The mole is an SI unit used to measure the amount of a substance. Ideal gases are gases that follow certain assumptions to simplify their behaviour.
Equations
description
equation
Number of particles in a substance
N=n×NA
Molar mass
M=nm
Pressure
p=AF
Newton's second law
Fatom=ΔtΔp
Change in momentum
Δp=−2mu
Constants
constant
symbol
value
Avogadroconstant
NA
6.02×1023mol−1
Variable definitions
quantity name
symbol
derived units
si base units
numberofparticles
N
numberofmoles
n
mol
mol
molarmass
M
kgmol−1
kgmol−1
mass
m
kg
kg
pressure
p
Pa
kgm−1s−2
force
F
N
kgms−2
changeinmomentum
Δp
kgms−1
kgms−1
The mole
The mole is an SI unit used to measure the amount of a substance and has the symbol mol. It is defined as the amount of a substance that contains the number of atoms contained in 12g of carbon-12, this number being the Avogadro constant NA with a value of 6.02×1023mol−1.
In other words, 1mol is equal to the amount of a substance that has 6.02×1023 atoms. To find the number of particles in a substance you can then use the equation:
N=n×NA
Where n is the number of moles with units mol.
Another quantity associated with the mole is the molar mass M, with units kgmol−1. It is defined as the mass per 1mol of substance and can be found with the equation:
M=nm
Example
Calculate the number of atoms in 20g of helium gas. Helium has a molar mass of 0.004kgmol−1.
Firstly, write down what you know:
m=20g=0.02kg
M=0.004kgmol−1
Write down the equation for molar mass :
M=nm
Rearrange it for n:
n=Mm
Substitute the numbers and calculate the number of moles in 20g of helium gas:
n=0.0040.02=5mol
Now write down the equation for the number of atoms in a substance:
N=n×NA
Substitute the values and calculate the number of atoms in the helium gas:
N=5×6.02×1023=3.01×1024
There are 3×1024 atoms in 20g of helium gas, to one significant figure.
The kinetic theory of gases
The kinetic theory of gases is a model used to describe the behaviour of ideal gases. These are different from real gases as they follow a set of assumptions to simplify their behaviour.
The assumptions followed by ideal gases are:
The gas particles have no intermolecular forces between each other.
The gas particles occupy a negligible volume compared to the gas itself.
All collisions are perfectly elastic and have negligible time compared to times between collisions, such that no kinetic energy is lost.
The gas particles move in random directions with random speeds.
There are a very large number of atoms or molecules in the gas.
By using these assumptions and Newton's laws it is possible to explain how the particles in a gas behave and cause pressure.
Pressure and change in momentum
When particles collide with a container wall, they exert a pressure. The pressure can be calculated with the following:
p=AF
Using Newton's second law, the force that is exerted onto the atoms from the wall, is the rate of change of momentum. The atoms exert an equal but opposite force on the wall. This force can be calculated using the following equation:
Fatom=ΔtΔp
Note: ΔtIs the time between collisions with the wall. Also, don't get confused with p for pressure and change in momentum. They mean different things!
The imagebelow shows how the movement of a particle colliding with a wall over time:
1.
Positive direction
A
Before
B
After
The particle approaching the wall with a momentum p=mu bounced back with the same momentum due to the collision being elastic. This means that the total change in momentum is equal to the following:
Δp=−2mu
Note: The reason that the total change in momentum is −2mu is due to the velocity changing from +ums−1 to −ums−1 after it has collided with the wall of a container. This is because it has changed direction.
Example
Calculate the change in momentum when a molecule with mass 3.0×10−26kg collides elastically at right angles with a wall at 650ms−1.
Firstly, write down what you know:
m=3.0×10−26kgu=650ms−1
Write down the equation needed:
Δp=−2mu
Substitute in the values, and calculate your final answer to the lowest number of significant figures given in the question:
Δp=−2×3.0×10−26×650=−3.9×10−23kgms−1
The change in momentum of the molecule is−3.9×10−23kgms−1.
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Unit 1
Mole calculations and Avogadro's constant - Higher
Unit 2
The mole and Avogadro's constant
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Unit 3
Ideal gases
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FAQs - Frequently Asked Questions
What is a mole?
A mole is an SI unit used to measure the amount of a substance. It is defined as the amount of a substance that has the same number of atoms as 12 g of carbon-12.
What is molar mass?
The molar mass is the mass of 1 mol of substance.
What is an ideal gas?
An ideal gas is a gas that follows a set of assumptions that simplify its behaviour.