1. How many ions in 0.187 mol of Na' ions? Ans.: 1.13 x1023 jons Nal 0.187 mol6.0 l6.022X1023:0n 3D1.13x1023 ions I mol Na 2. How many atoms in 1.45x10 mol of arsenic? Ans.: 8.73 x10 atoms As 6.022 x1023ataom | mol 1.45X10-1 = 8.73x/06
1. How many ions in 0.187 mol of Na' ions? Ans.: 1.13 x1023 jons Nal 0.187 mol6.0 l6.022X1023:0n 3D1.13x1023 ions I mol Na 2. How many atoms in 1.45x10 mol of arsenic? Ans.: 8.73 x10 atoms As 6.022 x1023ataom | mol 1.45X10-1 = 8.73x/06
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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![**Chapter 7 Worksheet**
**Ch. 7-1 pg. 228 pp#1-3 Moles ↔ Particles**
1. How many ions in 0.187 mol of Na⁺ ions?
Ans.: \( 1.13 \times 10^{23} \) ions Na⁺
Calculation:
\[ 0.187 \, \text{mol} \times \frac{6.022 \times 10^{23} \, \text{ions}}{1 \, \text{mol}} = 1.13 \times 10^{23} \, \text{ions} \, \text{Na}^+ \]
2. How many atoms in \( 1.45 \times 10^{-17} \) mol of arsenic?
Ans.: \( 8.73 \times 10^6 \) atoms As
Calculation:
\[ 1.45 \times 10^{-17} \, \text{mol} \times \frac{6.022 \times 10^{23} \, \text{atoms}}{1 \, \text{mol}} = 8.73 \times 10^6 \, \text{atoms} \, \text{As} \]
**Ch. 7-1 pg. 229**
3. How many moles do \( 5.66 \times 10^{25} \) lithium ions, Li⁺ equal?
Ans.: 94.0 mol Li⁺
4. How many moles in \( 3.161 \times 10^{21} \) molecules of CO₂?
Ans.: 0.00525 mol CO₂
**Ch. 7-1 pg. 231 pp#1-3 Mass ↔ Particles**
5. What is the mass of \( 2.11 \times 10^{24} \) atoms of copper?
Ans.: 223 g Cu
Calculation:
\[ 2.11 \times 10^{24} \, \text{atoms} \times \frac{63.55 \, \text{g}}{6.022 \times 10^{23} \, \text{atoms}} = 223 \, \text{g Cu} \]
6. What is](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fbb0fc032-1da3-4337-9872-956185f0c3aa%2F16269620-2f9b-4c1a-8a2f-77870e3ac706%2Fw3pfkk_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Chapter 7 Worksheet**
**Ch. 7-1 pg. 228 pp#1-3 Moles ↔ Particles**
1. How many ions in 0.187 mol of Na⁺ ions?
Ans.: \( 1.13 \times 10^{23} \) ions Na⁺
Calculation:
\[ 0.187 \, \text{mol} \times \frac{6.022 \times 10^{23} \, \text{ions}}{1 \, \text{mol}} = 1.13 \times 10^{23} \, \text{ions} \, \text{Na}^+ \]
2. How many atoms in \( 1.45 \times 10^{-17} \) mol of arsenic?
Ans.: \( 8.73 \times 10^6 \) atoms As
Calculation:
\[ 1.45 \times 10^{-17} \, \text{mol} \times \frac{6.022 \times 10^{23} \, \text{atoms}}{1 \, \text{mol}} = 8.73 \times 10^6 \, \text{atoms} \, \text{As} \]
**Ch. 7-1 pg. 229**
3. How many moles do \( 5.66 \times 10^{25} \) lithium ions, Li⁺ equal?
Ans.: 94.0 mol Li⁺
4. How many moles in \( 3.161 \times 10^{21} \) molecules of CO₂?
Ans.: 0.00525 mol CO₂
**Ch. 7-1 pg. 231 pp#1-3 Mass ↔ Particles**
5. What is the mass of \( 2.11 \times 10^{24} \) atoms of copper?
Ans.: 223 g Cu
Calculation:
\[ 2.11 \times 10^{24} \, \text{atoms} \times \frac{63.55 \, \text{g}}{6.022 \times 10^{23} \, \text{atoms}} = 223 \, \text{g Cu} \]
6. What is
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