / T1 = V2 / T2 , V1 = 500 ML, V2 = 350 ML

T1 = 300 K

• T2 = (V2 x T1 ) / V1

• T2 = (350 x 300) / 500 = 210 K

• KELVIN = 273 + DEGREES CELSIUS

• 210 = 273 + C0 , C0 = - 63

SOLVING GAY-LUSSAC LAW PROBLEMS

• WHAT IS THE PRESSURE OF A CONFINED GAS WITH AN ORIGINAL PRESSURE OF 3.0 ATM AND A TEMPERATURE OF 200K IF THE TEMPERATURE IS INCREASED TO 1000 C0 ?

• SOLUTION:

P1 / T1 = P2 / T2 , P1 = 3.0 ATM, T1 = 200 K

T2 = 1000 C0

• KELVIN = 273 + DEGREES CELSIUS

• K = 273 + 1000 = 1273 K

• P2 = (P1 x T2 ) / T1

• P2 = (3.0 x 1273) / 200 = 19.1 ATM

SOLVING GAY-LUSSAC LAW PROBLEMS• A SAMPLE OF CHLORINE IS RAISED TO 1140 MM OF HG

FROM A PRESSURE OF 0.50 ATM. IF THE ORIGINAL TEMPERATURE WAS 500 K, WHAT IS THE NEW TEMPERATURE IN CELSIUS ?

• SOLUTION:

P1 / T1 = P2 / T2 , P1 = 0.50 ATM, P2 = 1140 / 760 = 1.5 ATM

T1 = 500 K

T2 = (P2 x T1 ) / P1

T2 = (1.5 x 500) / 0.50 = 1500 K

• KELVIN = 273 + DEGREES CELSIUS• 1500 = 273 + C0 , C0 = 1227

SOLVING COMBINED LAW PROBLEMS• WHAT IS THE NEW VOLUME OF 650 ML OF NITROGEN AT

273 K AND 2.0 ATMS WHEN IT IS HEATED TO 819 K AND REDUCED TO 1.0 ATM PRESSURE ?

• SOLUTION:

• (P1 x V1 ) / T1 = (P2 x V2 ) / T2, P1 = 2.0 ATM, P2 = 1.0 ATM

T1 = 273 K, T2 = 819 K

V1 = 650 ml

V2 = (P1 x V1 x T2 ) / (P2 x T1 )

V2 = (2.0 x 650 x 819) / (1.0 x 273) = 3900 ml

SOLVING COMBINED LAW PROBLEMS• WHAT IS THE NEW PRESSURE OF 850 ML OF ARGON AT

1092 K AND 5.0 ATMS WHEN IT IS COOLED TO 273 C AND REDUCED TO A VOLUME OF 300 ML ?

• SOLUTION:

• (P1 x V1 ) / T1 = (P2 x V2 ) / T2, P1 = 5.0 ATM, V2 = 300 ML

T1 = 1092 K, V1 = 850 ML

T2 = (273 + 273) = 546 K

P2 = (P1 x V1 x T2 ) / (V2 x T1 )

P2 = (5.0 x 850 x 546) / (300 x 1092) = 7.1 ATM

SOLVING DALTON’S LAW PROBLEMS

A TANK CONTAINS THREE GASES, N2 , Cl2 AND O2 . THE NITROGEN PRESSURE IS 2.0 ATM, THE CHLORINE 380 MM OF HG AND THE OXYGEN 5.0 ATM. WHAT IS THE PRESSURE IN THE TANK ?

P TOTAL = PGAS A + P GAS B + P GAS C + P …….

P TOTAL = 2.0 ATM + (380/760)ATM + 5.0 ATM = 7.5 ATM

OR 7.5 x 760 = 5700 MM OF HG

SOLVING DALTON’S LAW PROBLEMS

A TANK CONTAINS THREE GASES, H2 , Br2 AND O2 . THE MASS OF HYDROGEN IS 2.0 GRAMS, THE BROMINE MASS IS 240 GRAMS AND THE OXYGEN MASS IS 16.0 GRAMS. THE TOTAL PRESSURE IN THE TANK WAS 4.0 ATM. WHAT IS THE PRESSURE OF THE OXYGEN IN THE TANK ?

• SOLUTION:

• PGAS A = (N GAS A / N TOTAL) x PTOTAL

• MOLES = GRAMS / MOLAR MASS

• H2 = 2.0 / 2.0 = 1.0 MOLES, Br2 = 240 / 160 =1.5 MOLES

O2 = 16.0 / 32 = 0.50 MOLES

PO2 = ( (0.50) / (1.0 + 1.5 + 0.50)) x 4.0 = 0.67 ATM

SOLVING IDEAL GAS LAW PROBLEMS

WHAT IS THE TEMPERATURE OF 68.0 GRAMS OF OF HYDROGEN SULFIDE GAS WITH A VOLUME OF 6.0 LITERS AND A PRESSURE OF 5.0 ATMS ?

SOLUTION:

P x V = N x R x T, P = 5.0 ATM, V = 6.0 LITERS N = 68.0 / 34.0 = 2.0 MOLES R = 0.0821 ATM x L / MOLES x K

T = (P x V) / (N x R) T = (5.0 x 6.0) / (2.0 x 0.0821) = 183 K• KELVIN = 273 + DEGREES CELSIUS• 183 = 273 + C0 , C0 = -90

SOLVING IDEAL GAS LAW PROBLEMS WHAT IS THE VOLUME OF 64.0 GRAMS OF OF OXYGEN GAS

WITH A TEMPERATURE OF 25 DEGREES CELSIUS AND A PRESSURE OF 3.0 ATMS ?

SOLUTION:

P x V = N x R x T, KELVIN = 273 + DEGREES

T= 25 + 273 = 298 K, P = 3.0 ATM

N = 64.0 / 32.0 = 2.0 MOLES

R = 0.0821 ATM x L / MOLES x K

V = (N x R x T) / P

V = (2.0 x 0.0821 x 298) / 3.0

• 183 = 273 + C0 , C0 = -90

SOLVING GRAHAM’S LAW PROBLEMS THE AVERAGE MOLECULAR SPEED OF AN OXYGEN

MOLECULE AT A SPECIFIC TEMPERATURE IS 500 M/SEC. WHAT IS THE AVERAGE SPEED OF A NEON MOLECULE AT THE SAME TEMPERATURE ?

v2 / v1 = ( m1 / m2)1/2

MOLAR MASS OXYGEN = 32.0, MOLAR MASS NEON = 20.0

m1 = 32, m2 = 20.0, v1 = 500 M / SEC

v2 = ( m1 / m2)1/2 (v1) = (32.0/ 20.0) 1/2 (500) =632 M/SEC

SOLVING GRAHAM’S LAW PROBLEMS WHAT IS MOLECULAR MASS OF SUBSTANCE X, IF AT A

SPECIFIC TEMPERATURE THE SPEED OF A NITROGEN MOLECULE IS 800 M/SEC. THE AVERAGE SPEED OF THE UNKNOWN GAS IS 650 M/SEC AT THE SAME TEMPERATURE ?

v2 / v1 = ( m1 / m2)1/2 (squaring both sides gives)

m1 / m2 = v22 / v1

2 (solving for m1 gives)

m1 = (v22 / v1

2) x m2

m2 = Molar mass of Nitrogen = 28.0

v2 = velocity of Nitrogen = 800 m / s

v1 = velocity of unknown gas = 650 m /s

m1 = (8002 / 6502) x 28 = 42.4

SOLVING STP PROBLEMS ONE MOLE OF ANY GAS AT STP ( 0 C OR 273 K AND 1 ATM

OR 760 MM OF HG) OCCUPIES 22.4 LITERS

HOW MANY GRAMS OF HYDROGEN ARE CONTAINED IN 89.6 LITERS AT STP ?

SOLUTION :

Liters divide by 22.4 moles

89.6 / 22.4 = 4.0 MOLES

MOLES x MOLAR MASS = GRAMS

4.0 x 2.0 = 8.0 GRAMS HYDROGEN

SOLVING STP PROBLEMS

MOLE OF ANY GAS AT STP ( 0 C OR 273 K AND 1 ATM OR 760 MM OF HG) OCCUPIES 22.4 LITERS

WHAT IS THE VOLUME OF 96.0 GRAMS OF SULFUR DIOXIDE AT STP ?

SOLUTION :

GRAMS / MOLAR MASS = MOLES

96.0 / 64.0 = 1.5 MOLES

MOLES X 22.4 LITERs

1.5 x 22.4 = 33.6 LITERS