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Sagot :
Gas laws discover the relationship of pressure, temperature, volume and amount of gas.
1. Boyles Law
Boyle's Law tells us that the volume of gas increases as the pressure decreases, meaning pressure is inversely propotional to volume.
Equation used for Boyles Law: P1V1 = P2V2
Example: A 17.50mL sample of gas is at 4.500 atm. What will be the volume if the pressure becomes 1.500 atm, with a fixed amount of gas and temperature?
So in this example we are given, P1 and P2, we are also given V1 and we want to know V2. What will happen to the volume if the pressure is increased.
V2 = P1V1/P2
V2 = (4.500 atm x 17.50 mL)/1.500atm
V2 = 52.50mL
This example proves that when the pressure is increased, the volume also increases.
2. Charles Law
Charles' Law tells us that the volume of gas increases as the temperature increases. Volume is directly proportional to Temperature.
The equation used: V1/T1 = V2/T2
Example: A sample of Carbon dioxide in a pump has volume of 20.5 mL and it is at 40.0 oC (=313.15 K). When the amount of gas and pressure remain constant, find the new volume of Carbon dioxide in the pump if temperature is increased to 65.0 oC (=333.15 K).
V2 = (V1 x T2)/T1
V2 = (20.5 mL x 333.15 K)/313.15K
V2 = 21.8 mL
The volume increased as the temperature increased.
3. Avogadro's Law tell us that the volume of gas increases as the amount of gas increases. Volume(V) is directly proportional to the Amount of gas(n).
Equation: P1/n1 = P2/n2 and V1/n1 = V2/n2
Example: A 3.80 g of oxygen gas in a pump has volume of 150 mL. constant temperature and pressure. If 1.20g of oxygen gas is added into the pump. What will be the new volume of oxygen gas in the pump if temperature and pressure held constant?
This problem is asking for V2 of oxygen. We have to first calculate the number of moles of Oxygen.
n1 = 3.80/(15.999 x 2)
n1 = 0.1188 mol
n2 = 1.20/(15.999 X 2)
n2 = 0.0375 mol
V2 = (V1 x n2)/n1
V2 = (150.0mL x 0.0375)/0.1188
V2 = 47.3485 mL
4. The ideal gas law
The ideal gas law is the combination of the three simple gas laws.
Equation: pV = nRT
Example: At 655mm Hg and 25.0oC, a sample of Chlorine gas has volume of 750mL. How many moles of Chlorine gas at this condition?
So we want number of moles.
n = PV/RT
n = 655mmHg x( 1 atm/760 mmHg) x 0.75 L/0.082057L⋅atm⋅mol-1.K-1 x 298.15
n = 0.026 mol
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