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Chapter 3: Problem 42

Tin(II) fluoride \(\left(\mathrm{SnF}_{2}\right)\) is often added to toothpaste as an ingredient to prevent tooth decay. What is the mass of \(\mathrm{F}\) in grams in \(24.6 \mathrm{~g}\) of the compound?

Short Answer

Expert verified
The mass of F in \(24.6 \mathrm{~g}\) of \(\mathrm{SnF}_{2}\) is given by \(24.6 \mathrm{~g}\) times the ratio of the molar mass of F to the molar mass of the compound.

Step by step solution

01

Determination of Molar Mass

First, the molar mass of the entire compound, \(\mathrm{SnF}_{2}\), must be determined.\nThe molar mass of Sn (Tin) is \(\approx118.71\) g/mol, and the molar mass of F (Fluorine) is \(\approx18.998\) g/mol. Since there are two F atoms in the compound, the total molar mass is \(118.71 + 2 * 18.998 = 156.706\) g/mol.
02

Ratio Calculation

The next step involves calculating the ratio of each element's molar mass to the total molar mass of the compound. For fluorine,\n\[ \frac {2 * 18.998} {156.706} \]
03

Mass of F in the compound

Then apply this ratio to the given mass of the compound to find the mass of F in \(24.6 \mathrm{~g}\) of the compound. Multiply \(24.6 \mathrm{~g}\) by the ratio calculated above to get the mass of F.

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Most popular questions from this chapter

When \(0.273 \mathrm{~g}\) of \(\mathrm{Mg}\) is heated strongly in a nitrogen \(\left(\mathrm{N}_{2}\right)\) atmosphere, a chemical reaction occurs. The product of the reaction weighs 0.378 g. Calculate the empirical formula of the compound containing \(\mathrm{Mg}\) and \(\mathrm{N}\). Name the compound.

How many grams of \(\mathrm{H}_{2} \mathrm{O}\) will be produced from the complete combustion of \(26.7 \mathrm{~g}\) of butane \(\left(\mathrm{C}_{4} \mathrm{H}_{10}\right) ?\)

Does \(1 \mathrm{~g}\) of hydrogen molecules contain as many \(\mathrm{H}\) atoms as \(1 \mathrm{~g}\) of hydrogen atoms?

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Why must a chemical equation be balanced? What law is obeyed by a balanced chemical equation?
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