Question

Tin metal reacts with hyrdogen to produce tin(2) fluoride and hydrogen gas. How many moles of hydrogen fluorde are required to react completely with 75.0g of tin

Answer 1

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

Sn(s)+2HF(g)→SnF2(s)+H2(g)

How many moles of hydrogen fluoride are required to react completely with 75.0 g of tin?

Step 1: List the known quantities and plan the problem.

Known

Known

given: 75.0 g Sn

molar mass of Sn = 118.69 g/mol

1 mol Sn = 2 mol HF (mole ratio)

Unknown

mol HF

Use the molar mass of Sn to convert the grams of Sn to moles. Then use the mole ratio to convert from mol Sn to mol HF. This will be done in a single two-step calculation.

g Sn → mol Sn → mol HF

Step 2: Solve.

75.0 g Sn× (1 mol Sn/118.69 g Sn) ×(2 mol HF/1 mol Sn) =1.26 mol HF