A 12.00 g sample of manganese is heated and allowed to react completely with the

Question

A 12.00 g sample of manganese is heated and allowed to react completely with the oxygen in the air to form an oxide having a mass of 18.99 g. What are the moles for each component? Also, what is the whole number ratio of manganese to oxygen. I need help with the conversion calculation, please...thank you!!!

Explanation / Answer

Mn(s) + O2(g) ---> Mn(x)O(y) (unbalanced equation) Mass of Mn in product = 12.00g Mass of product = 18.99g Therefore mass of O in product = 18.99-12.00 = 6.99g moles Mn = 12.00/54.93 = 0.218 mol of Mn moles O = 6.99/15.999 = 0.4369 mol of O Therefore product has a roughly 1:2 Mn:O stoichiometry (0.4369/0.218 = roughly 2) and the answer is MnO2

Related Questions

Navigate

• Browse (All)
• Browse A
• Subjects

---

---

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