Final answer:
To find the moles of Fe²⁺ ions in one tablet, calculate the molar mass of ferrous gluconate, divide the mass of ferrous gluconate provided (0.144 g) by its molar mass, and that will give the moles of Fe²⁺ ions contained in the tablet.
Step-by-step explanation:
The question asks to determine how many moles of Fe²⁺ ions are contained in one tablet of iron-supplemented vitamin, given that the tablet contains 0.144 g of ferrous gluconate (Fe(C6H10O7)2). To answer this question, we must use the molar mass of ferrous gluconate to convert the mass to moles.
First, we calculate the molar mass of ferrous gluconate using the formula:
- Fe: 1 x 55.85 g/mol
- C: 12 x 12.01 g/mol
- H: 20 x 1.008 g/mol
- O: 14 x 15.999 g/mol
Adding these values together gives the molar mass of ferrous gluconate. Then, we use this molar mass to convert the mass of ferrous gluconate in the tablet (0.144 g) to moles:
Moles of ferrous gluconate = Mass of ferrous gluconate / Molar mass of ferrous gluconate
Since each molecule of ferrous gluconate contains one iron (Fe²⁺) ion, the moles of ferrous gluconate would be equal to the moles of iron ions. Lastly, we compare the calculated value to the answer choices provided.