Question

Tin (II) fluoride is used in some toothpastes. It is made by a reaction of tin with hydrogen fluoride. How many grams of tin (II) fluoride are produced in the condition below, calculate to the nearest hundredth of a gram? Use the steps below to get yourself started.







(2 points)

Answer 1

1. Write out the balanced chemical equation for the reaction:

Sn + 2HF -> SnF2 + H2

2. Determine the molar mass of tin (II) fluoride (SnF2):
Molar mass of Sn = 118.71 g/mol
Molar mass of F = 19.00 g/mol
Molar mass of SnF2 = 118.71 + (2 * 19.00) = 156.71 g/mol

3. Convert the given mass of tin (Sn) to moles:
Given mass of tin (Sn) = 25.0 g
Moles of Sn = 25.0 g / 118.71 g/mol = 0.211 mol

4. Use the mole ratio from the balanced chemical equation to determine the moles of tin (II) fluoride (SnF2) produced:
From the balanced equation: 1 mol of Sn produces 1 mol of SnF2
Moles of SnF2 = 0.211 mol

5. Convert the moles of tin (II) fluoride (SnF2) to grams:
Mass of SnF2 = moles of SnF2 * molar mass of SnF2
= 0.211 mol * 156.71 g/mol
= 33.08 g

Therefore, approximately 33.08 grams of tin (II) fluoride are produced in this reaction.