Question

The chemical equation below shows the reaction between tin (sn) and hydrogen fluoride (hf). sn 2hf right arrow. 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 1

Stoichiometry calculation is used to know the moles of the substance yielded by the reaction. The moles of tin required to react with HF is 1 mole.

What is a mole?

Moles are the chemical units of the smallest entity present in the atoms, compounds, and molecules in a sample.  

The balanced chemical reaction is shown as,

$\rm Sn + 2 HF \rightarrow SnF_{2} + H_{2}$

From the reaction, 2 moles (40.02 gm) of hydrogen fluoride react with 1 mole of tin to produce the products.

Then, X number of moles are needed to react with 40 gm of hydrogen fluoride.

Solving for X:

$\begin{Aligned} \rm X &= \dfrac{(40\;\rm g \times 1\;\rm Mole)}{40.02\;\rm g}\\\\\\\rm X &= 0.999 \;\rm Moles \\\\\\&= 1 Mole\end{aligned}$

Therefore, to react with 40 gm of hydrogen fluoride, the moles required for tin are option A. 1 mole.

Learn more about moles here:

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