The combustion of 1.66 g ultrafine aluminum in air results in 2.97g of a product, which is a mixture of 80 % aluminum oxide and 20% aluminum nitride (% by mass) Use the empirical formula of aluminum oxide and find the formula for aluminum nitride. Report the molar amount of aluminum oxide: ттol so that the molar amount of aluminum in the nitride can be found as: тmol and the molar amount of nitrogen is: ттоl so that the ratio of aluminum to nitrogen can be found to be: а.и.

The combustion of 1.66 g ultrafine aluminum in air results in 2.97g of a product, which is a mixture of 80 % aluminum oxide and 20% aluminum nitride (% by mass) Use the empirical formula of aluminum oxide and find the formula for aluminum nitride. Report the molar amount of aluminum oxide: ттol so that the molar amount of aluminum in the nitride can be found as: тmol and the molar amount of nitrogen is: ттоl so that the ratio of aluminum to nitrogen can be found to be: а.и.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Write a balanced chemical equation based on the following description:solid C₄H₁₀O is burned with oxygen gas to produce gaseous carbon dioxide and water vapor
An important reaction for the conversion of natural gas toother useful hydrocarbons is the conversion of methane toethane.2 CH4(g)---->C2H6(g) + H2(g)In practice, this reaction is carried out in the presence of oxygen,which converts the hydrogen produced into water.2 CH4(g) + 1/2O2(g)---->C2H6(g) + H2O(g)Use Table 8.3 to estimate ΔH for these two reactions. Why isthe conversion of methane to ethane more favorable whenoxygen is used?
Write and balance the chemical equation and then determine which reactant is the limiting reagent based on the amounts of reagents given. Finally, determine how much water is produced in grams 2.0moles of nitric acid reacts with 2.1 moles of aqueous sodium hydroxide
Complete combustion of 4.5892 a particular compound that contains only carbon, hydrogen and oxygen produces 10.4324 g of CO2 and 4.2705 g of H2O. The empirical formula of the compound is given by C H O (indicate "1" if there is only one atom of a given type in the empirical formula.) The molar mass of the compound is found to be 116.16 g/mol in a different experiment. What is the molecular formula of the compound? C H O
Lead(II) oxide from an ore can be reduced to elemental lead by heating in a furnace with carbon. Calculate the expected yield of lead if 67.0 kg of lead oxide is heated with 67.0 kg of carbon.
The balanced equation for the decomposition of potassium chlorate is shown below. When carried out in lab, this reaction is found to produce 1.2 g of potassium chloride. For your convenience, the molar mass of each substance Is shown below their formulas (in purple). Use this Information to make the requested calculation: 2 KCIO3(s) -> 2 KCI(s) + 3 02(g) 122.551 74.551 32 Determine the percent yield if the reaction consumes 2900 mg of potassium chlorate:
How many grams of P2O5P2O5 are formed when 9.51 g 9.51 g of phosphorus reacts with excess oxygen? Show the unit analysis used for the calculation by placing the correct components into the unit-factor slots.
For the following reaction: C3Hg(g) + O2(g) ————> CO2(g) + H2O(g) a). balance the reaction b). determine the limiting reactant from 20.0 grams for each starting reactant c). calculate the theoretical yield of CO2(g) in grams d). calculate the percent yield if the actual yield was 10.7 grams
FeSO4 + Potassium phosphate à Iron (II) phosphate + K2SO4 State the Molar Ratio of the reaction.
Write a balanced chemical equation based on the following description: liquid C₇H₈O is burned with oxygen gas to produce gaseous carbon dioxide and water vapor
For the reaction Ti(s) + 2 F2 (g) → TIF4(s) compute the theoretical yield of the product (in grams) for each of the following initial amounts of reactants.
To determine the mass of SbF₃ needed to produce 1.00 g of Freon-12 (CCl₂F₂), you can use the balanced chemical equation and the molar masses of the substances involved. The balanced chemical equation for the reaction is not provided, but assuming a hypothetical balanced equation: