1What is relative atomic mass?
It is defined as the average mass of an atom of an element compared to 1/12 the mass of a carbon-12 atom.
2What is the unit for atomic mass, Ar?
There is no unit
3What is the formula of relative atomic mass
mass of one atom of the element / 1/12 the mass of a carbon-12 atom
4Where can you get the mass of one atom of an element
From the periodic table with the relative atomic mass number located under the element name
5What is relative molecular mass
It is defined as the average mass of one molecule of that substance compared to 1/12 the mass of a carbon-12 atom
6What is relative formula mass for ionic compounds
It is defined as the average mass of one unit of that substance compared to 1/12 the mass of a carbon-12 atom
7What is the formula for relative molecular mass
$\frac{mass \space of \space one \space molecule \space or \space one \space unit \space of \space the \space substance}{1/12 \space the \space mass \space of \space a \space carbon-12 \space atom}$
8What is Ar used to describe
Atoms
9What is Mr used to describe
Molecules
10What is the Mr of a compound
The sum of the Ar of the elements in a substance
11What value of atoms do you use to calculate molecular mass
Their relative atomic mass which is the bottom number in element in the periodic table
12How many particles does 1 mole contain?
$6 \times 10^{23}$
13How to calculate molar mass?
$The \space molecular \space mass \times the\space number\space of\space mols$
14What is the formula for number of moles?
$\frac{Mass \space of \space substance \space (g)} {Molar \space mass \space of \space the \space substance \space (g/mol)}$
15What is the formula for number of moles of gas
$\frac{Volume \space of \space gas \space (dm^3)} {24dm^3}$
16How much $cm^3$ is equal to $1 dm^3 $
1000
17What is the ratio of moles of gases equal to
The ratio of volumes of gases
18So how much oxygen will be produced if oxygen reacts with carbon dioxide and is 10 with the gas ratio being 2:1 respectively
5cm^3
19What is the formula for the number of moles of a solution
$Concentration \space of \space solution \space (mol/dm^3) \times volume \space of \space solution \space (dm^3)$
20How to convert a solution from $mol/dm^3 \space to \space g/dm^3$
Multiply it by the molar mass of the substance
21What’s a limiting reactant
It’s the lowest reactant which determines the amount of product formed