1.) A 10g example of an oxide of copper when heated in a stem of hydrogen forms

Question

1.) A 10g example of an oxide of copper when heated in a stem of hydrogen forms 1.26g of water. What is % of copper by mass in the compound?

2.) A sample of ammonium dichromate contains 2.25 moles of hydrogen atoms. How many moles of oxygen atoms are in the sample?

3.) Barium peroxide decomposes when heated to give BaO and O2. Write the balanced equation for this reaction. How many moles of O2 is formed when 0.500 mole of BaO2 is decomposed?

4.) Based on the given chemical equation, how many grams of aluminum are needed to react with 0.6 moles of hydrochloric acid? Al + HCl yields AlCl3 + H2

5.)For the reaction MnO2 + KOH + O2 + Cl2 produce KMnO4 + KCl + H2O
a. Balance the chemical equation.
b. If there is 100 g of each reactant available, which reagent is the limiting reactant?
c. how many grams of KMnO4 can be produced?

6.)NO2 + H2O produce HNO3 +NO
How many grams of nitric acid, HNO3, can be prepared from the reaction of 92.0 grams of nitrogen dioxide with 30 g of water?
What is the excess reactant?
How many grams of the excess reactant will be used?
How many grams of the excess reactant will be left unreacted?

7. How many moles of water will be produced from the complete combustion of 4.4g of C3H8?
8. How many grams of oxygen gas are required to burn 4.4 grams of C3H8?

Explanation / Answer

2) 2.25 moles of oxygen

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