The Reactivity of Tin with Hydrogen Fluoride
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?
Tin and Hydrofluoric Acid reacts as shown,
Sn + 2 HF → SnF₂ + H₂
According to Equation,
40.02 g (2 Moles) HF Required = 1 Mole of Sn for complete Reaction
So,
40 g of HF will require = X Moles of Sn
Solving for X,
X = (40 g × 1 Mole) ÷ 40.02 g
X ≈ 0.999 Moles ≈ 1 Mole
Result:
40 g of HF requires 1 Mole of Tin (Sn) for complete Reaction to produce SnF₂ and H₂.
How many moles of Sn are required to react with 40 g of HF? A. 1