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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![**Question:**
How many grams of Co are there in a sample of Co that contains \(8.40 \times 10^{23}\) atoms? [Text box] grams
**Explanation:**
This question asks for the mass in grams of a sample of cobalt (Co) which contains a specified number of atoms. To solve this, you can use Avogadro's number, which is \(6.022 \times 10^{23}\) atoms/mol, and the molar mass of cobalt. The calculation involves converting the number of atoms to moles and then to grams.
**Steps for Calculation:**
1. **Calculate Moles:**
\[
\text{Moles of Co} = \frac{8.40 \times 10^{23} \text{ atoms}}{6.022 \times 10^{23} \text{ atoms/mol}}
\]
2. **Convert to Grams:**
\[
\text{Mass in grams} = \text{Moles of Co} \times \text{Molar mass of Co (approximately 58.93 g/mol)}
\]
Provide the calculated result in the text box.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F15cd763b-5763-4f34-ac90-fb3a4d78f352%2Fd0bd440e-5895-4014-94fb-8ac15653aa54%2F744g2z4_processed.png&w=3840&q=75)
Transcribed Image Text:**Question:**
How many grams of Co are there in a sample of Co that contains \(8.40 \times 10^{23}\) atoms? [Text box] grams
**Explanation:**
This question asks for the mass in grams of a sample of cobalt (Co) which contains a specified number of atoms. To solve this, you can use Avogadro's number, which is \(6.022 \times 10^{23}\) atoms/mol, and the molar mass of cobalt. The calculation involves converting the number of atoms to moles and then to grams.
**Steps for Calculation:**
1. **Calculate Moles:**
\[
\text{Moles of Co} = \frac{8.40 \times 10^{23} \text{ atoms}}{6.022 \times 10^{23} \text{ atoms/mol}}
\]
2. **Convert to Grams:**
\[
\text{Mass in grams} = \text{Moles of Co} \times \text{Molar mass of Co (approximately 58.93 g/mol)}
\]
Provide the calculated result in the text box.
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