10. A compound is 42.3 % C, 5.94 % H, 32.9 % N, and 18.8 % O and has a molecular mass of 425.25 g/mol. Calculate the empirical and molecular formula. C15H25N10O5 11. How many moles of Al2O3 are produced by the reaction 200. g Al? 4Al + 302 2Al2O3 → 3.70 mole 12. How many moles Al are required to produce 300. g Al2O3? 4Al + 302 2Al2O3 → 5.88 mole 13. 100. g Al reacts with excess O2 to produce 150. g Al2O3 according to Calculate the theoretical and percentage yield. 4Al + 302 2 Al2O3. → 79.4 % 14. Calculate the energy produced by the complete reaction of 150. g H2. 2H2 + O2 2H2O + 130. KJ → 4.83 x 103 kJ 15. How many grams of H2 would be needed to produce 260. KJ of energy? 2H2 + O2 2H2O + 130. KJ → 8.08 g
10. A compound is 42.3 % C, 5.94 % H, 32.9 % N, and 18.8 % O and has a molecular mass of 425.25 g/mol. Calculate the empirical and molecular formula. C15H25N10O5 11. How many moles of Al2O3 are produced by the reaction 200. g Al? 4Al + 302 → 2Al2O3 3.70 mole 12. How many moles Al are required to produce 300. g Al2O3? 4Al + 302 → 2Al2O3 5.88 mole 13. 100. g Al reacts with excess O2 to produce 150. g Al2O3 according to Calculate the theoretical and percentage yield. 4Al + 302 → 2 Al2O3. 79.4 % 14. Calculate the energy produced by the complete reaction of 150. g H2. 2H2 + O2 → 2H2O + 130. KJ 4.83 x 103 kJ 15. How many grams of H2 would be needed to produce 260. KJ of energy? 2H2 + O2 → 2H2O + 130. KJ 8.08 g
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