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1 Student Worksheet 5.4A Extra Practice Questions: Gravimetric Stoichiometry Complete 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 oxygen from the air. 2. What mass of precipitate should form if 2.00 g of silver nitrate in solution is reacted with excess sodium sulfide solution? 3. Determine the mass of water vapor formed when 1.00 g of butane, C4H10g) 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?

1 Student Worksheet 5.4A Extra Practice Questions: Gravimetric Stoichiometry Complete 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 oxygen from the air. 2. What mass of precipitate should form if 2.00 g of silver nitrate in solution is reacted with excess sodium sulfide solution? 3. Determine the mass of water vapor formed when 1.00 g of butane, C4H10g) 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?

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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Student Worksheet 5.4A Extra Practice Questions: Gravimetric Stoichiometry Complete 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 oxygen from the air. 2. What mass of precipitate should form if 2.00 g of silver nitrate in solution is reacted with excess sodium 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 Masters Copyright 2002 Nelson Thomson Learning
Transcribed Image Text:Student Worksheet 5.4A Extra Practice Questions: Gravimetric Stoichiometry Complete 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 oxygen from the air. 2. What mass of precipitate should form if 2.00 g of silver nitrate in solution is reacted with excess sodium 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 Masters Copyright 2002 Nelson Thomson Learning
e > Questioning > Hypothesizing Predicting Planning Conducting 140 mL 120 100 Student Worksheet for Lab Exercise 5.4.1 Testing Gravimetric Stoichiometry INQUIRY SKILLS Recording Analyzing Evaluating Communicating ure 1 reacts with a solution of lead(II) nitrate. Unit 2 Lab and Study Masters The most rigorous test of any scientific concept is whether or not it can be used to make accurate predictions. If the prediction is shown to be valid, then the concept is judged to be acceptable. If the percentage difference between the actual and the predicted values is considered to be too great (e.g., more than 10%), then the concept may be judged unacceptable. The purpose of this lab exercise is to test the validity of the stoichiometric method. To do so, we will use the percentage difference between an experimental value and the value predicted by gravimetric stoichiometry. Prepare a lab report to present your findings. Provide a Prediction of the mass of lead produced in the single displacement reaction between zinc metal and aqueous lead (II) nitrate. In the Analysis of the evidence presented, answer the question. In your Evaluation, evaluate the experimental design, the predic- tion, and the method of gravimetric stoichiometry. Question What is the mass of lead produced by the reaction of 2.13 g of zinc with an excess of 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 lead produced. Experimental Design A 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. The mass of the lead is determined. Assume that the reagents used are pure and that the technical 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. Evidence In the beaker, crystals of a shiny black solid were produced and all of the zinc reacted. mass of filter paper = 0.92 g mass of dried filter paper plus lead = 7.60 g Analysis (c) Use the evidence to calculate the actual mass of lead produced. (d) Calculate a percentage difference between the experimental value and the predicted (theoretical) value of the mass of lead. The percentage difference is 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, is the gravimetric stoichiometric method valid? Copyright © 2002 Nelson Thomson Learning
Transcribed Image Text:e > Questioning > Hypothesizing Predicting Planning Conducting 140 mL 120 100 Student Worksheet for Lab Exercise 5.4.1 Testing Gravimetric Stoichiometry INQUIRY SKILLS Recording Analyzing Evaluating Communicating ure 1 reacts with a solution of lead(II) nitrate. Unit 2 Lab and Study Masters The most rigorous test of any scientific concept is whether or not it can be used to make accurate predictions. If the prediction is shown to be valid, then the concept is judged to be acceptable. If the percentage difference between the actual and the predicted values is considered to be too great (e.g., more than 10%), then the concept may be judged unacceptable. The purpose of this lab exercise is to test the validity of the stoichiometric method. To do so, we will use the percentage difference between an experimental value and the value predicted by gravimetric stoichiometry. Prepare a lab report to present your findings. Provide a Prediction of the mass of lead produced in the single displacement reaction between zinc metal and aqueous lead (II) nitrate. In the Analysis of the evidence presented, answer the question. In your Evaluation, evaluate the experimental design, the predic- tion, and the method of gravimetric stoichiometry. Question What is the mass of lead produced by the reaction of 2.13 g of zinc with an excess of 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 lead produced. Experimental Design A 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. The mass of the lead is determined. Assume that the reagents used are pure and that the technical 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. Evidence In the beaker, crystals of a shiny black solid were produced and all of the zinc reacted. mass of filter paper = 0.92 g mass of dried filter paper plus lead = 7.60 g Analysis (c) Use the evidence to calculate the actual mass of lead produced. (d) Calculate a percentage difference between the experimental value and the predicted (theoretical) value of the mass of lead. The percentage difference is 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, is the gravimetric stoichiometric method valid? Copyright © 2002 Nelson Thomson Learning
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