If iron is oxidized to Fe2+ by a copper(II) sulfate solution, and 0.607 grams of

Question

If iron is oxidized to Fe2+ by a copper(II) sulfate solution, and 0.607 grams of iron and 21.2 mL of 0.413M copper(II) sulfate react to form as much product as possible, how many millimoles (mmol) of the non-limiting reactant will remain unused at the end of the reaction? a.) Amount of non-limiting reactant remaining unused = ______mmol Copper(II) sulfate in solution is blue in color. Iron(II) sulfate is colorless. In the reaction described above, will the solution at the end of the experiment be blue or colorless? b.) The solution will be______

Explanation / Answer

how many moles is 0.854 grams of iron? To find that, you need to divide the mass (0.854g) by the Ar of iron, which is 55.8 Then, to find the amount of moles of copper sulphate, you multiply the concentration by the volume. that's 0.531 x 0.0112 whichever has more moles represents the reagent in excess, which will dictate the colour of the solution.

Related Questions

Navigate

• Browse (All)
• Browse I
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.