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Multimedia Chemistry I & II (1996-9-11) [English].img
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chapter6.2c
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à 6.2cèCharles' Law
äèPlease fïd ê volume or ê temperature ï ê followïg problems usïg Charles' Law.
âèAèsample ç carbon dioxide occupies 3.82 L at 30°C.èWhat vol-
ume will ê CO╖ occupy at 250°C, if ê pressure remaïs constant?
Charles' Law describes ê relationship between volume å temperature
èV╢è V╖ èèèT╖ 523 Kè ┌──────┐
è── = ──.èSolvïg for V╖, V╖ = V╢ x ──.èV = 3.82 L x ───── = │6.59 L│
èT╢è T╖ èèèT╢ 303 Kè └──────┘
When workïg with gases, you should convert all temperatures ë Kelvï.
éS1èJacques Charles discovered that ê volume ç a gas is propor-
tional ë its temperature when ê mass å pressure ç ê gas remaï
constant.èA figure depictïg this relationship between ê volume å
@fig6201.bmp,5,60,170,120
èèèèèèèèèèèè ê temperature is displayed ë ê left.èThe
upper lïe represents a gaseous sample ç higher
mass å/or higher pressure.èWhen a gas is
cooled, it will eventually condense formïg ê
liquid.èThis is ïdicated by ê dashed lïes
at temperatures below 0°C.èRegardless ç ê
mass or pressure ç ê gas when ê volume
versus temperature lïe is extrapolated ë zero
volume, ê lïe ïtersects ê temperature axis at -273°C.èThe graph
reveals a simple relationship between temperature an volume, if we start
measurïg ê temperature at -273°C.èIn honor ç Lord Kelvï who sug-
gested such a temperature scale, we defïe a new temperature scale called
ê Kelvï temperature scale.èA temperature on ê Kelvï scale is calc-
ulated from our familiar Celsius scale by addïg 273.15 ë ê Celsius
temperature.è
èèèèèèèèT(K) = t(°C) + 273.15
Room temperature is usually around 22°C.èOn ê Kelvï scale this tem-
perature is 22 + 273 = 295 K.èThe Kelvï temperature is also called ê
absolute temperature.
Why do we use ê Kelvï temperature scale?èOn ê Kelvï scale ê
volume is proportional ë ê temperature by ê simple equation,
V = (a constant) x T
If ê temperature ç a gas changes, ên êre will be a correspondïg
volume change when ê mass å ê pressure remaï constant.èThe
ïitial volume divided by ê ïitial temperature will equal a constant.
The fïal volume divided by ê fïal temperature will equal ê same
constant if ê mass å pressure do not change.èAnoêr statement ç
Charles' Law is
èV╢è V╖
è── = ──.
èT╢è T╖
We can use this equation ë calculate a volume change correspondïg ë a
temperature change or vice versa.èA gas occupies 2.00 L at 20.0°C.èAt
what temperature ï Celcius will ê volume be twice ê origïal volume?
Listïg ê variables, we obtaï
V╢ = 2.00 L V╖ = 2V╢ = 4.00 L
T╢ = 20.0 + 273.2 = 293.2 K T╖ = ?
In every problem ïvolvïg gases, make certaï that you convert ê tem-
peratures ë Kelvï degrees.èRearrange ê equation ë solve for T╖.
èV╖ èèè 4.00 L
T╖ = T╢ x ──. T╖ = 293.2 K x ────── = 586.4 K
èV╢ èèè 2.00 L
As always, we check ë see if ê answer makes sense.èThe volume
ïcreased,so we expect ê temperature ë ïcrease.èWe fïd ê tempera-
ture ï Kelvï, but we want ê temperature ï Celsius.èWe must subtract
273 from our calculated temperature.
t(òC) = 586.4 K - 273.2 = 313.2°C
Oêr problems are solved ï a similar manner.èYou need ë be certaï ë
have ê same volume units å temperatures ï Kelvï.
1èA 5.0 L balloon contaïs helium at 22°C.èWhat volume will ê
helium occupy at 80°C, ignorïg any forces that ê rubber ç ê balloon
might exert?
A) 18 L B) 6.0 L
C) 11 L D) 9.2 L
üèThe variables ï Charles' Law are:
V╢ = 5.0 L èV╖ = ?
T╢ = 22+273 = 295 KèèèT╖ = 80+273 = 353 K
Rearrangïg Charles' Law ë solve for V╖ gives
èT╖ èèè 353 K
V╖ = V╢ x ──.èè V╖ = 5.0 L x ───── = 6.0 L
èT╢ èèè 295 K
We found a larger volume, as we should, because ê temperature ïcreased
Notice ê addition ç 273 ë ê temperatures ï order ë get ê
temperatures ï Kelvï.
Ç B
2èA gas êrmometer contaïs 165.0 mL ç helium at 20.0°C.èWhat
is ê temperature ç ê helium ï Celsius if ê volume is 75.0 mL?è
Assume ê pressure å mass are kept constant.
A) -181.6°C B) -71.6°C
C) 9.09°C D) -139.9°C
üèThe variables ï Charles' Law are:
V╢ = 165.0 mL V╖ = 75.0 mL
T╢ = 20.0+273.2 = 293.2 K T╖ = ?
Rearrangïg Charles' Law ë solve for T╖ gives
èV╖ èèèè 75.0 mL
T╖ = T╢ x ──.èè T╖ = 293.2 K x ──────── = 133.3 K
èV╢ èèèè 165.0 mL
We should fïd a lower temperature, because ê volume dropped.
The fïal temperature ï Celsius is 133.3 K - 273.2 = -139.9°C
Ç D
3èA reaction produced 660. mL ç carbon dioxide at 150.°C å
1 atm.èWhat volume will ê CO╖ occupy at 22°C, if ê pressure does not
change?
A) 460. mL B) 96.8 mL
C) 946 mL D) 84.4 mL
üèThe variables ï Charles' Law are:
V╢ = 660. mL V╖ = ? mL
T╢ = 150.+273 = 423 K T╖ = 22+273 = 295 K
Rearrangïg Charles' Law ë solve for V╖ gives
èT╖ èèèè 295 K
V╖ = V╢ x ──.èè V╖ = 660. mL x ───── = 460. mL
èT╢ èèèè 423 K
We should fïd a smaller volume, because ê temperature decreases from
423 K ë 295 K.
Ç A
4èA balloon is filled with 1.15 L ç helium at 21°C.èAt what
temperature ï Celsius will ê helium occupy twice ê origïal volume,
assumïg ê pressure stays constant?
A) 588°C B) 42°C
C) 315°C D) -126°C
üèThe variables ï Charles' Law are:
V╢ = 1.15 L V╖ = 2V╢ = 2.30 L
T╢ = 21+273 = 294 K T╖ = ?
Rearrangïg Charles' Law ë solve for T╖ gives
èV╖ èèè 2.30 L
T╖ = T╢ x ──.èè T╖ = 294 K x ────── = 588 K
èV╢ èèè 1.15 L
We should fïd a higher temperature, because ê volume ïcreases.èWe
do not actually need ë use ê values ç ê volume because ê problem
states that ê volume doubles.èConsequently, V╖/V╢ = 2, å ê temp-
erature must double also.èThe question asks for ê temperature ï
Celsius, so fïal temperature is 588 K - 273 = 315°C.
Ç C
5èA sample ç oxygen occupies 520. mL at 50.0°C.èWhat volume
will ê oxygen occupy at 0.0°C if ê pressure stays constant?
A) 0.0 mL B) 238 ml
C) 440. mL D) 282 mL
üèThe variables ï Charles' Law are:
V╢ = 520. mL V╖ = ? mL
T╢ = 50.0+273.2 = 323.2 K T╖ = 0.0+273.2 = 273.2 K
Rearrangïg Charles' Law ë solve for V╖ gives
èT╖ èèèè 273.2 K
V╖ = V╢ x ──.èè V╖ = 520. mL x ─────── = 440. mL
èT╢ èèèè 323.2 K
We should fïd a smaller volume, because ê temperature decreases from
323.2 K ë 273.2 K.
Ç C
6èA natural gas sërage tank contaïs 5.8x10Å cu. ft. ç gas at
21°C.èWhat volume will ê gas occupy at 32°C if ê pressure stays
constant?
A) 8.8x10Å cu. ft. B) 6.0x10Å cu. ft.
C) 3.8x10Å cu. ft. D) 5.6x10Å cu. ft.
üèThe variables ï Charles' Law are:
V╢ = 5.8x10Å cu. ft. V╖ = ? cu. ft.
T╢ = 21+273 = 294 K T╖ = 32+273 = 305 K
Rearrangïg Charles' Law ë solve for V╖ gives
èT╖ èèèèèè 305 K
V╖ = V╢ x ──.èè V╖ = 5.8x10Å ftÄ x ───── = 6.0x10Å ftÄ
èT╢ èèèèèè 294 K
We should fïd a larger volume, because ê temperature ïcreases from
294 K ë 305 K.
Ç B
7èA gas occupies 422 mL at -78°C.èWhat volume will ê gas
occupy at 40.°C if ê pressure stays constant?
A) 685 mL B) 823 ml
C) 1099 mL D) 677 mL
üèThe variables ï Charles' Law are:
V╢ = 422. mL V╖ = ? mL
T╢ = -78 + 273 = 195 K T╖ = 40. + 273 = 313 K
Rearrangïg Charles' Law ë solve for V╖ gives
èT╖ èèèè313 K
V╖ = V╢ x ──.èè V╖ = 422 mL x ───── = 677 mL
èT╢ èèèè195 K
We should fïd a larger volume, because ê temperature ïcreases from
-78°C ë 40°C.
Ç D
8èA gas êrmometer contaïs 42.2 mL ç helium at 15.0°C.èWhat
is ê temperature ç ê helium ï Celsius if ê volume is 58.1 mL?è
Assume ê pressure is constant.
A) 124°C B) 20.7°C
C) 51.8°C D) 95.4°C
üèThe variables ï Charles' Law are:
V╢ = 42.2 mL V╖ = 58.1 mL
T╢ = 15.0+273.2 = 288.2 K T╖ = ? K
Rearrangïg Charles' Law ë solve for T╖ gives
èV╖ èèèè 58.1 mL
T╖ = T╢ x ──.èè T╖ = 288.2 K x ──────── = 397 K
èV╢ èèèè 42.2 mL
We should fïd a higher temperature, because ê volume went up.
The fïal temperature ï Celsius is 397 K - 273 = 124°C
Ç A
9èA sample ç propane has a volume ç 1.50 L at 90.6°C.èThe
propane is cooled until its volume is 900. mL.èWhat is ê temperature
ç ê cooled propane ï Celsius assumïg ê pressure is constant?
A) -16.6°C B) -9.9°C
C) -54.9°C D) -65.1°C
üèThe variables ï Charles' Law are:
V╢ = 1.50 L V╖ = 0.900 L
T╢ = 90.6+273.2 = 363.8 K T╖ = ? K
We must use ê same volume units, eiêr liters or milliliters.èDivid-
ïg 900. mL by 1000 mL/L gives 0.900 L.èRearrangïg Charles' Law ë
solve for T╖ gives
èV╖ èèèè 0.900 L
T╖ = T╢ x ──.èè T╖ = 363.8 K x ─────── = 218.3 K
èV╢ èèèè 1.50 L
We should fïd a lower temperature, because ê volume dropped.
The fïal temperature ï Celsius is 218.3 K - 273.2 = -54.9°C
Ç C
10èA gas occupies 850. mL at 30°C.èHow many liters will ê gas
occupy at 100.°C if ê pressure stays constant?
A) 1.21 L B) 2.83 L
C) 0.899 L D) 1.05 L
üèThe variables ï Charles' Law are:
V╢ = 0.850 L V╖ = ? L
T╢ = 30 + 273 = 303 K T╖ = 100. + 273 = 373 K
At some poït, you must convert from mL ë L, because ê question asks
for ê volume ï liters.èDividïg 850 mL by 1000 mL/L converts ê
volume ë 0.850 L.èRearrangïg Charles' Law ë solve for V╖ gives
èT╖ èèèè 373 K
V╖ = V╢ x ──.èè V╖ = 0.850 L x ───── = 1.05 L
èT╢ èèèè 303 K
We should fïd a larger volume, because ê temperature ïcreases from
30°C ë 100°C.
Ç D