I don’t know how to do this Student Worksheet 5.4AExtra Practice Questions: Gravimetric StoichiometryComplete the following stoichiometric problems. All answers should be expressed to the correct.number of significant digits.1. Calculate the mass of iron(III) oxide (rust) produced by the reaction of 500 g of iron with oxygenfrom the air.2. What mass of precipitate should form if 2.00 g of silver nitrate in solution is reacted with excesssodium sulfide solution?3. Determine the mass of water vapor formed when 1.00 g of butane, C4H₁0), is burned in a lighter.4. Silver metal can be recovered from waste silver nitrate solutions by reaction with copper metal.What mass of silver can be obtained using 50 g of copper?-20 Unit 2 Lab and Study MastersCopyright 2002 Nelson Thomson Learning e Questioning HypothesizingPredictingPlanningConducting140 mL120100Student Worksheet for Lab Exercise 5.4.1Testing Gravimetric StoichiometryINQUIRY SKILLSRecordingAnalyzingEvaluatingCommunicatingure 1reacts with a solution of lead(II) nitrate.Unit 2 Lab and Study MastersThe most rigorous test of any scientific concept is whether or not it can be usedto make accurate predictions. If the prediction is shown to be valid, then theconcept is judged to be acceptable. If the percentage difference between theactual and the predicted values is considered to be too great (e.g., more than10%), then the concept may be judged unacceptable.The purpose of this lab exercise is to test the validity of the stoichiometricmethod. To do so, we will use the percentage difference between an experimentalvalue and the value predicted by gravimetric stoichiometry.Prepare a lab report to present your findings. Provide a Prediction of themass of lead produced in the single displacement reaction between zinc metaland aqueous lead (II) nitrate. In the Analysis of the evidence presented, answerthe question. In your Evaluation, evaluate the experimental design, the predic-tion, and the method of gravimetric stoichiometry.QuestionWhat is the mass of lead produced by the reaction of 2.13 g of zinc with an excessof lead(II) nitrate in solution (Figure 1)?Prediction(a) Write a balanced equation for the reaction.(b) Use the gravimetric stoichiometric method to predict the mass of leadproduced.Experimental DesignA known mass of zinc is placed in a beaker with an excess of lead (II) nitrate solu-tion. The lead produced in the reaction is separated by filtration and dried. Themass of the lead is determined. Assume that the reagents used are pure and that thetechnical skills used in carrying out the experiment are adequate for the experi-ment. An excess of one reactant is used to ensure the complete reaction of the lim-iting reagent.EvidenceIn the beaker, crystals of a shiny black solid were produced and all of the zincreacted.mass of filter paper = 0.92 gmass of dried filter paper plus lead = 7.60 gAnalysis(c) Use the evidence to calculate the actual mass of lead produced.(d) Calculate a percentage difference between the experimental value and thepredicted (theoretical) value of the mass of lead. The percentage differenceis calculated by dividing the difference in mass by the predicted mass.Evaluation(e) Why was an excess of lead (II) nitrate in solution used in this experiment?(f) How can we tell when the lead(II) nitrate is in excess?(g) Based on the evidence and your evaluation of the experimental design, isthe gravimetric stoichiometric method valid?Copyright © 2002 Nelson Thomson Learning

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I don’t know how to do this Student Worksheet 5.4AExtra Practice Questions: Gravimetric StoichiometryComplete the following stoichiometric problems. All answers should be expressed to the correct.number of significant digits.1. Calculate the mass of iron(III) oxide (rust) produced by the reaction of 500 g of iron with oxygenfrom the air.2. What mass of precipitate should form if 2.00 g of silver nitrate in solution is reacted with excesssodium sulfide solution?3. Determine the mass of water vapor formed when 1.00 g of butane, C4H₁0), is burned in a lighter.4. Silver metal can be recovered from waste silver nitrate solutions by reaction with copper metal.What mass of silver can be obtained using 50 g of copper?-20 Unit 2 Lab and Study MastersCopyright 2002 Nelson Thomson Learning e> Questioning> HypothesizingPredictingPlanningConducting140 mL120100Student Worksheet for Lab Exercise 5.4.1Testing Gravimetric StoichiometryINQUIRY SKILLSRecordingAnalyzingEvaluatingCommunicatingure 1reacts with a solution of lead(II) nitrate.Unit 2 Lab and Study MastersThe most rigorous test of any scientific concept is whether or not it can be usedto make accurate predictions. If the prediction is shown to be valid, then theconcept is judged to be acceptable. If the percentage difference between theactual and the predicted values is considered to be too great (e.g., more than10%), then the concept may be judged unacceptable.The purpose of this lab exercise is to test the validity of the stoichiometricmethod. To do so, we will use the percentage difference between an experimentalvalue and the value predicted by gravimetric stoichiometry.Prepare a lab report to present your findings. Provide a Prediction of themass of lead produced in the single displacement reaction between zinc metaland aqueous lead (II) nitrate. In the Analysis of the evidence presented, answerthe question. In your Evaluation, evaluate the experimental design, the predic-tion, and the method of gravimetric stoichiometry.QuestionWhat is the mass of lead produced by the reaction of 2.13 g of zinc with an excessof lead(II) nitrate in solution (Figure 1)?Prediction(a) Write a balanced equation for the reaction.(b) Use the gravimetric stoichiometric method to predict the mass of leadproduced.Experimental DesignA known mass of zinc is placed in a beaker with an excess of lead (II) nitrate solu-tion. The lead produced in the reaction is separated by filtration and dried. Themass of the lead is determined. Assume that the reagents used are pure and that thetechnical skills used in carrying out the experiment are adequate for the experi-ment. An excess of one reactant is used to ensure the complete reaction of the lim-iting reagent.EvidenceIn the beaker, crystals of a shiny black solid were produced and all of the zincreacted.mass of filter paper = 0.92 gmass of dried filter paper plus lead = 7.60 gAnalysis(c) Use the evidence to calculate the actual mass of lead produced.(d) Calculate a percentage difference between the experimental value and thepredicted (theoretical) value of the mass of lead. The percentage differenceis calculated by dividing the difference in mass by the predicted mass.Evaluation(e) Why was an excess of lead (II) nitrate in solution used in this experiment?(f) How can we tell when the lead(II) nitrate is in excess?(g) Based on the evidence and your evaluation of the experimental design, isthe gravimetric stoichiometric method valid?Copyright © 2002 Nelson Thomson Learning

Accepted Answer

Answers:-
1) Mass of iron oxide = 718.18 g
2) Mass of precipitate (Ag2S) = 1.45 g 
3) Mass of water…