Tin (II) flouride is used in some toothpastes. It lis made by the rxn of tin with hydrogen flouride. How many grams of tin (II) flouride are produced from the rxn of 30,00 g of HF with Sn?

Question

- Balance equation
Sn + 2 HF---> 1 SnF2 +H2
-Identify what you have and what you need
known: mass of HF = 30.00g
Unknown: mass of SnF2 g
Use balanced equation to find mole ratios
- 2 mol HF / 1 mol SnF2
- 1 mol SnF2 / 2 mol HF

select the best answer for the sample reaction.

(1 point)

117.5 g
117.5 g

118.7 g
118.7 g

4701 g
4701 g

50.01 g

Answer 1

To find out how many grams of tin(II) fluoride (SnF2) are produced from 30.00 g of hydrogen fluoride (HF), we can follow these steps:

1. Balance the Reaction: The balanced equation you've provided is already correct: \[ \text{Sn} + 2 \text{HF} \rightarrow \text{SnF}_2 + \text{H}_2 \]

2. Calculate Moles of HF: To find the moles of HF, we need its molar mass. The molar mass of HF can be calculated as follows:

   • H: 1.01 g/mol
   • F: 19.00 g/mol
   • Molar mass of HF = 1.01 g/mol + 19.00 g/mol = 20.01 g/mol

   Now calculate the moles of HF: \[ \text{moles of HF} = \frac{\text{mass of HF}}{\text{molar mass of HF}} = \frac{30.00 \text{ g}}{20.01 \text{ g/mol}} \approx 1.499 \text{ mol} \]

3. Use Mole Ratios to Find Moles of SnF2: According to the balanced equation, 2 moles of HF produce 1 mole of SnF2. \[ \text{moles of SnF}_2 = \frac{1.499 \text{ mol HF}}{2} \approx 0.7495 \text{ mol SnF}_2 \]

4. Calculate the Mass of SnF2: Now we need the molar mass of SnF2:

   • Sn: 118.71 g/mol
   • F: 19.00 g/mol (we have 2 Fluorine atoms)
   • Molar mass of SnF2 = 118.71 g/mol + 2(19.00 g/mol) = 118.71 g/mol + 38.00 g/mol = 156.71 g/mol

   Now calculate the mass of SnF2 produced: \[ \text{mass of SnF}_2 = \text{moles of SnF}_2 \times \text{molar mass of SnF}_2 = 0.7495 \text{ mol} \times 156.71 \text{ g/mol} \approx 117.5 \text{ g} \]

So, the best answer for the mass of tin(II) fluoride produced from the reaction is 117.5 g.