Iron tablets were analyzed using $0.05 \mathrm{M}, 18 \mathrm{mLKMnO}_{4}$. (MW of iron $56 \frac{\mathrm{g}}{\mathrm{m}} \mathrm{ol}$ ) Calculate the mass of iron presenting in the tables in milligrams.

Select one:
a. 213
b. 252
c. 198
d. 244

Question

Iron tablets were analyzed using $0.05 \mathrm{M}, 18 \mathrm{mLKMnO}_{4}$. (MW of iron $56 \frac{\mathrm{g}}{\mathrm{m}} \mathrm{ol}$ ) Calculate the mass of iron presenting in the tables in milligrams.

Select one:
a. 213
b. 252
c. 198
d. 244

Accepted Answer

***D*** ∻Key Concept∻ ⚹Stoichiometry and Redox Reactions⚹ ∻Explanation∻ ⚹To determine the mass of iron in the tablets, we use the stoichiometry of the redox reaction between iron and potassium permanganate. The balanced equation and molar ratios help us calculate the moles of iron, which can then be converted to mass using the molar mass of iron.⚹◊What is the molarity of the potassium permanganate solution being used in the analysis of the iron tablets?⍭ Generate me a similar question◊

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