Stoichiometric Calculations Using Chemical Equations

Chemistry ⇒ Stoichiometry and Chemical Calculations

Stoichiometric Calculations Using Chemical Equations starts at 10 and continues till grade 12. QuestionsToday has an evolving set of questions to continuously challenge students so that their knowledge grows in Stoichiometric Calculations Using Chemical Equations. How you perform is determined by your score and the time you take. When you play a quiz, your answers are evaluated in concept instead of actual words and definitions used.

See sample questions for grade 12

A mixture contains 5.0 g of H_2 and 32.0 g of O_2. How many grams of H_2O can be formed? (2H_2 + O_2 \rightarrow 2H_2O; Molar mass H_2 = 2.0 g/mol, O_2 = 32.0 g/mol, H_2O = 18.0 g/mol)

A reaction has a percent yield of 80%. If the theoretical yield is 50 g, what is the actual yield?

A reaction mixture contains 0.25 mol of A and 0.40 mol of B. The balanced equation is A + 2B \rightarrow C. What is the maximum number of moles of C that can be formed?

A reaction produces 15.0 g of product, but the theoretical yield is 20.0 g. What is the percent yield?

A sample of 5.0 g of Mg reacts with excess HCl. How many liters of H_2 gas at STP are produced? (Mg + 2HCl \rightarrow MgCl_2 + H_2; Molar mass Mg = 24.3 g/mol)

A student reacts 10.0 g of Ca with 20.0 g of Cl_2 to form CaCl_2 according to the equation: Ca + Cl_2 \rightarrow CaCl_2. Which is the limiting reactant? (Molar masses: Ca = 40.1 g/mol, Cl_2 = 70.9 g/mol)

Calculate the number of moles of AgNO_3 required to completely react with 0.5 moles of NaCl in the reaction: AgNO_3 + NaCl \rightarrow AgCl + NaNO_3.

Describe the steps involved in determining the limiting reactant in a chemical reaction.

How many grams of CO_2 are produced from 10.0 g of C_6H_{12}O_6 in the reaction: C_6H_{12}O_6 \rightarrow 2C_2H_5OH + 2CO_2? (Molar mass C_6H_{12}O_6 = 180.0 g/mol, CO_2 = 44.0 g/mol)

How many grams of NaCl are produced when 2.0 moles of Na react with excess Cl_2? (2Na + Cl_2 \rightarrow 2NaCl; Molar mass NaCl = 58.5 g/mol)

How many liters of CO_2 at STP are produced from 10.0 g of CaCO_3? (CaCO_3 \rightarrow CaO + CO_2; Molar mass CaCO_3 = 100.1 g/mol; 1 mol gas at STP = 22.4 L)

How many moles of CO_2 are produced when 5 moles of C_2H_6 combust completely? (C_2H_6 + 3.5O_2 \rightarrow 2CO_2 + 3H_2O)

How many moles of H_2O are produced when 3 moles of O_2 react with excess H_2? (2H_2 + O_2 \rightarrow 2H_2O)

How many moles of O_2 are needed to completely combust 4 moles of C_2H_6? (2C_2H_6 + 7O_2 \rightarrow 4CO_2 + 6H_2O)

If 2.0 moles of H_2 react with excess O_2, how many grams of H_2O are formed? (2H_2 + O_2 \rightarrow 2H_2O; Molar mass H_2O = 18.0 g/mol)

If 3.0 moles of Fe react with 2.0 moles of O_2 to form Fe_2O_3 (4Fe + 3O_2 \rightarrow 2Fe_2O_3), what is the limiting reactant?

If 4 moles of NH_3 are produced from the reaction N_2 + 3H_2 \rightarrow 2NH_3, how many moles of H_2 are required?

In the reaction 2C + O_2 \rightarrow 2CO, if 24 g of C reacts with 64 g of O_2, what is the limiting reactant? (Molar mass C = 12.0 g/mol, O_2 = 32.0 g/mol)

In the reaction 2KClO_3 \rightarrow 2KCl + 3O_2, how many grams of O_2 are produced from 12.25 g of KClO_3? (Molar mass: KClO_3 = 122.5 g/mol, O_2 = 32.0 g/mol)

In the reaction 2Na + 2H_2O \rightarrow 2NaOH + H_2, how many grams of NaOH are produced from 4.6 g of Na? (Molar mass Na = 23.0 g/mol, NaOH = 40.0 g/mol)