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1. Refer to Table 7.3 and calculate the mass of the sample of unknown that was heated by subtracting the mass of the empty test tube from the mass of the test tube and sample before heating. Record this mass in Table 7.4. 2. Calculate the mass of oxygen produced by the reaction by subtracting the mass of the test tube and sample after heating from the mass of the test tube and sample before heating. Record this mass in Table 7.4. 3. Note that the mass (in grams) of oxygen produced can be converted to moles by multiplying the mass by the following conversion factor: 1.00 mol 02 32.0 g O2 Convert the mass of oxygen produced that you calculated in Step 2 into moles of oxygen produced and record the number in Table 7.4. 4. According to Equation 7.2, the decomposition of 2 mol KCIOs produces 3 mol O2. Thus, the number of moles of KCIO, that were decomposed can be calculated by multiplying the number of moles of oxygen produced by the following conversion factor 2 mol KCIO 3 mol O2 Calculate the number of moles of KCIO, that were decomposed and record the value in Table 7.4. Note that this is the number of moles of solid KCIOs that were in the heated sample of unknown mixture. 5. Calculate the number of grams of KCIOs that were decomposed by multiplying the number of moles of KCIO, calculated in Step 4 by the following conversion factor: 123 8 KCI03 1.00 mol KCIOa Record the calculated mass of KCIO, decomposed in Table 7.4. 6. Use the mass of th e sample of unknown you calculated in Step 1 and the mass of KCIOs you calculated in Step 5 to calculate the percentage of KCIO, in the sample of unknown. This is done by using the following equation: % KClo, _ mass of KClO3 d (Eq. 7.3) unknown sample mass sample mass 100

1. Refer to Table 7.3 and calculate the mass of the sample of unknown that was heated by subtracting the mass of the empty test tube from the mass of the test tube and sample before heating. Record this mass in Table 7.4. 2. Calculate the mass of oxygen produced by the reaction by subtracting the mass of the test tube and sample after heating from the mass of the test tube and sample before heating. Record this mass in Table 7.4. 3. Note that the mass (in grams) of oxygen produced can be converted to moles by multiplying the mass by the following conversion factor: 1.00 mol 02 32.0 g O2 Convert the mass of oxygen produced that you calculated in Step 2 into moles of oxygen produced and record the number in Table 7.4. 4. According to Equation 7.2, the decomposition of 2 mol KCIOs produces 3 mol O2. Thus, the number of moles of KCIO, that were decomposed can be calculated by multiplying the number of moles of oxygen produced by the following conversion factor 2 mol KCIO 3 mol O2 Calculate the number of moles of KCIO, that were decomposed and record the value in Table 7.4. Note that this is the number of moles of solid KCIOs that were in the heated sample of unknown mixture. 5. Calculate the number of grams of KCIOs that were decomposed by multiplying the number of moles of KCIO, calculated in Step 4 by the following conversion factor: 123 8 KCI03 1.00 mol KCIOa Record the calculated mass of KCIO, decomposed in Table 7.4. 6. Use the mass of th e sample of unknown you calculated in Step 1 and the mass of KCIOs you calculated in Step 5 to calculate the percentage of KCIO, in the sample of unknown. This is done by using the following equation: % KClo, _ mass of KClO3 d (Eq. 7.3) unknown sample mass sample mass 100

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Chemistry
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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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Table 7.3 (data) Mass of empty test tube 7.568
  Mass of test tube and sample before heating  7.999
  mass of test tube and sample after heating 7.866
Table 7.4 (report)    
  Mass of unknown sample that was heated  
  Mass of oxygen produced  
  Moles of oxygen produced  
  Moles of KCIO3decomposed (moles of KCIO3 in sample)  
  Mass of KCIO3 Decomposed (mass of KCIO3 in sample)  
  Percentage of KCIO3 in sample  
     
1. Refer to Table 7.3 and calculate the mass of the sample of unknown that was heated by subtracting the mass of the empty test tube from the mass of the test tube and sample before heating. Record this mass in Table 7.4. 2. Calculate the mass of oxygen produced by the reaction by subtracting the mass of the test tube and sample after heating from the mass of the test tube and sample before heating. Record this mass in Table 7.4. 3. Note that the mass (in grams) of oxygen produced can be converted to moles by multiplying the mass by the following conversion factor: 1.00 mol 02 32.0 g O2 Convert the mass of oxygen produced that you calculated in Step 2 into moles of oxygen produced and record the number in Table 7.4. 4. According to Equation 7.2, the decomposition of 2 mol KCIOs produces 3 mol O2. Thus, the number of moles of KCIO, that were decomposed can be calculated by multiplying the number of moles of oxygen produced by the following conversion factor 2 mol KCIO 3 mol O2 Calculate the number of moles of KCIO, that were decomposed and record the value in Table 7.4. Note that this is the number of moles of solid KCIOs that were in the heated sample of unknown mixture. 5. Calculate the number of grams of KCIOs that were decomposed by multiplying the number of moles of KCIO, calculated in Step 4 by the following conversion factor: 123 8 KCI03 1.00 mol KCIOa Record the calculated mass of KCIO, decomposed in Table 7.4. 6. Use the mass of th e sample of unknown you calculated in Step 1 and the mass of KCIOs you calculated in Step 5 to calculate the percentage of KCIO, in the sample of unknown. This is done by using the following equation: % KClo, _ mass of KClO3 d (Eq. 7.3) unknown sample mass sample mass 100
Transcribed Image Text:1. Refer to Table 7.3 and calculate the mass of the sample of unknown that was heated by subtracting the mass of the empty test tube from the mass of the test tube and sample before heating. Record this mass in Table 7.4. 2. Calculate the mass of oxygen produced by the reaction by subtracting the mass of the test tube and sample after heating from the mass of the test tube and sample before heating. Record this mass in Table 7.4. 3. Note that the mass (in grams) of oxygen produced can be converted to moles by multiplying the mass by the following conversion factor: 1.00 mol 02 32.0 g O2 Convert the mass of oxygen produced that you calculated in Step 2 into moles of oxygen produced and record the number in Table 7.4. 4. According to Equation 7.2, the decomposition of 2 mol KCIOs produces 3 mol O2. Thus, the number of moles of KCIO, that were decomposed can be calculated by multiplying the number of moles of oxygen produced by the following conversion factor 2 mol KCIO 3 mol O2 Calculate the number of moles of KCIO, that were decomposed and record the value in Table 7.4. Note that this is the number of moles of solid KCIOs that were in the heated sample of unknown mixture. 5. Calculate the number of grams of KCIOs that were decomposed by multiplying the number of moles of KCIO, calculated in Step 4 by the following conversion factor: 123 8 KCI03 1.00 mol KCIOa Record the calculated mass of KCIO, decomposed in Table 7.4. 6. Use the mass of th e sample of unknown you calculated in Step 1 and the mass of KCIOs you calculated in Step 5 to calculate the percentage of KCIO, in the sample of unknown. This is done by using the following equation: % KClo, _ mass of KClO3 d (Eq. 7.3) unknown sample mass sample mass 100
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