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Answered

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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?

Sagot :

Solution:

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.

[tex]\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}}[/tex]

[tex]\boxed{\text{mass of SnF₂ = 215.4 g}}[/tex]

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