the mole 9.5
Post on 27-Jun-2015
578 Views
Preview:
TRANSCRIPT
Chapter 9.5Percentage Composition
by Mass
Percentage Composition of Compounds
Chemists need to conduct analysis in order to find out how much of each element there is in a new compound.
They do so by finding out the mass of each element in the compound.
In this way, chemists know the percentage composition of a compound.
How do we find the percentage composition of
element?
Percentage by mass of an element in a compound
Ar of element × number of atoms in formula
Mr of compound
= 100%
The percentage by mass of an element in a compound can be found using the formula:
Worked Example 1:Ammonia (NH3)
• Calculate the percentage composition by mass of nitrogen and hydrogen present in ammonia, NH3.
• Step 1:Relative molecular mass (Mr) of ammonia
= 1 x A r of N + 3 x A r of H
= 14 + 3= 17
• Percentage composition of nitrogen in ammonia = A r of nitrogen x number of nitrogen atoms in formula X 100%
relative molecular mass (M r) of ammonia
= 14 x1 x 100% 17= 82.4 %
• Percentage composition of hydrogen in a ammonia = A r of hydrogen x number of atoms in formula X 100%
• relative molecular mass (M r) of ammonia
• = 1 x 3 x 100%
• 17• = 17.6 %•
Worked Example 2: Hydrogen Peroxide (H2O2)
Mr of hydrogen peroxide (H2O2) = (2 × 1) + (2 × 16) = 34
Percentage of hydrogen in hydrogen peroxide
Ar of hydrogen × number of hydrogen atoms
Mr of hydrogen peroxide =
1 2
34=
= 5.9 %
100%
100%
Calculate the percentage composition by mass of hydrogen and oxygen present in hydrogen peroxide (H2O2)
Percentage of oxygen in hydrogen peroxide
Ar of oxygen × number of oxygen atoms
Mr of hydrogen peroxide =
16 2
34=
= 94.1 %
100%
100%
Example 3 Calculate the percentage of water in copper(II) sulphate crystals (CuSO4.5H2O).
Mr of copper(II) sulphate crystals = 64 + 32 + (4 × 16) + (5 × 18) = 250
Mr of water = (1 × 2) + 16 = 18
Percentage of water in CuSO4.5H2OMr of water × number of water molecules
Mr of copper(II) sulphate crystals =
18 5
250=
= 36 %
100%
100%
Worked Example 4
• Calculate the mass of calcium in 25g of calcium nitrate Ca(NO3)2
• Step 1: Mr of Ca(NO3)2
= 40 + 2 x (14 + 16 x 3) = 164
• Step 2: Percentage composition by mass of Ca in Ca(NO3)2
= A r of Ca x number of Ca atoms in formula X 100%
M r of Ca(NO3)2
= 40 X 1 X 100% 164
= 24.39%
• Step 3: Mass of calcium in 25g of calcium nitrate = 24.39/100 X 25g= 6.10g
Worked Example 5
Calculate the mass of water in 54.1g of FeCl3. 6H2O
Step 1: Mr of FeCl3. 6H2O
= 56 + 35.5 X 3 + 6 x (1 X 2 + 16) = 270.5
Step 2: Mr of water, H2O = 2 X 1 + 16 = 18
• Step 3: Percentage composition by mass of water in FeCl3. 6H2O
= Mr of water x No. of water molecules in formula X 100%
M r of FeCl3. 6H2O
= 18 X 6 X 100% 270.5
= 39.9%
Step 4: Mass of water in 54.1g of FeCl3. 6H2O
• = 39.9/ 100 X 54.1= 21.6g
Worked Example 5 (cont’d)
top related