Iron(II) sulfate, FeSO4, is prescribed for the treatment of anemia. How many moles of FeSO4 are present in a standard 300 mg tablet? How many iron(II) ions?

검증된 단계별 안내

Step 1: Determine the molar mass of FeSO_4.

Step 2: Convert the mass of the FeSO_4 tablet from milligrams to grams.

Step 3: Use the molar mass to convert the mass of FeSO_4 in grams to moles.

Step 4: Recognize that each mole of FeSO_4 contains one mole of Fe^{2+} ions.

Step 5: Calculate the number of Fe^{2+} ions using Avogadro's number.

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주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is calculated by summing the atomic masses of all the atoms in a chemical formula. For iron(II) sulfate (FeSO4), the molar mass is approximately 151.91 g/mol, which is essential for converting between mass and moles.

Moles and Mass Relationship

The relationship between moles and mass is defined by the equation: moles = mass (g) / molar mass (g/mol). This equation allows us to determine the number of moles of a substance when its mass is known. In this case, knowing the mass of the FeSO4 tablet enables us to calculate the moles of FeSO4 present.

Stoichiometry

Stoichiometry is the area of chemistry that deals with the quantitative relationships between the reactants and products in a chemical reaction. In this context, it helps us understand how many iron(II) ions are produced from the dissociation of FeSO4 in solution, as each formula unit of FeSO4 yields one iron(II) ion.