Find the empirical formula for the following molecular composition. 28 % nitroge

Question

Find the empirical formula for the following molecular composition. 28 % nitrogen, 72 % oxygen If the compound in the above problem has a molar mass of 108 g/mol, what is the molecular formula? Using the molecular formula from the above problem, combine it with dihydrogen monoxide and complete the reaction, list the type of reaction. If there are 45 g of each reactant in the above reaction, what is the limiting reactant, how much product can be produced, and how much excess reactant is left over?

Explanation / Answer

Post one more question to get the remaining answers

Let the mass be 100 gms

Molar mass of N2 = 28

Number of moles of N2 = 28/28 = 1

Number of moles of O2 = 72/32 = 2.25 moles

Hence the empirical formula of the compound N2O5

b) Molar mass of N2O5 = 2 * 14 + 5 * 16 = 108 gm/mol

Hence the compound is N2O5

c) N2O5 + H2O ------ HNO3 + O2

Related Questions

Navigate

• Browse (All)
• Browse F
• Subjects

---

---

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