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. (d) Determine moles and mass (g) of FeO required.

Verified step by step guidance

1. <Step 1: Write the balanced chemical equation for the reaction.> \[ \text{FeO} + \text{TiO}_2 \rightarrow \text{FeTiO}_3 \]
2. <Step 2: Calculate the molar mass of FeTiO3 using the atomic masses of Fe, Ti, and O.>
3. <Step 3: Determine the moles of FeTiO3 needed by dividing the given mass (2.500 g) by the molar mass of FeTiO3.>
4. <Step 4: Use the stoichiometry of the balanced equation to find the moles of FeO required. Since the reaction is 1:1, the moles of FeO needed will be equal to the moles of FeTiO3.>
5. <Step 5: Calculate the mass of FeO required by multiplying the moles of FeO by its molar mass.>

Key Concepts

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced chemical equation. It allows chemists to determine the proportions of substances involved in a reaction, which is essential for predicting how much of each reactant is needed to produce a desired amount of product.

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is crucial for converting between the mass of a substance and the number of moles, enabling the calculation of how much of each reactant is required to achieve a specific mass of product in a chemical reaction.

Limiting Reactant

The limiting reactant is the substance that is completely consumed first in a chemical reaction, thus determining the maximum amount of product that can be formed. Identifying the limiting reactant is essential for accurate stoichiometric calculations, as it influences the amounts of other reactants needed and the yield of the product.