One method to synthesize ionic solids is by the heating of two reactants at high temperatures. Consider the reaction of FeO with TiO₂ to form FeTiO₃. Determine the amount of each of the two reactants to prepare 2.500 g FeTiO₃, assuming the reaction goes to completion. (a) Write a balanced chemical reaction. (c) Determine the moles of FeTiO₃.

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1. Step 1: Write the balanced chemical equation for the reaction. The reaction between FeO and TiO2 to form FeTiO3 can be represented as: \[ \text{FeO} + \text{TiO}_2 \rightarrow \text{FeTiO}_3 \]. Ensure that the equation is balanced in terms of atoms on both sides.
2. Step 2: Calculate the molar mass of FeTiO3. To do this, sum the atomic masses of iron (Fe), titanium (Ti), and oxygen (O) based on their respective quantities in the formula FeTiO3. Use the periodic table to find the atomic masses: Fe = 55.85 g/mol, Ti = 47.87 g/mol, O = 16.00 g/mol.
3. Step 3: Determine the moles of FeTiO3 needed to produce 2.500 g of the compound. Use the formula: \[ \text{moles} = \frac{\text{mass}}{\text{molar mass}} \]. Substitute the mass of FeTiO3 (2.500 g) and the molar mass calculated in Step 2 into this formula.
4. Step 4: Use stoichiometry to find the moles of FeO and TiO2 required. From the balanced equation, the molar ratio of FeO to FeTiO3 and TiO2 to FeTiO3 is 1:1. Therefore, the moles of FeO and TiO2 needed are equal to the moles of FeTiO3 calculated in Step 3.
5. Step 5: Calculate the mass of each reactant (FeO and TiO2) required. Use the formula: \[ \text{mass} = \text{moles} \times \text{molar mass} \]. Find the molar masses of FeO and TiO2 using the periodic table: FeO = 71.85 g/mol, TiO2 = 79.87 g/mol. Multiply the moles of each reactant by their respective molar masses to find the mass needed.