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You may either copy the table onto your pre-lab assignment, or you may write your answers in the table and turn in this sheet as part of your assignment. 1. Briefly describe three general safety rules for working with a Bunsen burner. 2. The following data were obtained when a sample of barium chloride hydrate was analyzed as described in the Procedure section Mass of empty test tube Mass of test tube and hydrate (before heating) Mass of test tube and anhydrous salt (after heating) 18.42 g 20.75 g 20.41 g Calculate (a) the original mass of the hydrate, (b) the mass of water lost upon heating and (c) the experimental percent water in the hydrate. 3. As shown in the table below, the general formula of barium chloride hydrate is BaCl, nH;O, where n is the number of water molecules. Complete the table, and calculate the theoretical percent water in the hydrate. Note that BaCl, is not a hydrate; it is simply the anhydrous salt.

You may either copy the table onto your pre-lab assignment, or you may write your answers in the table and turn in this sheet as part of your assignment. 1. Briefly describe three general safety rules for working with a Bunsen burner. 2. The following data were obtained when a sample of barium chloride hydrate was analyzed as described in the Procedure section Mass of empty test tube Mass of test tube and hydrate (before heating) Mass of test tube and anhydrous salt (after heating) 18.42 g 20.75 g 20.41 g Calculate (a) the original mass of the hydrate, (b) the mass of water lost upon heating and (c) the experimental percent water in the hydrate. 3. As shown in the table below, the general formula of barium chloride hydrate is BaCl, nH;O, where n is the number of water molecules. Complete the table, and calculate the theoretical percent water in the hydrate. Note that BaCl, is not a hydrate; it is simply the anhydrous salt.

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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I need help with question number two listed on the file attached. 

You may either copy the table onto your pre-lab assignment, or you may write your answers in the table and turn in this sheet as part of your assignment. 1. Briefly describe three general safety rules for working with a Bunsen burner. 2. The following data were obtained when a sample of barium chloride hydrate was analyzed as described in the Procedure section Mass of empty test tube Mass of test tube and hydrate (before heating) Mass of test tube and anhydrous salt (after heating) 18.42 g 20.75 g 20.41 g Calculate (a) the original mass of the hydrate, (b) the mass of water lost upon heating and (c) the experimental percent water in the hydrate. 3. As shown in the table below, the general formula of barium chloride hydrate is BaCl, nH;O, where n is the number of water molecules. Complete the table, and calculate the theoretical percent water in the hydrate. Note that BaCl, is not a hydrate; it is simply the anhydrous salt.
Transcribed Image Text:You may either copy the table onto your pre-lab assignment, or you may write your answers in the table and turn in this sheet as part of your assignment. 1. Briefly describe three general safety rules for working with a Bunsen burner. 2. The following data were obtained when a sample of barium chloride hydrate was analyzed as described in the Procedure section Mass of empty test tube Mass of test tube and hydrate (before heating) Mass of test tube and anhydrous salt (after heating) 18.42 g 20.75 g 20.41 g Calculate (a) the original mass of the hydrate, (b) the mass of water lost upon heating and (c) the experimental percent water in the hydrate. 3. As shown in the table below, the general formula of barium chloride hydrate is BaCl, nH;O, where n is the number of water molecules. Complete the table, and calculate the theoretical percent water in the hydrate. Note that BaCl, is not a hydrate; it is simply the anhydrous salt.
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