This paper will discuss the gas laws which are: Avogadro’s principle, Boyle’s law and Charles’ law. Almost every undergraduate and graduate chemistry book introducing the ideal gas with these three laws.
These laws are constantly made of pressure, volume, amount of gas and temperature. The ideal gas law is PV=nRT. The three laws of gas define the relationship between pressure (P), volume (V), amount of gas (n) and temperature (T). Boyle’s law says that volume increases when pressure decreases. Charles’ law says that volume increases when temperature increases. Avogadro’s law says that volume increases when amount of gas increases. The ideal gas law is the result of combining the three laws of gas.
Avogadro’s Law: Avogadro's Law is a principle
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He proved that 6.022 x 1023 particles are present in 1 mole of a gas. which means if there is 1 mole of Hilum atom, then there are 6.022 x 1023 atoms of Helium. If there is 1 mole of sodium chloride, then there is one mole of Na+ and one mole of Cl- ion in the solid. Also, if there is 1 mole of oxygen molecule, therefor there are 6.022 x 1023 molecule of oxygen atoms
At Standard Temperature and Pressure 6.022 x 1023 particles of any gas will occupy 22.4L From this, the number of particles can be found when the volume at STP is given. For example, If 2.24L of oxygen gas at STP has given, then it can be easily conclude that the volume would contain one tenth of the mole of oxygen gas. That is, total number of 6.022 x 1022 molecules of oxygen will be present.
CONSEQUENCES OF AVOGADRO'S LAW
There are a few important consequences of Avogadro's law
The molar volume of all ideal gases at 1 atm pressure and 0°C is 22.4 L
the volume increases. the amount of gas increases, only If temperature and pressure of a gas are constant
when the volume decreases and amount of gas decreases, If pressure and temperature of a gas are constant.
The fallowing graph shows the relationship between mass (n) and volume (v) as shown in Avogadro's Law.
Boyle’s Law:
Robert William Boyle is an Irish. Boyle was born in
• These particles are much smaller than the distance between particles, therefore the volume of a gas is mostly empty space and the volume of the gas molecule themselves is negligible. • There is no force of attraction between gas particles or between the particles and the walls of the container. • Collisions between
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Colin Turner Professor Kuykendall CHE 102 10 February 2017 Title: Experiment 2: Determining The Molar Mass of a Volatile Liquid Introduction: In this lab experiment, the ideal gas law will be used to find the average molecular mass of the unknown liquid as a gas. This will be done by heating the liquid until it is in its gaseous state and then once it is there it will be determined what the average molecular mass is.
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so when you multiply the 2.9 by 2 it gives you 5.8 cm3 which was my result. As the voltage increases the volume of hydrogen and oxygen increases. The standard deviation when I used 9 volts for hydrogen it was 0.7 + 0.23= 0.93 and 0.7-0.23= 0.47 so the range of values is between 0.47 cm3 to 0.93 cm3. When I used 9 volts for oxygen it was 0.3+0.12=0.42 and 0.3-0.12=0.18 so the range of values is between 0.18 cm3 to 0.42 cm3.