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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A mixture of 10.0 g of sodium reacts with 10.0 g of chlorine gas to form sodium chloride. Which is the limiting reactant? (Na = 23.0, Cl = 35.5) 2Na + Cl2 → 2NaCl
A reaction of 10.0 g of potassium chlorate (KClO3) decomposes to form potassium chloride and oxygen gas. Calculate the volume of O2 produced at STP. (K = 39.1, Cl = 35.5, O = 16.0) 2KClO3 → 2KCl + 3O2
A reaction of 2.00 g of hydrogen gas with excess nitrogen produces ammonia. Calculate the mass of ammonia formed. (H = 1.0, N = 14.0) N2 + 3H2 → 2NH3
A reaction produces 44.8 L of CO2 gas at STP. How many moles of CO2 is this?
A reaction produces 5.60 L of oxygen gas at STP. How many grams of O2 is this? (O = 16.0)
A sample of 3.00 g of magnesium reacts with hydrochloric acid. Calculate the volume of hydrogen gas produced at STP. (Mg = 24.3) Mg + 2HCl → MgCl2 + H2
A sample of 4.00 g of hydrogen gas reacts with excess oxygen. What volume of water vapor is produced at STP? 2H2 + O2 → 2H2O
A student reacts 5.00 g of sodium carbonate (Na2CO3) with excess hydrochloric acid. Calculate the volume of CO2 gas produced at STP. (Na = 23.0, C = 12.0, O = 16.0)
Calculate the mass of water produced when 8.00 g of methane is combusted in excess oxygen. (C = 12.0, H = 1.0) CH4 + 2O2 → CO2 + 2H2O
Describe how to determine the limiting reactant in a mass-mass stoichiometric problem.
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.
If 10.0 g of aluminum reacts with excess oxygen, what mass of aluminum oxide (Al2O3) is formed? (Al = 27.0, O = 16.0) 4Al + 3O2 → 2Al2O3
If 10.0 g of calcium reacts with excess hydrochloric acid, what mass of calcium chloride (CaCl2) is produced? (Ca = 40.1, Cl = 35.5) Ca + 2HCl → CaCl2 + H2
If 2.00 L of H2 gas reacts with excess O2 gas at STP, what volume of H2O vapor is produced? 2H2 + O2 → 2H2O
If 3.00 g of carbon reacts with excess oxygen, what volume of CO2 gas is produced at STP? (C = 12.0) C + O2 → CO2
If 5.00 L of hydrogen gas reacts with 2.50 L of oxygen gas at STP, what is the limiting reactant? 2H2 + O2 → 2H2O
In the reaction 2H2 + O2 → 2H2O, what volume of O2 (at STP) is required to react completely with 4.0 g of H2? (H = 1.0)
