Example 3.18 - Calculating Percent Yield (1)Example 3.18 - Calculating Percent Yield (2)Student Exercises - Stoichiometry (1) – (MOD)Student Exercises – Stoichiometry (1) – (MOD)Student Exercises - Stoichiometry (2) – (MOD)Student Exercises – Stoichiometry (2) – (MOD)Student Exercises - Stoichiometry (3) – (MOD)Student Exercises – Stoichiometry (3) – (MOD)Student Exercises - Stoichiometry (4) – (MOD)Student Exercises – Stoichiometry (4) – (MOD)Section 3.11The Concept of Limiting ReactantCopyright ©2018 Cengage Learning. All Rights Reserved.Example 3.18 - Calculating Percent Yield (1)Taylor prepares silver chloride by the following reaction. 2 AgNO3 (aq) + CaCl2 (aq)  2 AgCl (s) + Ca(NO3)2 (aq). If 17.54 g of CaCl2 is mixed with excess AgNO3 in solution, and Taylor gets 29.11 g of AgCl product, calculate Taylor’s percent yield.Section 3.11The Concept of Limiting ReactantCopyright ©2018 Cengage Learning. All Rights Reserved.Example 3.18 - Calculating Percent Yield (2)Section 3.11The Concept of Limiting ReactantCopyright ©2018 Cengage Learning. All Rights Reserved.Student Exercises - Stoichiometry (1) – (MOD)Water can be produced by the following reaction 2 H2 (g) + O2 (g)  2 H2O (ℓ). If we need to make 45.23 g of water, how many grams of O2 do we need and how many grams of H2 do we need?Section 3.11The Concept of Limiting ReactantCopyright ©2018 Cengage Learning. All Rights Reserved.Student Exercises – Stoichiometry (1) – (MOD)Section 3.11The Concept of Limiting ReactantCopyright ©2018 Cengage Learning. All Rights Reserved.Student Exercises - Stoichiometry (2) – (MOD)In the Haber process, N2 (g) + 3 H2 (g)  2 NH3 (g).If 3.50 mol of N2 and 7.50 mol of H2 react, how much NH3 can theoretically be produced? If this is a limiting reactant problem, determined the moles of excess reactant remaining.Section 3.11The Concept of Limiting ReactantCopyright ©2018 Cengage Learning. All Rights Reserved.Student Exercises – Stoichiometry (2) – (MOD)Section 3.11The Concept of Limiting ReactantCopyright ©2018 Cengage Learning. All Rights Reserved.Student Exercises - Stoichiometry (3) – (MOD)For the chemical reaction NaOH (s) + CO2 (g)  Na2CO3 (s) + H2O (ℓ), a 2.536 g pellet of NaOH absorbs a stoichiometric amount of CO2. What is the mass of the pellet after the CO2 is absorbed?Section 3.11The Concept of Limiting ReactantCopyright ©2018 Cengage Learning. All Rights Reserved.Student Exercises – Stoichiometry (3) – (MOD)Section 3.11The Concept of Limiting ReactantCopyright ©2018 Cengage Learning. All Rights Reserved.Student Exercises - Stoichiometry (4) – (MOD)A student wishes to prepare Cu by reacting CuCl2 with Al metal. The reaction is CuCl2 (aq) + Al (s)  AlCl3 (aq) + Cu (s). The student dissolves 8.532 g of CuCl2 in 150 mL of water, then adds 3.546 g of Al. The student actually produces 2.143 g of Cu. Calculate the percent yield.Section 3.11The Concept of Limiting ReactantCopyright ©2018 Cengage Learning. All Rights Reserved.Student Exercises – Stoichiometry (4) –