the chemical equation below shows the reaction between tin (sn) and hydrogen fluoride (hf). sn + 2hf → snf₂…

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 completely with 40 g of hf? 1 mole 2 moles 3 moles 4 moles

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 completely with 40 g of hf? 1 mole 2 moles 3 moles 4 moles

Answer

Answer:

A. 1 mole

Explanation:

Step1: Calculate moles of HF

$n_{HF}=\frac{m}{M}=\frac{40\ g}{20.01\ g/mol}\approx2\ mol$

Step2: Use mole - ratio from equation

From $Sn + 2HF\rightarrow SnF_2+H_2$, the mole - ratio of $Sn$ to $HF$ is $1:2$. If $n_{HF} = 2\ mol$, then $n_{Sn}=\frac{1}{2}\times n_{HF}=\frac{1}{2}\times2\ mol = 1\ mol$