Question

Tin(II) fluoride is added to some dental products to help

prevent cavities. Tin(II) fluoride is prepared according
to the following equation:
Sn(s) + 2HF(aq) → SnF2(aq) + H2(g)
How many grams of tin(II) fluoride can be produced
from 55.0 g of hydrogen fluoride if there is plenty of tin
available to react?

Answer 1

To find the mass of tin(II) fluoride produced from 55.0 g of hydrogen fluoride, we can use stoichiometry. By converting the mass of tin to moles, using the balanced equation, and calculating the grams of HF, we can determine that 55.0 g of HF can react completely with 18.52 g of tin to produce tin(II) fluoride.

Step-by-step explanation:

To determine the mass of tin(II) fluoride produced, we need to use stoichiometry to calculate the number of moles of hydrogen fluoride (HF) required to react with 55.0 g of tin. First, we need to convert the mass of tin to moles by dividing by its molar mass. Then, we use the balanced equation to find the ratio between tin and HF. According to the equation, 1 mole of Sn reacts with 2 moles of HF to produce 1 mole of SnF2. Finally, we convert the moles of HF to grams by multiplying by its molar mass.

Let's calculate:

1. Calculate the moles of tin: Moles of Sn = Mass of Sn / Molar mass of Sn
2. Use the mole ratio from the balanced equation to find the moles of HF: Moles of HF = Moles of Sn x (2 moles of HF / 1 mole of Sn)
3. Calculate the grams of HF: Mass of HF = Moles of HF x Molar mass of HF

Plug in the values to calculate:

Moles of Sn = 55.0 g / 118.71 g/mol = 0.463 mol

Moles of HF = 0.463 mol x (2 mol HF / 1 mol Sn) = 0.926 mol

Mass of HF = 0.926 mol x 20.01 g/mol = 18.52 g

Therefore, 55.0 g of hydrogen fluoride can react completely with 18.52 g of tin to produce tin(II) fluoride.

Answer 2

Step 1: Calculate the molar mass of HF and SnF₂.

For HF

molar mass = (1.008 g/mol × 1) + (19.00 g/mol × 1)

molar mass = 20.008 g/mol

For SnF₂

molar mass = (118.7 g/mol × 1) + (19.00 g/mol × 2)

molar mass = 156.7 g/mol

Step 2: Determine the mole ratio needed.

mole ratio = 2 mol HF : 1 mol SnF₂

Step 3: Calculate the mass of SnF₂ produced by using the mole ratio.

`\text{mass of SnF₂ = 55.0 g HF} × \frac{\text{1 mol HF}}{\text{20.008 g HF}} × \frac{\text{1 mol SnF₂}}{\text{2 mol HF}} × \frac{\text{156.7 g SnF₂}}{\text{1 mol SnF₂}}`

`\boxed{\text{mass of SnF₂ = 215.4 g}}`