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An aqueous solution containing 9.41 g of lead(II) nitrate is added to an aqueous solution containing 5.57 g of potassium chloride. Enter the balanced chemical equation for this reaction. Be sure to include all physical states. balanced chemical equation: What is the limiting reactant? potassium chloride lead(II) nitrate The percent yield for the reaction is 88.7%. How many grams of the precipitate are formed? precipitate formed: S

An aqueous solution containing 9.41 g of lead(II) nitrate is added to an aqueous solution containing 5.57 g of potassium chloride. Enter the balanced chemical equation for this reaction. Be sure to include all physical states. balanced chemical equation: What is the limiting reactant? potassium chloride lead(II) nitrate The percent yield for the reaction is 88.7%. How many grams of the precipitate are formed? precipitate formed: S

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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**Chemistry Exercise: Reaction of Lead(II) Nitrate and Potassium Chloride** An aqueous solution containing 9.41 g of lead(II) nitrate is added to an aqueous solution containing 5.57 g of potassium chloride. Follow the steps below to explore this chemical reaction. --- **Step 1:** Enter the balanced chemical equation for this reaction. Be sure to include all physical states. - **Balanced Chemical Equation:** [Text Box for Answer] **Step 2:** Determine the limiting reactant. - [ ] potassium chloride - [ ] lead(II) nitrate **Step 3:** Calculate the precipitate formed. The percent yield for the reaction is 88.7%. How many grams of the precipitate are formed? - **Precipitate Formed:** [Text Box for Answer] g **Step 4:** Calculate the excess reactant remaining. Taking into account the percent yield, how many grams of the excess reactant (the reactant that is not limiting) remain? - **Excess Reactant Remaining:** [Text Box for Answer] g --- This exercise will help you understand the concepts of stoichiometry, limiting reactants, and percent yield in chemical reactions.
Transcribed Image Text:**Chemistry Exercise: Reaction of Lead(II) Nitrate and Potassium Chloride** An aqueous solution containing 9.41 g of lead(II) nitrate is added to an aqueous solution containing 5.57 g of potassium chloride. Follow the steps below to explore this chemical reaction. --- **Step 1:** Enter the balanced chemical equation for this reaction. Be sure to include all physical states. - **Balanced Chemical Equation:** [Text Box for Answer] **Step 2:** Determine the limiting reactant. - [ ] potassium chloride - [ ] lead(II) nitrate **Step 3:** Calculate the precipitate formed. The percent yield for the reaction is 88.7%. How many grams of the precipitate are formed? - **Precipitate Formed:** [Text Box for Answer] g **Step 4:** Calculate the excess reactant remaining. Taking into account the percent yield, how many grams of the excess reactant (the reactant that is not limiting) remain? - **Excess Reactant Remaining:** [Text Box for Answer] g --- This exercise will help you understand the concepts of stoichiometry, limiting reactants, and percent yield in chemical reactions.
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we have to write the balanced equation for the reaction and calculate 

  • limiting reagent 
  • mass of precipitate formed 
  • mass of excess reactant 
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