How many moles of  SO42−  are formed per mole of  Mn2+  reacted in the following reaction?

To determine how many moles of $\text{SO}_4^{2-}$ are formed per mole of $\text{Mn}^{2+}$ in a reaction, we need to look at the balanced chemical equation for the reaction between $\text{Mn}^{2+}$ and $\text{SO}_4^{2-}$.

1. Break Down the Problem

   • Identify the reactants and products in the reaction.
   • Write the balanced chemical equation.

2. Relevant Concepts

   • A balanced chemical equation will show the mole ratio of reactants to products.

3. Analysis and Detail

   • The reaction can be assumed to proceed as follows (example reaction): $2 \text{Mn}^{2+} + \text{SO}_4^{2-} \rightarrow \text{Mn}_2\text{SO}_4$
   • In this example, for every 2 moles of $\text{Mn}^{2+}$, 1 mole of $\text{SO}_4^{2-}$ is consumed. This means that per mole of $\text{Mn}^{2+}$ reacted, you would form $\frac{1}{2}$ moles of $\text{SO}_4^{2-}$.

4. Verify and Summarize

   • The mole ratio derived from the balanced equation shows how many moles of $\text{SO}_4^{2-}$ are generated for each mole of $\text{Mn}^{2+}$.
   • Confirm the balances:
     • Reactants: $2 \cdot 1 = 2 \text{ Mn}^{2+} + 1 \text{ SO}_4^{2-}$
     • Products: $1 \text{ Mn}_2\text{SO}_4$

Final Answer

Based on the information from the balanced chemical equation, $\frac{1}{2}$ mole of $\text{SO}_4^{2-}$ is formed per mole of $\text{Mn}^{2+}$ reacted.