Tin (ii) fluoride , snf2, is found in some toothpastes. tin (iii) fluoride is made by reacting solid tin with hydrogen fluoride according to the following balanced equation. sn(s) + 2 hf (g) -> snf2(s) + h2(g) how many moles of tin are needed to react with 8.4 moles of hydrogen fluoride ?

The Balance Chemical Equation is as;

                                 Sn  +  2 HF   →    SnF₂  +  H₂

According to Equation,

                        2 Moles of HF requires  =  1 Mole of Sn
So,
                 8.4 Moles of HF will require  =  X Moles of Sn

Solving for X,
                            X  =  (8.4 mol × 1 mol) ÷ 2 mol

                            X  =  4.2 Moles of Sn

Result:
           4.2 Moles of Tin are needed to react with 8.4 moles of Hydrogen Fluoride

Sorry i dont understand the question can you rephase it?

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