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Calculate the empirical formula of the alum. Show (URGENT NEED HELP FAST) calculations for moles a hydrate and moles water. Chart is second photo and can be used for reference.

Calculate the empirical formula of the alum. Show (URGENT NEED HELP FAST) calculations for moles a hydrate and moles water. Chart is second photo and can be used for reference.

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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Calculate the empirical formula of the alum. Show (URGENT NEED HELP FAST) calculations for moles a hydrate and moles water. Chart is second photo and can be used for reference.
**Calculating the Empirical Formula of Alum** To determine the empirical formula of the alum, follow the procedure outlined in Example 1. Ensure you show your calculations for Trial 1. - **Moles Anhydrate**: (Note: The molar mass of \( \text{KAl(SO}_4\text{)}_2 \) is 258.21 g/mol) _[Space for input of calculated moles]_ - **Moles Water**: _[Space for input of calculated moles]_ **Results**: - **Trial 1**: \( \text{KAl(SO}_4\text{)}_2 \cdot \_\_ \text{H}_2\text{O} \) - **Trial 2**: \( \text{KAl(SO}_4\text{)}_2 \cdot \_\_ \text{H}_2\text{O} \) *150 – Report Sheet*
Transcribed Image Text:**Calculating the Empirical Formula of Alum** To determine the empirical formula of the alum, follow the procedure outlined in Example 1. Ensure you show your calculations for Trial 1. - **Moles Anhydrate**: (Note: The molar mass of \( \text{KAl(SO}_4\text{)}_2 \) is 258.21 g/mol) _[Space for input of calculated moles]_ - **Moles Water**: _[Space for input of calculated moles]_ **Results**: - **Trial 1**: \( \text{KAl(SO}_4\text{)}_2 \cdot \_\_ \text{H}_2\text{O} \) - **Trial 2**: \( \text{KAl(SO}_4\text{)}_2 \cdot \_\_ \text{H}_2\text{O} \) *150 – Report Sheet*
**Empirical Formula of Alum** 1. **Mass of beaker plus alum, \( \text{KAl(SO}_4\text{)}_2 \cdot x\text{H}_2\text{O} \):** - Trial 1: 50.249 g - Trial 2: 57.925 g 2. **Mass of beaker:** - Trial 1: 48.973 g - Trial 2: 56.446 g 3. **Mass of alum:** - Trial 1: 1.276 g - Trial 2: 1.479 g 4. **Mass of beaker plus anhydrate:** - Trial 1: 49.665 g - Trial 2: 57.254 g 5. **Mass of anhydrate, \( \text{KAl(SO}_4\text{)}_2 \):** - Trial 1: 0.692 g - Trial 2: 0.808 g 6. **Mass of water:** - Trial 1: 0.584 g - Trial 2: 0.671 g Calculate the empirical formula of the alum as shown in Example 1. Show your calculation for Trial 1.
Transcribed Image Text:**Empirical Formula of Alum** 1. **Mass of beaker plus alum, \( \text{KAl(SO}_4\text{)}_2 \cdot x\text{H}_2\text{O} \):** - Trial 1: 50.249 g - Trial 2: 57.925 g 2. **Mass of beaker:** - Trial 1: 48.973 g - Trial 2: 56.446 g 3. **Mass of alum:** - Trial 1: 1.276 g - Trial 2: 1.479 g 4. **Mass of beaker plus anhydrate:** - Trial 1: 49.665 g - Trial 2: 57.254 g 5. **Mass of anhydrate, \( \text{KAl(SO}_4\text{)}_2 \):** - Trial 1: 0.692 g - Trial 2: 0.808 g 6. **Mass of water:** - Trial 1: 0.584 g - Trial 2: 0.671 g Calculate the empirical formula of the alum as shown in Example 1. Show your calculation for Trial 1.
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