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a. How many moles of carbon tetrachloride, CC14, are present in a sample that contains 6.30 moles of chlorine atoms? |mol CCl4 b. How many moles of chlorine atoms are present in a sample that contains 4.95 moles of CCL4? mol Cl

a. How many moles of carbon tetrachloride, CC14, are present in a sample that contains 6.30 moles of chlorine atoms? |mol CCl4 b. How many moles of chlorine atoms are present in a sample that contains 4.95 moles of CCL4? mol Cl

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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### Chemistry Problems: Moles and Chemical Compounds #### Problem a: **Question:** How many moles of carbon tetrachloride, \( \text{CCl}_4 \), are present in a sample that contains 6.30 moles of chlorine atoms? **Blank Input:** \_\_\_\_\_ mol \( \text{CCl}_4 \) #### Problem b: **Question:** How many moles of chlorine atoms are present in a sample that contains 4.95 moles of \( \text{CCl}_4 \)? **Blank Input:** \_\_\_\_\_ mol Cl
Transcribed Image Text:### Chemistry Problems: Moles and Chemical Compounds #### Problem a: **Question:** How many moles of carbon tetrachloride, \( \text{CCl}_4 \), are present in a sample that contains 6.30 moles of chlorine atoms? **Blank Input:** \_\_\_\_\_ mol \( \text{CCl}_4 \) #### Problem b: **Question:** How many moles of chlorine atoms are present in a sample that contains 4.95 moles of \( \text{CCl}_4 \)? **Blank Input:** \_\_\_\_\_ mol Cl
## Calculating the Molar Mass of Sulfur Tetrafluoride (SF₄) Use the References to access important values if needed for this question. ### Instructions: Complete the table below for calculating the molar mass of the compound sulfur tetrafluoride. | Molar Mass of Element | Moles | Mass in One Mole of Sulfur Tetrafluoride | |-----------------------|-------|------------------------------------------| | S | [____] g/mol | × [____] mol = [_____ ] g | | F | [____] g/mol | × [____] mol = [_____ ] g | ### Total Molar Mass Calculation: \[ \text{Molar mass of sulfur tetrafluoride} = \boxed{\underline{\text{_______}}} \text{ g/mol} \] ### Explanation of Tables and Calculations: 1. **Molar Mass of Element:** - This column is for entering the molar masses of the elements sulfur (S) and fluorine (F). You can find these values in a periodic table or reference material. 2. **Moles:** - This column is for entering the number of moles of each element in one mole of sulfur tetrafluoride (SF₄). For sulfur tetrafluoride, there is 1 mole of sulfur and 4 moles of fluorine. 3. **Mass in One Mole of Sulfur Tetrafluoride:** - Multiply the molar mass of each element by the number of moles to find the contribution of each element to the total molar mass of sulfur tetrafluoride. ### Example Calculation: - Suppose you have the molar mass of sulfur (S) as 32.07 g/mol and the molar mass of fluorine (F) as 19.00 g/mol. Then the table would be filled out as follows: | Molar Mass of Element | Moles | Mass in One Mole of Sulfur Tetrafluoride | |-----------------------|-------|------------------------------------------| | S (32.07 g/mol) | × 1 mol | = 32.07 g | | F (19.00 g/mol) | × 4 mol | = 76.00 g | The total molar mass of sulfur tetrafluoride can then be calculated by summing the individual masses: \[ 32.07 \, \text{
Transcribed Image Text:## Calculating the Molar Mass of Sulfur Tetrafluoride (SF₄) Use the References to access important values if needed for this question. ### Instructions: Complete the table below for calculating the molar mass of the compound sulfur tetrafluoride. | Molar Mass of Element | Moles | Mass in One Mole of Sulfur Tetrafluoride | |-----------------------|-------|------------------------------------------| | S | [____] g/mol | × [____] mol = [_____ ] g | | F | [____] g/mol | × [____] mol = [_____ ] g | ### Total Molar Mass Calculation: \[ \text{Molar mass of sulfur tetrafluoride} = \boxed{\underline{\text{_______}}} \text{ g/mol} \] ### Explanation of Tables and Calculations: 1. **Molar Mass of Element:** - This column is for entering the molar masses of the elements sulfur (S) and fluorine (F). You can find these values in a periodic table or reference material. 2. **Moles:** - This column is for entering the number of moles of each element in one mole of sulfur tetrafluoride (SF₄). For sulfur tetrafluoride, there is 1 mole of sulfur and 4 moles of fluorine. 3. **Mass in One Mole of Sulfur Tetrafluoride:** - Multiply the molar mass of each element by the number of moles to find the contribution of each element to the total molar mass of sulfur tetrafluoride. ### Example Calculation: - Suppose you have the molar mass of sulfur (S) as 32.07 g/mol and the molar mass of fluorine (F) as 19.00 g/mol. Then the table would be filled out as follows: | Molar Mass of Element | Moles | Mass in One Mole of Sulfur Tetrafluoride | |-----------------------|-------|------------------------------------------| | S (32.07 g/mol) | × 1 mol | = 32.07 g | | F (19.00 g/mol) | × 4 mol | = 76.00 g | The total molar mass of sulfur tetrafluoride can then be calculated by summing the individual masses: \[ 32.07 \, \text{
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