The reaction is:
2 Ag2O-------------4 Ag + O2
The answer is o,43 mole silver.
Balanced equation. C2H6O + 3O2 --> 2CO2 + 3H2O 0.274 moles C2H6O (2 moles CO2/1 mole C2H6O) = 0.548 moles carbon dioxide produced ============================
250 g iron (III) oxide is equal to 1,565 moles.
8,4 liters of nitrous oxide at STP contain 2,65 moles.
The reaction of carbon dioxide and potassium oxide is 4KO2 + 2CO2 = 2K2CO3 + 3O2. 156 grams of CO2 is 3.54 moles, which will produce 5.31 moles of O2.
It decomposes into calcium oxide and carbon dioxide
silver and oxygen
Decomposes into metallic silver and oxygen.
.913 moles
Balanced equation. 4Na + O2 -> 2Na2O 10 moles Na (2 moles Na2O/4 moles Na) = 5.0 moles Na2O produced
Copper(II) oxide decomposes at about 1500 C but Aluminium oxide decomposes at above 2000 C
2Ca + O2 --> 2CaO The molar mass of Calcium is 40g/mol. 36.5g/40g gives you 0.9125 moles of Calcium. The moles of calcium are equivalent to the moles of Calcium oxide. The answer is 0.9125 moles of calcium oxide. Correct me if I am wrong.
1400 grams
silver carbonate decomposes into silver (1) oxide and carbon dioxide Ag2CO3-->Ag2O + CO2 Because both sides are equal you do not have to balance the equation. note: Because silver is a transitional metal you had the choice between silver (3) and silver (1). I decided to choose Silver (1) because that meant that the silver carbonate was completely decomposed and also it is easier to balance the equation.
This is a mole stoichiometry problem. Start with the balanced equation for the synthesis of aluminum oxide: 4Al + 3O2 --> 2Al2O3. The ratio of aluminum to aluminum oxide in this equation is 4:2, or 2:1, so 5.23 moles Al means half that number for Al2O3, so about 2.62 moles of aluminum oxide will be produced.
4Na+O2 2Na2O
This value is 38,9 mol.
12.32 l n20