Question

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

Answer 1

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.

Answer 2

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.