The balanced chemical equation for the reaction between iron and oxygen is:
4 Fe + 3 O2 → 2 Fe2O3
From the balanced equation, we can see that 4 moles of iron react with 3 moles of oxygen to form 2 moles of iron oxide.
To calculate the amount of iron oxide (rust) produced, we need to determine the number of moles of iron. We can use the molar mass of iron to convert grams to moles.
Molar mass of iron (Fe) = 55.845 g/mol
Number of moles of iron = 100g / 55.845 g/mol = 1.79 moles
From the balanced equation, we know that 4 moles of iron react with 2 moles of iron oxide. Therefore, the molar ratio between iron and iron oxide is 4:2 or 1:0.5.
Number of moles of iron oxide (rust) produced = 1.79 moles * 0.5 = 0.895 moles
To calculate the mass of iron oxide produced, we can use the molar mass of iron oxide.
Molar mass of iron oxide (Fe2O3) = 159.69 g/mol
Mass of iron oxide (rust) produced = 0.895 moles * 159.69 g/mol = 143.07 g
Therefore, 100g of iron should produce 143.07g of rust.
iron reacts with oxygen to form iron oxide. if 100g of iron reacts with excess oxygen, how much rust should be produced?
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