Question

The chemical equation below shows the reaction between tin (Sn) and hydrogen fluoride (HF). Sn + 2HF mc017-1.jpg 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?

Answer 1

A. 1

Step-by-step explanation:

Answer 2

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.