Download - Gas equations
![Page 1: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/1.jpg)
Gases
Gas equations
![Page 2: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/2.jpg)
BOYLE’S LAWP
![Page 3: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/3.jpg)
VP ∝ 1
![Page 4: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/4.jpg)
have
PressureAmount
Gases
Volume
Temperature
Amount
![Page 5: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/5.jpg)
x =x =x =x =x =
Volume(dm3)
Pressure(units)
k(proportionality constant: PV)
5 1 5
2,5 2 5
1,67 3 5
1,25 4 5
1 5 5
0,833 6 5
1
2
3
4
5
6 x =
![Page 6: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/6.jpg)
Volume(dm3)
Pressure(units)
k(proportionality constant: PV)
V1 = 5 P1 = 1 5
2,5 2 5
1,67 3 5
1,25 4 5
1 5 5
0,833 6 5
1
2
3
4
5
6
![Page 7: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/7.jpg)
V1 x P1 = k
![Page 8: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/8.jpg)
Volume(dm3)
Pressure(units)
k(proportionality constant: PV)
V1 = 5 P1 = 1 5
V2 = 2,5 P2 = 2 5
1,67 3 5
1,25 4 5
1 5 5
0,833 6 5
1
2
3
4
5
6
![Page 9: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/9.jpg)
V1 x P1 = k
V2 x P2 = k
![Page 10: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/10.jpg)
V1 x P1 = k
V2 x P2 = k
V1 x P1 = V2 x P2
![Page 11: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/11.jpg)
V1 x P1 = k
V2 x P2 = k
V1 x P1 = V2 x P2
P1V1 = P2V2
![Page 12: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/12.jpg)
V1 x P1 = k
V2 x P2 = k
V1 x P1 = V2 x P2
P1V1 = P2V2
![Page 13: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/13.jpg)
P1V1 = P2V2
![Page 14: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/14.jpg)
PRESSURE AND TEMPERATUREP T
![Page 15: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/15.jpg)
TP ∝
![Page 16: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/16.jpg)
have
Amount
Gases
Temperature
Pressure
Volume
Amount
![Page 17: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/17.jpg)
TemperaturePressure
(kPa) k =
(°C) (K)
20 293 1,00 0,0034
40 313 1,07 0,0034
60 333 1,14 0,0034
80 353 1,21 0,0034
100 373 1,28 0,0034
313 586 2,01 0,0034
1
2
3
4
5
6
![Page 18: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/18.jpg)
TemperaturePressure
(kPa) k =
(°C) (K)
20 T1=293 P1=1,00 0,0034
40 313 1,07 0,0034
60 333 1,14 0,0034
80 353 1,21 0,0034
100 373 1,28 0,0034
313 586 2,01 0,0034
1
2
3
4
5
6
![Page 19: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/19.jpg)
= k
![Page 20: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/20.jpg)
TemperaturePressure
(kPa) k =
(°C) (K)
20 T1=293 P1=1,00 0,0034
40 T2=313 P2=1,07 0,0034
60 333 1,14 0,0034
80 353 1,21 0,0034
100 373 1,28 0,0034
313 586 2,01 0,0034
1
2
3
4
5
6
![Page 21: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/21.jpg)
= k = k
![Page 22: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/22.jpg)
= k = k=
![Page 23: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/23.jpg)
=
![Page 24: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/24.jpg)
CHARLES’ LAWV T
![Page 25: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/25.jpg)
V ∝ T
![Page 26: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/26.jpg)
TemperatureVolume
have
Gases
Amount
Pressure
![Page 27: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/27.jpg)
TemperatureVolume
(cm3) k =
(°C) (K)
1 274 34 0,12
14 287 36 0,13
53 326 37 0,11
76 349 41 0,12
1
2
3
4
![Page 28: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/28.jpg)
= k = k
![Page 29: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/29.jpg)
= k = k=
![Page 30: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/30.jpg)
=
![Page 31: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/31.jpg)
GENERAL GAS EQUATION T
![Page 32: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/32.jpg)
Amount
have
Gases
Pressure
TemperatureVolume
![Page 33: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/33.jpg)
Pressure
TemperatureVolume
have
Gases
Amount
![Page 34: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/34.jpg)
P1V1 = P2V2
==
![Page 35: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/35.jpg)
=
![Page 36: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/36.jpg)
QUESTION 1
![Page 37: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/37.jpg)
Question
A gas bubble at the bottom of a lake has a volume of 200cm3 at a temperature of 8C. This bubble rises and when it reaches the surface where the temperature is 15C and the pressure is 100kPa, its volume increases to 550cm3. Calculate the pressure on the bubble when it was at the bottom of the lake.
![Page 38: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/38.jpg)
8C = 281 K
15C = 288 K
![Page 39: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/39.jpg)
==
P1 =
P1 = 268 kPa
![Page 40: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/40.jpg)
==
P1 =
P1 = 268 kPa
![Page 41: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/41.jpg)
==
P1 =
P1 = 268 kPa
![Page 42: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/42.jpg)
have
Gases
Pressure
TemperatureVolume
Amount
![Page 43: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/43.jpg)
Amount
Pressure
TemperatureVolume
have
Gases
![Page 44: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/44.jpg)
Amount
(n)
![Page 45: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/45.jpg)
moles(mol)
measured in
Amount
(n)
![Page 47: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/47.jpg)
n
n
n
n
![Page 48: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/48.jpg)
n
n
n
n
P
P
P
P
![Page 49: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/49.jpg)
nP ∝
![Page 50: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/50.jpg)
=
=
![Page 51: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/51.jpg)
QUESTION
![Page 52: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/52.jpg)
Question
1 mole of gas at 101,3 kPa and 273 K has a volume of 22,4 dm3. What is the volume of 5 moles of gas at 120 kPa and 280 K?
![Page 53: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/53.jpg)
=
=
V2 =
V2 = 97 dm3
![Page 54: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/54.jpg)
=
=
V2 =
V2 = 97 dm3
![Page 55: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/55.jpg)
=
=
V2 =
V2 = 97 dm3
![Page 56: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/56.jpg)
=
=
V2 =
V2 = 97 dm3
![Page 57: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/57.jpg)
Standard Temperature: 273 K
Standard Pressure: 101,3 kPa
![Page 58: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/58.jpg)
STP
Standard Temperature: 273 K
Standard Pressure: 101,3 kPa
![Page 59: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/59.jpg)
STP
Standard Temperature: 273 K
Standard Pressure: 101,3 kPa
Volume of 1 mole of any gas at STP: 22,4 dm3
![Page 60: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/60.jpg)
=
=
8,3 =
![Page 61: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/61.jpg)
=
8,3 =
![Page 62: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/62.jpg)
=
8,3 =
![Page 63: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/63.jpg)
=
8,3 =
R =
PV = nRT
![Page 64: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/64.jpg)
=
8,3 =
R =
PV = nRT
![Page 65: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/65.jpg)
GENERAL GAS EQUATIONPV = nRT
![Page 66: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/66.jpg)
Universal Gas Constant
R = 8,3 J • mol-1 • K-1
![Page 67: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/67.jpg)
Universal Gas Equation
PV = nRT
![Page 68: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/68.jpg)
=
=
8,3 =
R =
![Page 69: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/69.jpg)
=
=
8,3 =
R =
![Page 70: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/70.jpg)
𝑅=8,3 𝑘𝑃𝑎 ∙𝑑𝑚3
𝑚𝑜𝑙 ∙𝐾
![Page 71: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/71.jpg)
1 000 Pa = 1 kPa
![Page 72: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/72.jpg)
1 m3 = 1 000 dm3
![Page 73: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/73.jpg)
1 000 Pa = 1 kPa1 m3 = 1 000 dm3
![Page 74: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/74.jpg)
![Page 75: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/75.jpg)
![Page 76: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/76.jpg)
![Page 77: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/77.jpg)
![Page 78: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/78.jpg)
![Page 79: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/79.jpg)
Universal Gas Constant
R = 8,3 J • mol-1 • K-1
![Page 80: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/80.jpg)
Universal Gas Constant
R = 8,3 J • mol-1 • K-1
![Page 81: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/81.jpg)
QUESTION
![Page 82: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/82.jpg)
Question
What is the volume of 5 moles of gas at 120 kPa and 280 K?
![Page 83: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/83.jpg)
PV = nRT
120•V = 5•8,3•280
V =
V = 97 dm3
![Page 84: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/84.jpg)
PV = nRT
120•V = 5•8,3•280
V =
V = 97 dm3
![Page 85: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/85.jpg)
PV = nRT
120•V = 5•8,3•280
V =
V = 97 dm3
![Page 86: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/86.jpg)
PV = nRT
120•V = 5•8,3•280
V =
V = 97 dm3
![Page 87: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/87.jpg)
SI units
P : PaT : K
V : m3
n : mol
![Page 88: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/88.jpg)
Question
What is the volume of 5 moles of gas at 120 kPa and 280 K?
![Page 89: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/89.jpg)
120 kPa = 120 000 Pa
![Page 90: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/90.jpg)
PV = nRT
120•V = 5•8,3•280
V =
V = 97 dm3
![Page 91: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/91.jpg)
PV = nRT
120 000•V = 5•8,3•280
V =
V = 97 dm3
![Page 92: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/92.jpg)
PV = nRT
120 000•V = 5•8,3•280
V =
V = 97 dm3
![Page 93: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/93.jpg)
PV = nRT
120 000•V = 5•8,3•280
V =
V = 0,097 m3
![Page 94: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/94.jpg)
PV = nRT
120 000•V = 5•8,3•280
V =
V = 0,097 m3
![Page 95: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/95.jpg)
V = 0,097 m3 x = 97 dm3
![Page 96: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/96.jpg)
QUESTION
![Page 97: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/97.jpg)
Question
A sample of nitrogen gas has a mass of 7 g and a volume of 5,6 dm3 at a temperature of 27 °C. Calculate the pressure of the gas.
![Page 98: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/98.jpg)
PV = nRT
![Page 99: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/99.jpg)
![Page 100: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/100.jpg)
N2 (g)
![Page 101: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/101.jpg)
N2
M = 2(14)g•mol-1
M = 28 g•mol-1
![Page 102: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/102.jpg)
n = 7 g N2 x = 0,25 mol N2
![Page 103: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/103.jpg)
n = 7 g N2 x = 0,25 mol N2
![Page 104: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/104.jpg)
T = 27 + 273 = 300 K
![Page 105: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/105.jpg)
V = 5,6 dm3 x = 5,6 x 10-3 m3
![Page 106: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/106.jpg)
V = 5,6 dm3 x = 5,6 x 10-3 m3
![Page 107: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/107.jpg)
V = 5,6 dm3 x = 5,6 x 10-3 m3
T = 27 + 273 = 300 K
n = 7 g N2 x = 0,25 mol N2
![Page 108: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/108.jpg)
V = 5,6 dm3 x = 5,6 x 10-3 m3
T = 27 + 273 = 300 K
n = 7 g N2 x = 0,25 mol N2
![Page 109: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/109.jpg)
PV = nRT
P• 5,6 x 10-3 = 0,25 • 8,3 • 300
P =
P = 111 160 Pa
P = 111,160 kPa = 111 kPa
![Page 110: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/110.jpg)
PV = nRT
P• 5,6 x 10-3 = 0,25 • 8,3 • 300
P =
P = 111 160 Pa
P = 111,160 kPa = 111 kPa
![Page 111: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/111.jpg)
PV = nRT
P• 5,6 x 10-3 = 0,25 • 8,3 • 300
P =
P = 111 160 Pa
![Page 112: Gas equations](https://reader036.vdocuments.us/reader036/viewer/2022062706/557d112dd8b42a153b8b51ed/html5/thumbnails/112.jpg)
PV = nRT
P• 5,6 x 10-3 = 0,25 • 8,3 • 300
P =
P = 111 160 Pa
P = 111,160 kPa = 111 kPa