How many milliliters of 0.250 M KMnO4 are needed to react with 3.55 g of iron(II) sulfate, FeSO

step 1 So we are given again. So we'll find first number of moles of FESO4. We have the mass of FESO4 d

How many milliliters of 0.250 M KMnO4 are needed to react...

How many milliliters of $0.250 \mathrm{M} \mathrm{KMnO}_{4}$ are needed to react with $3.55 \mathrm{~g}$ of iron(II) sulfate, $\mathrm{FeSO}_{4}$ ? The reaction is as follows: $$ \begin{array}{r} 10 \mathrm{FeSO}_{4}(a q)+2 \mathrm{KMnO}_{4}(a q)+8 \mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow \\ 5 \mathrm{Fe}_{2}\left(\mathrm{SO}_{4}\right)_{3}(a q)+2 \mathrm{MnSO}_{4}(a q)+\mathrm{K}_{2} \mathrm{SO}_{4}(a q)+ \\ 8 \mathrm{H}_{2} \mathrm{O}(l) \end{array} $$

How many milliliters of $0.250 \mathrm{M} \mathrm{KMnO}_{4}$ are needed to react with $3.55 \mathrm{~g}$ of iron(II) sulfate, $\mathrm{FeSO}_{4}$ ? The reaction is as follows:
$$
\begin{array}{r}
10 \mathrm{FeSO}_{4}(a q)+2 \mathrm{KMnO}_{4}(a q)+8 \mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow \\
5 \mathrm{Fe}_{2}\left(\mathrm{SO}_{4}\right)_{3}(a q)+2 \mathrm{MnSO}_{4}(a q)+\mathrm{K}_{2} \mathrm{SO}_{4}(a q)+ \\
8 \mathrm{H}_{2} \mathrm{O}(l)
\end{array}
$$

Key Concepts

Molarity

Molarity is defined as the number of moles of solute per liter of solution. It is used to relate the volume of a solution to the amount of dissolved substance, playing a crucial role in determining how much of a reacting compound is present in a given volume.

Balanced Chemical Equation

A balanced chemical equation provides the stoichiometrically correct relationships between reactants and products in a chemical reaction. It indicates the precise molar ratios of each substance involved, which is essential for calculating how much of one reactant is needed to completely react with another.

Stoichiometry

Stoichiometry involves using the molar relationships provided by the balanced chemical equation to calculate the amounts of reactants and products. It allows one to convert between masses, moles, and volumes, ensuring that the proportions of substances in a chemical reaction are properly maintained.

Molar Mass

Molar mass is the mass of one mole of a substance, expressed in grams per mole. It is used to convert a measured mass of a compound into moles, which is a necessary step in stoichiometric calculations.

Unit Conversion

Unit conversion is the process of converting one set of units to another, such as converting grams to moles or milliliters to liters. This is essential in chemical calculations to ensure consistency in the units used throughout the problem.

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