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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 mass... 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 moles of Fe

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Answer

To find the moles of iron, we use the formula:

$\text{moles} = \frac{\text{mass}}{\text{molar mass}}$

Substituting the values:

$\text{moles of Fe} = \frac{2.80}{56.0} = 0.05$

Step 2

Calculate the moles of Cl

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Answer

Next, we calculate the moles of chlorine using the same formula:

$\text{moles of Cl} = \frac{3.55}{35.5} = 0.1$

Step 3

Determine the simplest ratio

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Answer

Now we find the simplest mole ratio by dividing both values by the smallest number of moles:

For Fe: $\frac{0.05}{0.05} = 1$ For Cl: $\frac{0.1}{0.05} = 2$

This gives us a ratio of Fe to Cl of 1:2.

Step 4

Write the empirical formula

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Answer

The empirical formula based on the ratio is:

$\text{FeCl}_2$

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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

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

Calculate the moles of Fe

Calculate the moles of Cl

Determine the simplest ratio

Write the empirical formula

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