Quantitative Relationships in Chemical Changes

Reading a balanced equation as a recipe: moles, masses, limiting reagents and yield.

16 questions, free, marked as you go with a worked explanation on every one.

What this covers

What is the molar mass of carbon dioxide, CO₂? Use C = 12.01 and O = 16.00 g/mol.
How many moles are there in 88.02 g of carbon dioxide?
For the reaction 2H₂ + O₂ → 2H₂O, how many moles of oxygen are needed to react completely with 6.0 mol of hydrogen?
For 2H₂ + O₂ → 2H₂O, what mass of water is produced from 2.0 mol of hydrogen? Use H = 1.01 and O = 16.00 g/mol.
For 2H₂ + O₂ → 2H₂O, you start with 4.0 mol H₂ and 3.0 mol O₂. How many moles of water can form?
A reaction should theoretically produce 10.0 g of product, but only 8.5 g is collected. What is the percent yield?
What does it mean for a reactant to be the limiting reagent?
What does a balanced chemical equation tell you? Select all that apply.
Why must a chemical equation be balanced before it is used for calculations?
Use the table. How many moles of the NaCl sample are there?
Balance the equation by counting atoms: __Mg + __O₂ → __MgO. What coefficient goes in front of MgO?
Which coefficients correctly balance: __N₂ + __H₂ → __NH₃?
In the reaction 2H₂ + O₂ → 2H₂O, how many moles of H₂ are needed to react completely with 3 moles of O₂?
In the reaction N₂ + 3H₂ → 2NH₃, if 5 moles of N₂ react completely, how many moles of NH₃ are produced?
Balance the equation: C3H8 + O2 -> CO2 + H2O. What coefficient belongs in front of O2?
Balance the equation: KClO3 -> KCl + O2. What coefficient belongs in front of O2?