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 10

A reaction has the equation: 2AgNO_3 + Cu \rightarrow Cu(NO_3)_2 + 2Ag. If 0.5 moles of Cu are used, how many moles of Ag are produced?

A reaction has the equation: 2C + O_2 \rightarrow 2CO. If 24 g of C reacts with 32 g of O_2, which is the limiting reactant? (C = 12 g/mol, O_2 = 32 g/mol)

A student burns 16 g of CH_4 in excess O_2 (CH_4 + 2O_2 \rightarrow CO_2 + 2H_2O). How many grams of CO_2 are produced? (CH_4 = 16 g/mol, CO_2 = 44 g/mol)

A student reacts 10 g of Fe with excess S according to Fe + S \rightarrow FeS. How many grams of FeS are produced? (Fe = 56 g/mol, S = 32 g/mol, FeS = 88 g/mol)

A student reacts 5.0 g of Ca with excess HCl according to the equation: Ca + 2HCl \rightarrow CaCl_2 + H_2. Calculate the mass of H_2 produced. (Ca = 40 g/mol, H_2 = 2 g/mol)

Describe the steps involved in calculating the mass of product formed from a given mass of reactant using a balanced chemical equation.

How many grams of NaCl are produced when 5.85 g of Na reacts with excess Cl_2 (2Na + Cl_2 \rightarrow 2NaCl)? (Na = 23 g/mol, NaCl = 58.5 g/mol)

How many molecules of CO_2 are produced when 0.5 moles of C_2H_6 are combusted according to: 2C_2H_6 + 7O_2 \rightarrow 4CO_2 + 6H_2O? (Avogadro's number = 6.02 \times 10^{23}))

If 0.25 moles of Mg react with excess HCl (Mg + 2HCl \rightarrow MgCl_2 + H_2), how many liters of H_2 gas at STP are produced? (1 mole gas at STP = 22.4 L)

If 10 g of H_2O are decomposed by electrolysis (2H_2O \rightarrow 2H_2 + O_2), how many grams of O_2 are formed? (H_2O = 18 g/mol, O_2 = 32 g/mol)

If 2.0 moles of Na react with excess Cl_2 according to 2Na + Cl_2 \rightarrow 2NaCl, how many moles of NaCl are formed?

If 3.0 moles of H_2 react with 2.0 moles of O_2 (2H_2 + O_2 \rightarrow 2H_2O), 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?

If the actual yield of a reaction is 8.0 g and the theoretical yield is 10.0 g, what is the percent yield?

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 g/mol)

In the reaction 2SO_2 + O_2 \rightarrow 2SO_3, how many liters of O_2 at STP are needed to react with 4.48 L of SO_2?

What is the mole ratio of H_2 to O_2 in the balanced equation: 2H_2 + O_2 \rightarrow 2H_2O?

A chemist wants to produce 100 g of water by reacting hydrogen and oxygen gases. The balanced equation is 2H_2 + O_2 \rightarrow 2H_2O. Calculate the minimum mass of O_2 required. (H_2O = 18 g/mol, O_2 = 32 g/mol)

A reaction has the equation: 2K + Br_2 \rightarrow 2KBr. If 19.6 g of K (K = 39.1 g/mol) are reacted with 80.0 g of Br_2 (Br_2 = 160 g/mol), what is the maximum mass of KBr (KBr = 119 g/mol) that can be formed?

A sample of calcium carbonate (CaCO_3) is heated according to the equation: CaCO_3 \rightarrow CaO + CO_2. If 50.0 g of CaCO_3 (CaCO_3 = 100 g/mol) is decomposed, calculate the volume of CO_2 gas produced at STP (1 mole gas = 22.4 L).