Final answer:
The student's question pertains to stoichiometry, which is a chemical process of calculating the quantities of reactants and products involved in a chemical reaction. To answer it, one needs the balanced chemical equation and must follow steps to convert mass to moles, use the stoichiometric ratio, and then convert moles back to mass to find the grams of Mn₂O₃ produced.
Step-by-step explanation:
The question asks how many grams of Mn₂O₃ can be produced from the complete reaction of 46.8 grams of MnO₂. This is a stoichiometry problem that requires the use of the balanced chemical equation for the reaction in question. Although the balanced chemical equation is not provided, here is the general approach to solve such a problem:
- Write down the balanced chemical equation for the reaction between MnO₂ and the corresponding reactant(s) to form Mn₂O₃.
- Calculate the number of moles of MnO₂ that the given mass (46.8 g) represents.
- Using the molar ratio from the balanced equation, calculate the number of moles of Mn₂O₃ that would be produced.
- Calculate the mass of Mn₂O₃ produced by multiplying the number of moles of Mn₂O₃ by its molar mass.
To illustrate with an example, assume the balanced equation is A MnO₂ + B other reactant(s) → C Mn₂O₃:
- Calculate moles of MnO₂: moles = 46.8 g / molar mass of MnO₂.
- Calculate moles of Mn₂O₃ produced using the stoichiometric coefficients: moles Mn₂O₃ = (moles of MnO₂) * (C/A).
- Calculate mass of Mn₂O₃: mass Mn₂O₃ = moles Mn₂O₃ * molar mass Mn₂O₃.