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Mass-Mass, Mass-Volume, and Volume-Volume Calculations in Reactions

Chemistry ⇒ Stoichiometry and Chemical Calculations

Mass-Mass, Mass-Volume, and Volume-Volume Calculations in Reactions starts at 11 and continues till grade 12. QuestionsToday has an evolving set of questions to continuously challenge students so that their knowledge grows in Mass-Mass, Mass-Volume, and Volume-Volume Calculations in Reactions. 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
Describe the difference between a mass-mass and a mass-volume stoichiometric calculation.
Describe the steps required to calculate the mass of a product formed from a given mass of reactant in a chemical reaction.
Explain why it is important to use a balanced chemical equation in stoichiometric calculations.
Explain why the volume ratios of gases in a chemical reaction at STP are the same as the mole ratios.
A reaction produces 18.0 g of H2O. How many moles of H2O is this? (Molar mass: H2O = 18.0 g/mol)
A reaction produces 2.24 L of O2 at STP. How many grams of O2 is this? (Molar mass: O2 = 32.0 g/mol)
A reaction requires 32.0 g of O2. What is the volume of O2 at STP? (Molar mass: O2 = 32.0 g/mol)
A reaction uses 5.0 g of Na and produces H2 gas. What volume of H2 is produced at STP? (2Na + 2H2O → 2NaOH + H2; Molar mass: Na = 23.0 g/mol)
Which law allows you to relate the volumes of gases in a chemical reaction at constant temperature and pressure? (1) Boyle's Law (2) Avogadro's Law (3) Charles's Law (4) Dalton's Law
Which of the following best describes a mass-mass stoichiometric calculation? (1) Calculating the mass of a product from the mass of a reactant (2) Calculating the volume of a gas from the mass of a solid (3) Calculating the number of atoms in a molecule (4) Calculating the concentration of a solution
Which of the following is a correct step in a mass-volume calculation? (1) Convert mass to moles, then moles to volume (2) Convert volume to mass, then mass to moles (3) Convert moles to mass, then mass to volume (4) Convert volume to moles, then moles to mass
Which of the following is a mass-volume calculation? (1) Calculating the mass of a product from the mass of a reactant (2) Calculating the volume of a gas produced from the mass of a reactant (3) Calculating the mass of a reactant from the volume of a gas (4) Both 2 and 3
Fill in the blank: At standard temperature and pressure (STP), 1 mole of any ideal gas occupies _______ L.
Fill in the blank: In the reaction 2H2 + O2 → 2H2O, 2.0 g of H2 will produce _______ L of H2O at STP.
Fill in the blank: In the reaction 2H2 + O2 → 2H2O, 22.4 L of O2 at STP will produce _______ L of H2O.
Fill in the blank: In the reaction 2H2 + O2 → 2H2O, 4.0 g of H2 will produce _______ g of H2O. (Molar mass: H2 = 2.0 g/mol, H2O = 18.0 g/mol)
True or False: In a mass-mass calculation, the limiting reactant determines the maximum amount of product that can be formed.
True or False: In a mass-volume calculation, you can use the molar volume of a gas at STP to convert between moles and volume.
True or False: The coefficients in a balanced chemical equation represent the ratio of moles, not the ratio of masses.
True or False: The mass of a product in a chemical reaction can be calculated directly from the mass of a reactant without using the balanced equation.