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. What mass of sodium chloride (NaCl) is produced when 12.5 grams of sodium (Na) reacts with an excess of chlorine gas (Cl2)?
The balanced equation is 2Na + Cl2 → 2NaCl. Using the molar mass of NaCl (58.44 g/mol), the mass of NaCl produced is 32.8 grams.
What mass of silver (Ag) is produced when 25.0 grams of copper (Cu) reacts with an excess of silver nitrate (AgNO3) solution?
The balanced equation is Cu + 2AgNO3 → Cu(NO3)2 + 2Ag. Using the molar mass of Ag (107.87 g/mol), the mass of Ag produced is 33.7 grams.
How many grams of sodium hydroxide (NaOH) are required to neutralize 20.0 grams of sulfuric acid (H2SO4)?
The balanced equation is 2NaOH + H2SO4 → Na2SO4 + 2H2O. Using the molar mass of NaOH (40.00 g/mol), the mass of NaOH required is 39.2 grams.
What volume of hydrogen gas (H2) is produced when 30.0 grams of zinc (Zn) reacts with an excess of hydrochloric acid (HCl)?
The balanced equation is Zn + 2HCl → ZnCl2 + H2. Using the molar volume of H2 (22.4 L/mol), the volume of H2 produced is 13.8 liters.
. What volume of oxygen gas (O2) is required to completely burn 25.0 grams of propanol (C3H7OH)?
The balanced equation is 2C3H7OH + 9O2 → 6CO2 + 8H2O. Using the molar volume of O2 (22.4 L/mol), the volume of O2 required is 33.6 liters.
The balanced equation is 2Na + Cl2 → 2NaCl. Using the molar mass of NaCl (58.44 g/mol), the mass of NaCl produced is 32.8 grams.
The balanced equation is 2Al + 6HCl → 2AlCl3 + 3H2. Using the molar volume of H2 (22.4 L/mol), the volume of H2 produced is 22.4 liters.
How many grams of barium sulfate (BaSO4) are produced when 20.0 grams of barium chloride (BaCl2) reacts with an excess of sulfuric acid (H2SO4)?
The balanced equation is BaCl2 + H2SO4 → BaSO4 + 2HCl. Using the molar mass of BaSO4 (233.39 g/mol), the mass of BaSO4 produced is 27.0 grams.
What mass of water (H2O) is produced when 10.0 grams of octane (C8H18) is completely burned in oxygen (O2)?
The balanced equation is 2C8H18 + 25O2 → 16CO2 + 18H2O. Using the molar mass of H2O (18.02 g/mol), the mass of H2O produced is 12.6 grams.
How many grams of iron(III) oxide (Fe2O3) are required to react with 18.0 grams of aluminum (Al) to produce iron (Fe) and aluminum oxide (Al2O3)?
The balanced equation is 2Al + Fe2O3 → 2Fe + Al2O3. Using the molar mass of Fe2O3 (159.69 g/mol), the mass of Fe2O3 required is 53.2 grams.
How many grams of iron(III) oxide (Fe2O3) are produced when 20.0 grams of iron (Fe) reacts with an excess of oxygen gas (O2)?
The balanced equation is 4Fe + 3O2 → 2Fe2O3. Using the molar mass of Fe2O3 (159.69 g/mol), the mass of Fe2O3 produced is 28.7 grams.
What is the limiting reactant when 10.0 grams of methane (CH4) reacts with 20.0 grams of oxygen (O2)?
The balanced equation is CH4 + 2O2 → CO2 + 2H2O. Calculating the moles of each reactant, methane is the limiting reactant.
What volume of carbon dioxide (CO2) is produced when 15.0 grams of calcium carbonate (CaCO3) is heated?
The balanced equation is CaCO3 → CaO + CO2. Using the molar volume of CO2 (22.4 L/mol), the volume of CO2 produced is 6.72 liters.
How many liters of hydrogen gas (H2) are produced when 25.0 grams of magnesium (Mg) reacts with an excess of hydrochloric acid (HCl)?
The balanced equation is 2Mg + 4HCl → 2MgCl2 + 2H2. Using the molar volume of H2 (22.4 L/mol), the volume of H2 produced is 13.4 liters.
What mass of sodium sulfate (Na2SO4) is produced when 25.0 grams of sodium hydroxide (NaOH) reacts with an excess of sulfuric acid (H2SO4)?
The balanced equation is 2NaOH + H2SO4 → Na2SO4 + 2H2O. Using the molar mass of Na2SO4 (142.04 g/mol), the mass of Na2SO4 produced is 35.5 grams.
What mass of water (H2O) is produced when 15.0 grams of methanol (CH3OH) is completely burned in oxygen (O2)?
The balanced equation is CH3OH + 3/2O2 → CO2 + 2H2O. Using the molar mass of H2O (18.02 g/mol), the mass of H2O produced is 12.0 grams.
How many grams of carbon dioxide (CO2) are produced when 15.0 grams of propane (C3H8) is completely burned in oxygen (O2)?
The balanced equation is C3H8 + 5O2 → 3CO2 + 4H2O. Using the molar mass of CO2 (44.01 g/mol), the mass of CO2 produced is 33.0 grams.
How many grams of iron (Fe) are produced when 50.0 grams of iron(III) oxide (Fe2O3) is reduced by hydrogen gas (H2)?
The balanced equation is Fe2O3 + 3H2 → 2Fe + 3H2O. Using the molar mass of Fe (55.85 g/mol), the mass of Fe produced is 35.0 grams.
What mass of copper(II) oxide (CuO) is required to react with 15.0 grams of aluminum (Al) to produce copper (Cu) and aluminum oxide (Al2O3)?
The balanced equation is 2Al + 3CuO → Al2O3 + 3Cu. Using the molar mass of CuO (79.55 g/mol), the mass of CuO required is 35.8 grams.8.
How many liters of carbon dioxide (CO2) are produced when 12.0 grams of calcium carbonate (CaCO3) is heated?
The balanced equation is CaCO3 → CaO + CO2. Using the molar volume of CO2 (22.4 L/mol), the volume of CO2 produced is 5.36 liters.
How many liters of carbon dioxide (CO2) are produced when 35.0 grams of calcium carbonate (CaCO3) reacts with an excess of hydrochloric acid (HCl)?
The balanced equation is CaCO3 + 2HCl → CaCl2 + CO2 + H2O. Using the molar volume of CO2 (22.4 L/mol), the volume of CO2 produced is 15.7 liters.
. What volume of oxygen gas (O2) is required to completely burn 10.0 grams of ethanol (C2H5OH)?
The balanced equation is C2H5OH + 3O2 → 2CO2 + 3H2O. Using the molar volume of O2 (22.4 L/mol), the volume of O2 required is 13.4 liters.
What volume of ammonia (NH3) is produced when 25.0 grams of nitrogen (N2) reacts with an excess of hydrogen gas (H2)?
The balanced equation is N2 + 3H2 → 2NH3. Using the molar volume of NH3 (22.4 L/mol), the volume of NH3 produced is 22.4 liters.
How many grams of carbon monoxide (CO) are produced when 20.0 grams of methane (CH4) is partially burned in oxygen (O2)?
The balanced equation is CH4 + 3/2O2 → CO + 2H2O. Using the molar mass of CO (28.01 g/mol), the mass of CO produced is 22.4 grams.
. How many grams of ammonia (NH3) are produced when 18.0 grams of nitrogen (N2) reacts with an excess of hydrogen gas (H2)?
The balanced equation is N2 + 3H2 → 2NH3. Using the molar mass of NH3 (17.03 g/mol), the mass of NH3 produced is 34.1 grams.
What mass of lead(II) sulfate (PbSO4) is produced when 28.0 grams of lead(II) nitrate (Pb(NO3)2) reacts with an excess of sodium sulfate (Na2SO4)?
The balanced equation is Pb(NO3)2 + Na2SO4 → PbSO4 + 2NaNO3. Using the molar mass of PbSO4 (303.26 g/mol), the mass of PbSO4 produced is 31.5 grams.