NUMBER OF MOLES/MOLE RATIO
What is the mole ratio of water to glucose (C6H12O6) in the chemical equation for cellular respiration?
C6H12O6 + 6O2 -> 6CO2 + 6H2O
What is the mass of 0.5 moles of sodium chloride (NaCl)?
The molar mass of NaCl is 58.44 g/mol.
If 10 g of copper is reacted with excess sulfuric acid (H2SO4) to produce copper(II) sulfate (CuSO4) according to the balanced chemical equation, what is the theoretical yield of CuSO4 in grams? If the actual yield of CuSO4 obtained in the lab is 8 g, what is the percentage yield of CuSO4 for the reaction?
Cu + 2H2SO4 -> CuSO4 + 2H2O
The molar masses are: Cu = 63.55 g/mol H2SO4 = 98.08 g/mol CuSO4 = 159.61 g/mol
Question: Balance the following chemical equation: Fe2O3 + CO -> Fe + CO2
The balanced chemical equation is: 2 Fe2O3 + 3 CO -> 4 Fe + 3 CO2
The question was: How many grams of sulfur are required to react completely with 33.8 grams of zinc according to the equation Zn + S → ZnS ?
The answer is 16.57 grams of sulfur are required.
How many moles of oxygen gas (O2) are needed to react completely with 8 moles of propane (C3H8) in the combustion reaction
C3H8 + 5O2 -> 3CO2 + 4H2O?
What mass of potassium nitrate (KNO3) is needed to make 0.2 moles of nitrogen gas (N2) according to the following balanced equation? 2KNO3 -> 2KNO2 + O2 + N2
KNO3 = 101.11 g/mol N2 = 28.02 g/mol
You react 10.0 g of magnesium with 50.0 mL of 1.0 M hydrochloric acid (HCl) according to the balanced equation: Mg + 2HCl -> MgCl2 + H2 What is the limiting reagent and what mass of hydrogen gas (H2) can be produced? If the actual yield of H2 obtained in the lab is 0.50 g, what is the percentage yield of H2 for the reaction?
The molar masses are: Mg = 24.31 g/mol HCl = 36.46 g/mol MgCl2 = 95.21 g/mol H2 = 2.02 g/mol
Balance the following chemical equation: C3H8 + O2 -> CO2 + H2O
The balanced chemical equation is: C3H8 + 5 O2 -> 3 CO2 + 4 H2O
The question was: How many grams of CaCO3 are needed to produce 44.8 grams of CO2 according to the equation CaCO3 → CaO + CO2 ?
The answer is 67.20 grams of CaCO3 are needed.
If 0.25 moles of calcium chloride (CaCl2) react with 0.20 moles of sodium carbonate (Na2CO3), how many moles of calcium carbonate (CaCO3) will be produced in the following balanced chemical equation?
CaCl2 + Na2CO3 → CaCO3 + 2NaCl
What mass of sodium chloride (NaCl) is needed to react completely with 0.5 moles of silver nitrate (AgNO3) to form solid silver chloride (AgCl) and aqueous sodium nitrate (NaNO3)? AgNO3 + NaCl → AgCl + NaNO3
AgNO3 = 169.87 g/mol NaCl = 58.44 g/mol AgCl = 143.32 g/mo
In an experiment, you start with 0.50 g of benzene (C6H6) and react it with excess nitric acid (HNO3) to produce 0.65 g of nitrobenzene. What is the percentage yield of nitrobenzene? C6H6 + HNO3 --> C6H5NO2 + H2O
The molar masses are: C6H6 = 78.11 g/mol HNO3 = 63.01 g/mol C6H5NO2 = 123.11 g/mol
Balance the following chemical equation: KClO3 -> KCl + O2
The balanced chemical equation is: 2 KClO3 -> 2 KCl + 3 O2
A certain compound has a molar mass of 60.05 g/mol and contains only carbon, hydrogen, and oxygen. A 0.6625 g sample of the compound is burned in excess oxygen, producing 1.747 g of CO2 and 0.7164 g of H2O. What is the empirical formula of the compound?
C3.5H7O2
In the reaction between hydrogen gas (H2) and nitrogen gas (N2) to form ammonia gas (NH3), what is the maximum mass of NH3 that could be produced if you start with 10 g of H2 and 50 g of N2?
3H2 + N2 → 2NH3
Hydrogen peroxide (H2O2) decomposes into water (H2O) and oxygen gas (O2). If 50.0 g of H2O2 is decomposed to produce water and oxygen gas according to the balanced chemical equation, what is the mass of oxygen gas produced? 2H2O2 -> 2H2O + O2
The molar mass of H2O2 is 34.01 g/mol and the molar mass of O2 is 32.00 g/mol.
In an experiment, you prepare a solution by dissolving 15 g of potassium chloride (KCl) in 50 mL of water. What is the concentration of this solution in molarity?
The molar mass of KCl is 74.55 g/mol.
Balance the following chemical equation: NaOH + H3PO4 -> Na3PO4 + H2O
The balanced chemical equation is: 3 NaOH + H3PO4 -> Na3PO4 + 3 H2O
What is the percent yield of a reaction if 8.75 g of product was obtained when 10.00 g of reactant was used and the theoretical yield is 12.50 g?
Percent Yield = (Actual yield / Theoretical yield) x 100%
In the Haber process, nitrogen gas (N2) and hydrogen gas (H2) react to form ammonia gas (NH3). If 50.0 g of N2 reacts with an excess of H2 to form 30.0 g of NH3, what is the percent yield of NH3 for the reaction?
N2 + 3H2 → 2NH3
What mass of calcium chloride (CaCl2) is needed to react completely with 75.0 g of sodium carbonate (Na2CO3) to form calcium carbonate (CaCO3) and aqueous sodium chloride (NaCl) according to the balanced chemical equation? CaCl2 + Na2CO3 -> CaCO3 + 2NaCl
CaCl2 = 110.98 g/mol Na2CO3 = 105.99 g/mol CaCO3 = 100.09 g/mol
In a chemical reaction, 1.25 g of a reactant A is mixed with 25.0 ml of a solution containing 0.75 M of reactant B. The reaction is expected to produce 2.50 g of product P, but the actual yield is only 1.80 g. What is the limiting reactant in this reaction and what is the percentage yield of the product, taking into account the initial concentration of reactant B?
The limiting reactant is B and the percentage yield of product P, taking into account the initial concentration of reactant B, is 138.3%.
Balance the following chemical equation: C8H18 + O2 -> CO2 + H2O
The balanced chemical equation is: 2 C8H18 + 25 O
What is the molarity of a solution that contains 8.50 g of NaOH dissolved in 750 mL of solution?
the molarity of the solution is 0.2833 mol/L.