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Stoichiometric Calculations Using Chemical Equations

Chemistry ⇒ Stoichiometry and Chemical Calculations

Stoichiometric Calculations Using Chemical Equations starts at 10 and continues till grade 12. QuestionsToday has an evolving set of questions to continuously challenge students so that their knowledge grows in Stoichiometric Calculations Using Chemical Equations. How you perform is determined by your score and the time you take. When you play a quiz, your answers are evaluated in concept instead of actual words and definitions used.
See sample questions for grade 11
A reaction has a percent yield of 60%. If the theoretical yield is 50.0 g, what is the actual yield?
A reaction has a theoretical yield of 25.0 g and an actual yield of 20.0 g. What is the percent yield?
A reaction produces 15.0 g of product, but the theoretical yield is 20.0 g. What is the percent yield?
A sample of 10.0 g of H2 reacts with excess O2 to form H2O. How many grams of H2O are produced? (2H2 + O2 → 2H2O; Molar mass: H2 = 2.0 g/mol, H2O = 18.0 g/mol)
A student mixes 8.0 g of H2 with 32.0 g of O2. According to the equation 2H2 + O2 → 2H2O, which reactant is in excess? (Molar mass: H2 = 2.0 g/mol, O2 = 32.0 g/mol)
A student reacts 10.0 g of Ca with 20.0 g of Cl2 to form CaCl2 according to the equation: Ca + Cl2 → CaCl2. Which is the limiting reactant? (Molar masses: Ca = 40.1 g/mol, Cl2 = 70.9 g/mol)
Describe the steps involved in solving a stoichiometric problem involving mass-to-mass conversion.
Explain the difference between theoretical yield and actual yield.
Explain why a balanced chemical equation is necessary for stoichiometric calculations.
How many grams of NaCl are produced when 2.0 moles of Na react with excess Cl2? (2Na + Cl2 → 2NaCl; Molar mass NaCl = 58.5 g/mol)
How many liters of CO2 at STP are produced from 10.0 g of CaCO3? (CaCO3 → CaO + CO2; Molar mass: CaCO3 = 100.0 g/mol; 1 mol gas at STP = 22.4 L)
How many moles of CO2 are produced when 5 moles of C2H6 combust completely? (C2H6 + 3.5O2 → 2CO2 + 3H2O)
If 2.0 moles of Fe react with 3.0 moles of O2 to form Fe2O3 (4Fe + 3O2 → 2Fe2O3), what is the limiting reactant?
If 4 moles of NH3 are produced from the reaction N2 + 3H2 → 2NH3, how many moles of H2 are required?
In the reaction 2KClO3 → 2KCl + 3O2, how many grams of O2 are produced from 12.25 g of KClO3? (Molar mass: KClO3 = 122.5 g/mol, O2 = 32.0 g/mol)
In the reaction 2Na + 2H2O → 2NaOH + H2, how many grams of NaOH are produced from 4.6 g of Na? (Molar mass: Na = 23.0 g/mol, NaOH = 40.0 g/mol)
In the reaction 2SO2 + O2 → 2SO3, how many moles of SO3 are formed from 5 moles of SO2?
What is the mole ratio of H2O to O2 in the balanced equation: 2H2 + O2 → 2H2O?