what number of molecules of O2 is consumed when 33.6 litres of H2o is produced according to the following reaction ( NH3 +O2 ÷ No + H2O
Answers
Explanation:
Stoichiometry: the numericalrelationship between chemical quantities in a balanced chemical equation. Ex. 4NH3 + 5O2 → 4NO + 6H2OThe reaction above can mean: 4 molecules of NH3reacts with 5 molecules of O2to produce 4 molecules of NO and 6 molecules of H2O.It also can be interpreted as: 4 molesof NH3reacts with 5 molesof O2to produce 4 molesof NO and 6 molesof H2O.How many moles of water can be produced from 4 moles of NH3in the chemical reaction above? (assume excess O2)How many moles of water can be produced from 5.6moles of NH3in the chemical reaction above?To solve this problem we need to use a mole ratioderived from the balanced chemical equation (text uses term "equivalence") Mole ratios relating amounts of NH3and H2O in equation above:4 moles NH3 or 6 moles H2O6 mole H2O 4 moles NH
4 NH3 + 5 O2 → 4 NO + 6 H2OHow many moles of O2are needed to produce 7.2 moles of NO? (assume there is excess NH3)How many moles of ammonia (NH3) is needed for complete reaction with 0.850 moles of oxygen gas?Mass-to-Mass ConversionsGrams A Moles A Moles B Grams BConversion factor:Use molar mass of AUse mole ratio fromthe balanced equationUse molar mass of B(molar mass N2H4= 32.05g/mol; H2O2= 34.02 g/mol)Ex. How many grams of H2O2are needed to completely react with 50.0 g of N2H4? N2H4 (l)+ 2 H2O2(l)→N2(g)+ 4