A compound of iron and chlorine was formed by reacting 2.80 g of iron with 3.55 g of chlorine - Edexcel - GCSE Chemistry - Question 6 - 2014 - Paper 1
Question 6
A compound of iron and chlorine was formed by reacting 2.80 g of iron with 3.55 g of chlorine.
Calculate the empirical formula of the compound.
(relative atomic mas... show full transcript
Worked Solution & Example Answer:A compound of iron and chlorine was formed by reacting 2.80 g of iron with 3.55 g of chlorine - Edexcel - GCSE Chemistry - Question 6 - 2014 - Paper 1
Step 1
Calculate the number of moles of Iron (Fe)
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Answer
To find the number of moles of iron, use the formula:
ext{Moles} = rac{ ext{mass}}{ ext{molar mass}}
For iron:
Mass = 2.80 g
Molar mass of Fe = 56.0 g/mol
Thus, the calculation is:
ext{Moles of Fe} = rac{2.80 ext{ g}}{56.0 ext{ g/mol}} = 0.05 ext{ mol}
Step 2
Calculate the number of moles of Chlorine (Cl)
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Answer
For chlorine:
Mass = 3.55 g
Molar mass of Cl = 35.5 g/mol
Using the same formula:
ext{Moles of Cl} = rac{3.55 ext{ g}}{35.5 ext{ g/mol}} = 0.1 ext{ mol}
Step 3
Determine the simplest mole ratio
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Next, find the simplest ratio of moles of Fe to moles of Cl:
Moles of Fe = 0.05
Moles of Cl = 0.1
The ratio can be simplified by dividing by the smallest number of moles:
ext{Ratio of Fe:Cl} = rac{0.05}{0.05} : rac{0.1}{0.05} = 1 : 2
Step 4
Write the empirical formula
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Answer
From the simplest ratio of 1:2, the empirical formula of the compound is:
