Fluorine reacts with uranium hexafluoride, \(\mathrm{UF}_{6}\), as represented by this equation: \(\mathrm{U}(\mathrm{s})+3 \mathrm{~F}_{2}(\mathrm{~g}) \rightarrow \mathrm{UF}_{6}(\mathrm{~g})\) How many fluorine molecules are required to produce \(2.0 \mathrm{mg}\) of uranium hexafluoride, \(\mathrm{UF}_{6}\), from an excess of uranium? The molar mass of \(\mathrm{UF}_{6}\) is \(352.0 \mathrm{~g} \mathrm{~mol}^{-1} .\) (a) \(5.13 \times 10^{18}\) (b) \(1.026 \times 10^{19}\) (c) \(2.052 \times 10^{19}\) (d) \(1.026 \times 10^{20}\)

Chemical reaction stoichiometry is a branch of chemistry that quantifies the relationships between reactants and products in chemical reactions. Using stoichiometry, we can predict how much of each substance is needed or produced in a reaction. The key tool for this prediction is the balanced chemical equation, which provides the mole-to-mole ratio between reactants and products.

Consider a simple reaction where substance A reacts with substance B to produce substance C. If the balanced equation states that 1 molecule of A reacts with 2 molecules of B to produce 3 molecules of C, we have a clear relationship: for every mole of A, we need two moles of B to make three moles of C. This example illustrates the fundamental principle of stoichiometry: the law of conservation of mass, which states that mass is neither created nor destroyed in a chemical reaction. Therefore, the amount of reactants consumed will equal the amount of products formed, allowing us to perform exact calculations.

Mole-to-mole ratio calculations are a critical part of solving stoichiometry problems. These ratios come directly from the coefficients of a balanced chemical equation. The coefficients indicate the number of moles of each substance involved in the reaction.

In the case of the reaction between uranium (U) and fluorine (F2), the balanced equation tells us that 1 mole of U reacts with 3 moles of F2 to produce 1 mole of UF6. To calculate the amount of a reactant required or the amount of a product yielded, we need to compare the given information to these ratios. For example, if we are given the mass of the product UF6 and need to find the number of F2 molecules needed, we first convert the mass of UF6 to moles, and then use the 1:3 mole ratio to find the moles of F2 required.

Avogadro's number, approximately 6.022 x 10^23 molecules/mol, is a fundamental constant in chemistry that represents the number of units (atoms, molecules, ions, etc.) in one mole of any substance. It bridges the gap between the atomic scale and the macroscopic scale, allowing chemists to work with quantities of substances in the lab.

To utilize Avogadro's number in stoichiometry problems, after calculating the moles of a reactant or product needed, we multiply that amount by Avogadro's number to convert it to the actual number of molecules or atoms. When asked how many fluorine molecules are required to produce a certain amount of UF6, after finding the moles of F2 needed using the balanced chemical equation and mole-to-mole ratios, we then multiply by Avogadro's number to find the precise number of F2 molecules.