The chemical equation below shows the reaction between tin (Sn) and hydrogen fluoride (HF). Sn + 2HF SnF2 + H2 The molar mass of HF is 20.01 g/mol. How many moles of Sn are required to react with 40 g of HF? 1 2 3 4
40/20 = 2 mol of HF
Sn to HF ratio is 1:2 so divide the 2 mol of HF by 2 to get 1 mol of Sn.
Answer: 1 mole
Explanation:
\(Sn+2HF\rightarrow SnF_2+H_2\)
Moles of \(HF=\frac{\text{ given mass}}{\text{ molar mass}}\)
Given mass= 40 g
Molar mass= 20.01 g/mol
Moles of \(HF=\frac{40g}{20.01g/mole}=2moles\)
From the given balanced chemical equation, it can be seen that 2 moles of HF react with 1 mole of Sn.
Thus 1 mole of Sn are required to react with 40 g of HF.