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Tin metal reacts with hydrogen fluoride to produce tin(II) fluoride and hydrogen gas according to the following balanced equation:

Sn(s)+HF(g)→SnF2(s)+H2(g)

Balance the given chemical equation and solve for the mass in grams of hydrogen fluoride, HF needed to react with 5 moles of tin, Sn.

Respuesta :

First step is to balance the chemical equation:

Sn(s) + 4HF(g) → SnF2(s) + 2H2(g)

To find the mass in grams of hydrogen fluoride needed to react with 5 moles of tin:

1. Calculate the molar mass of HF:

  Molar mass of H = 1g/mol

  Molar mass of F = 19g/mol

  Molar mass of HF = 1g/mol + 19g/mol = 20g/mol

2. Calculate the number of moles of HF needed using the balanced equation:

  5 moles of Sn × (4 moles of HF / 1 mole of Sn) = 20 moles of HF

3. Convert moles to grams:

  Mass = moles × molar mass

  Mass = 20 moles × 20g/mol = 400g

So, 400 grams of hydrogen fluoride are needed to react with 5 moles of tin.

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