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.
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See sample questions for grade 11
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 produces 44.8 L of CO2 gas at STP. How many moles of CO2 is this?
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)
A sample of 4.0 g of H2 reacts with excess O2. What is the mass of H2O produced? (2H2 + O2 → 2H2O; Molar mass: H2 = 2.0 g/mol, H2O = 18.0 g/mol)
A student has 10.0 g of CaCO3. How many grams of CO2 can be produced by heating it? (CaCO3 → CaO + CO2; Molar mass: CaCO3 = 100.0 g/mol, CO2 = 44.0 g/mol)
A student reacts 16.0 g of CH4 with excess O2. How many grams of CO2 are produced? (CH4 + 2O2 → CO2 + 2H2O; Molar mass: CH4 = 16.0 g/mol, CO2 = 44.0 g/mol)
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.
If 10.0 g of hydrogen reacts with excess oxygen, what mass of water (H2O) is produced? (Molar mass: H2 = 2.0 g/mol, H2O = 18.0 g/mol)
If 2.0 g of H2 reacts with O2, what volume of O2 is required at STP? (2H2 + O2 → 2H2O)
If 22.4 L of H2 reacts with N2 at STP, what volume of NH3 is produced? (N2 + 3H2 → 2NH3)
If 5.0 g of NaCl is dissolved in water, how many moles of NaCl are present? (Molar mass: NaCl = 58.5 g/mol)
If 5.6 L of N2 reacts with excess H2 at STP, what volume of NH3 is produced? (N2 + 3H2 → 2NH3)
In the reaction: N2 + 3H2 → 2NH3, what is the volume of NH3 produced at STP from 6.72 L of H2?
