3 **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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How many grams of Co are there in a sample of Co that contains 8.40×1023 atoms? grams

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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