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Ascorbic acid (C,H3O6) is also known as Vitamin C. How many molecules of C6H;O6 does a Vitamin C drink with 1.000 × 10³ mg CH¿O6 contain?

Ascorbic acid (C,H3O6) is also known as Vitamin C. How many molecules of C6H;O6 does a Vitamin C drink with 1.000 × 10³ mg CH¿O6 contain?

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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**Calculating the Number of Molecules in Vitamin C (Ascorbic Acid)** Ascorbic acid (\( \text{C}_6\text{H}_8\text{O}_6 \)) is commonly known as Vitamin C. To determine how many molecules of \(\text{C}_6\text{H}_8\text{O}_6\) are present in a Vitamin C drink containing \(1.000 \times 10^3\) mg of \(\text{C}_6\text{H}_8\text{O}_6\), we will perform the following calculations. ### Steps for Calculation 1. **Starting Amount:** - The given mass is \(1.000 \times 10^3\) mg of \(\text{C}_6\text{H}_8\text{O}_6\). 2. **Convert Milligrams to Grams:** - Since \(1 \text{ g} = 1000 \text{ mg}\), \(1.000 \times 10^3 \text{ mg} = 1 \text{ g}\). 3. **Determine Moles of \(\text{C}_6\text{H}_8\text{O}_6\):** - The molar mass of \(\text{C}_6\text{H}_8\text{O}_6\) is 176.12 g/mol. - Moles = \( \frac{1 \text{ g}}{176.12 \text{ g/mol}} \). 4. **Calculate Number of Molecules:** - Use Avogadro's number, \(6.022 \times 10^{23} \text{ molecules/mol}\). - Number of molecules = Moles \( \times 6.022 \times 10^{23} \text{ molecules/mol}\). ### Diagram Explanation - **Starting Amount Box:** Input for initial quantity. - **Multiplication and Division Formula:** Assists in organizing conversion steps. - **Buttons for Operations:** Add factor \( \times (\hspace{2mm}) \), Delete, Answer, and Reset. - **Constants and Values:** Buttons for frequently used constants (like molar mass and Avogadro's number). ### Note Accurate calculations are crucial in determining molecular quantities to understand the chemical composition effectively. This process is essential in chemistry education
Transcribed Image Text:**Calculating the Number of Molecules in Vitamin C (Ascorbic Acid)** Ascorbic acid (\( \text{C}_6\text{H}_8\text{O}_6 \)) is commonly known as Vitamin C. To determine how many molecules of \(\text{C}_6\text{H}_8\text{O}_6\) are present in a Vitamin C drink containing \(1.000 \times 10^3\) mg of \(\text{C}_6\text{H}_8\text{O}_6\), we will perform the following calculations. ### Steps for Calculation 1. **Starting Amount:** - The given mass is \(1.000 \times 10^3\) mg of \(\text{C}_6\text{H}_8\text{O}_6\). 2. **Convert Milligrams to Grams:** - Since \(1 \text{ g} = 1000 \text{ mg}\), \(1.000 \times 10^3 \text{ mg} = 1 \text{ g}\). 3. **Determine Moles of \(\text{C}_6\text{H}_8\text{O}_6\):** - The molar mass of \(\text{C}_6\text{H}_8\text{O}_6\) is 176.12 g/mol. - Moles = \( \frac{1 \text{ g}}{176.12 \text{ g/mol}} \). 4. **Calculate Number of Molecules:** - Use Avogadro's number, \(6.022 \times 10^{23} \text{ molecules/mol}\). - Number of molecules = Moles \( \times 6.022 \times 10^{23} \text{ molecules/mol}\). ### Diagram Explanation - **Starting Amount Box:** Input for initial quantity. - **Multiplication and Division Formula:** Assists in organizing conversion steps. - **Buttons for Operations:** Add factor \( \times (\hspace{2mm}) \), Delete, Answer, and Reset. - **Constants and Values:** Buttons for frequently used constants (like molar mass and Avogadro's number). ### Note Accurate calculations are crucial in determining molecular quantities to understand the chemical composition effectively. This process is essential in chemistry education
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