Question

After 5.00 g of after 5.00g iron filings rusted completely, it weighted 7.15 g. If a 8.50 g sample

of iron filings used 1.60 g of oxygen to partially rust, how much iron was not oxidized?

Answer 1

To find out how much iron was not oxidized, we need to determine the amount of iron that was oxidized by using the molar mass of iron.

Step-by-step explanation:

To find out how much iron was not oxidized, we need to determine the amount of iron that was oxidized. From the given information, we know that 8.50 g of iron filings used 1.60 g of oxygen to partially rust. The balanced chemical equation for this reaction is:

2 Fe(s) + O₂(g) + 4 H+ (aq) → 2 Fe²+ (aq) + 2 H₂O(1)

From this equation, we can see that for every 1.60 g of oxygen used, 2 moles of iron were oxidized. Now, we can calculate the amount of iron that was oxidized by using the molar mass of iron.