Iron is produced in a single displacement reaction with iron II cyanide and tin. How many grams of iron are produced when you use 1.98 g of tin?
To determine the number of grams of iron produced in the reaction, we can use stoichiometry.
First, we need to write the balanced chemical equation for the reaction:
Fe(CN)₂ + Sn → Fe + Sn(CN)₂
From the balanced equation, we see that 1 mole of iron (Fe) is produced from 1 mole of tin (Sn). We need to find the number of moles of tin in order to calculate the moles of iron produced.
To find the number of moles of tin, we use the molar mass of tin (Sn), which is 118.71 g/mol.
Moles of tin = mass of tin / molar mass of tin
Moles of tin = 1.98 g / 118.71 g/mol
Moles of tin ≈ 0.0167 mol
Now that we have the number of moles of tin, we can use stoichiometry to find the moles of iron produced.
From the balanced equation, we know that 1 mole of tin reacts to produce 1 mole of iron.
Moles of iron = Moles of tin
Moles of iron ≈ 0.0167 mol
Finally, we can calculate the mass of iron produced using the molar mass of iron (Fe), which is 55.85 g/mol.
Mass of iron = Moles of iron × molar mass of iron
Mass of iron = 0.0167 mol × 55.85 g/mol
Mass of iron ≈ 0.934 g
Therefore, when you use 1.98 g of tin, approximately 0.934 g of iron is produced in the reaction.