**Question 21:** Given 6.40 g of HBr. How many moles is this? *To calculate the number of moles from a given mass, use the formula:* \[ \text{Moles} = \frac{\text{Mass (g)}}{\text{Molar Mass (g/mol)}} \] *First, find the molar mass of HBr:* - **Hydrogen (H):** 1.01 g/mol - **Bromine (Br):** 79.90 g/mol *Molar mass of HBr = 1.01 + 79.90 = 80.91 g/mol* *Now substitute the values into the formula:* \[ \text{Moles of HBr} = \frac{6.40 \, \text{g}}{80.91 \, \text{g/mol}} \] *Calculate to find the moles.* **Question 20: Calculation of Lead (II) Chromate Weight** You need 0.0100 moles of lead (II) chromate. How much should you weigh on the scale? ### Explanation: To determine the mass you need to weigh, follow these steps: 1. **Identify the Molar Mass:** - Determine the molar mass of lead (II) chromate (PbCrO₄). - Lead (Pb) has a molar mass of approximately 207.2 g/mol. - Chromium (Cr) has a molar mass of approximately 51.996 g/mol. - Oxygen (O) has a molar mass of 16.00 g/mol, and in chromate, it appears four times. 2. **Calculate the Total Molar Mass:** \[ \text{Molar Mass of PbCrO}_4 = 207.2 \, (Pb) + 51.996 \, (Cr) + 4 \times 16.00 \, (O) \] \[ = 207.2 + 51.996 + 64.00 = 323.196 \, \text{g/mol} \] 3. **Calculate the Mass Required:** - Use the moles given (0.0100 moles) and the molar mass to find the mass. \[ \text{Mass} = \text{Moles} \times \text{Molar Mass} = 0.0100 \, \text{moles} \times 323.196 \, \text{g/mol} \] \[ = 3.23196 \, \text{g} \] Therefore, you should weigh approximately 3.23 grams of lead (II) chromate on the scale.
**Question 21:** Given 6.40 g of HBr. How many moles is this? *To calculate the number of moles from a given mass, use the formula:* \[ \text{Moles} = \frac{\text{Mass (g)}}{\text{Molar Mass (g/mol)}} \] *First, find the molar mass of HBr:* - **Hydrogen (H):** 1.01 g/mol - **Bromine (Br):** 79.90 g/mol *Molar mass of HBr = 1.01 + 79.90 = 80.91 g/mol* *Now substitute the values into the formula:* \[ \text{Moles of HBr} = \frac{6.40 \, \text{g}}{80.91 \, \text{g/mol}} \] *Calculate to find the moles.* **Question 20: Calculation of Lead (II) Chromate Weight** You need 0.0100 moles of lead (II) chromate. How much should you weigh on the scale? ### Explanation: To determine the mass you need to weigh, follow these steps: 1. **Identify the Molar Mass:** - Determine the molar mass of lead (II) chromate (PbCrO₄). - Lead (Pb) has a molar mass of approximately 207.2 g/mol. - Chromium (Cr) has a molar mass of approximately 51.996 g/mol. - Oxygen (O) has a molar mass of 16.00 g/mol, and in chromate, it appears four times. 2. **Calculate the Total Molar Mass:** \[ \text{Molar Mass of PbCrO}_4 = 207.2 \, (Pb) + 51.996 \, (Cr) + 4 \times 16.00 \, (O) \] \[ = 207.2 + 51.996 + 64.00 = 323.196 \, \text{g/mol} \] 3. **Calculate the Mass Required:** - Use the moles given (0.0100 moles) and the molar mass to find the mass. \[ \text{Mass} = \text{Moles} \times \text{Molar Mass} = 0.0100 \, \text{moles} \times 323.196 \, \text{g/mol} \] \[ = 3.23196 \, \text{g} \] Therefore, you should weigh approximately 3.23 grams of lead (II) chromate on the scale.
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 21:** Given 6.40 g of HBr. How many moles is this?
*To calculate the number of moles from a given mass, use the formula:*
\[ \text{Moles} = \frac{\text{Mass (g)}}{\text{Molar Mass (g/mol)}} \]
*First, find the molar mass of HBr:*
- **Hydrogen (H):** 1.01 g/mol
- **Bromine (Br):** 79.90 g/mol
*Molar mass of HBr = 1.01 + 79.90 = 80.91 g/mol*
*Now substitute the values into the formula:*
\[ \text{Moles of HBr} = \frac{6.40 \, \text{g}}{80.91 \, \text{g/mol}} \]
*Calculate to find the moles.*](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5994c871-4ac2-48ae-a76d-bd3d0eb23887%2F107ab046-4252-4262-be38-4dbcb0a956e1%2Fkon36be_processed.png&w=3840&q=75)
Transcribed Image Text:**Question 21:** Given 6.40 g of HBr. How many moles is this?
*To calculate the number of moles from a given mass, use the formula:*
\[ \text{Moles} = \frac{\text{Mass (g)}}{\text{Molar Mass (g/mol)}} \]
*First, find the molar mass of HBr:*
- **Hydrogen (H):** 1.01 g/mol
- **Bromine (Br):** 79.90 g/mol
*Molar mass of HBr = 1.01 + 79.90 = 80.91 g/mol*
*Now substitute the values into the formula:*
\[ \text{Moles of HBr} = \frac{6.40 \, \text{g}}{80.91 \, \text{g/mol}} \]
*Calculate to find the moles.*
![**Question 20: Calculation of Lead (II) Chromate Weight**
You need 0.0100 moles of lead (II) chromate. How much should you weigh on the scale?
### Explanation:
To determine the mass you need to weigh, follow these steps:
1. **Identify the Molar Mass:**
- Determine the molar mass of lead (II) chromate (PbCrO₄).
- Lead (Pb) has a molar mass of approximately 207.2 g/mol.
- Chromium (Cr) has a molar mass of approximately 51.996 g/mol.
- Oxygen (O) has a molar mass of 16.00 g/mol, and in chromate, it appears four times.
2. **Calculate the Total Molar Mass:**
\[
\text{Molar Mass of PbCrO}_4 = 207.2 \, (Pb) + 51.996 \, (Cr) + 4 \times 16.00 \, (O)
\]
\[
= 207.2 + 51.996 + 64.00 = 323.196 \, \text{g/mol}
\]
3. **Calculate the Mass Required:**
- Use the moles given (0.0100 moles) and the molar mass to find the mass.
\[
\text{Mass} = \text{Moles} \times \text{Molar Mass} = 0.0100 \, \text{moles} \times 323.196 \, \text{g/mol}
\]
\[
= 3.23196 \, \text{g}
\]
Therefore, you should weigh approximately 3.23 grams of lead (II) chromate on the scale.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5994c871-4ac2-48ae-a76d-bd3d0eb23887%2F107ab046-4252-4262-be38-4dbcb0a956e1%2Fic1p95c_processed.png&w=3840&q=75)
Transcribed Image Text:**Question 20: Calculation of Lead (II) Chromate Weight**
You need 0.0100 moles of lead (II) chromate. How much should you weigh on the scale?
### Explanation:
To determine the mass you need to weigh, follow these steps:
1. **Identify the Molar Mass:**
- Determine the molar mass of lead (II) chromate (PbCrO₄).
- Lead (Pb) has a molar mass of approximately 207.2 g/mol.
- Chromium (Cr) has a molar mass of approximately 51.996 g/mol.
- Oxygen (O) has a molar mass of 16.00 g/mol, and in chromate, it appears four times.
2. **Calculate the Total Molar Mass:**
\[
\text{Molar Mass of PbCrO}_4 = 207.2 \, (Pb) + 51.996 \, (Cr) + 4 \times 16.00 \, (O)
\]
\[
= 207.2 + 51.996 + 64.00 = 323.196 \, \text{g/mol}
\]
3. **Calculate the Mass Required:**
- Use the moles given (0.0100 moles) and the molar mass to find the mass.
\[
\text{Mass} = \text{Moles} \times \text{Molar Mass} = 0.0100 \, \text{moles} \times 323.196 \, \text{g/mol}
\]
\[
= 3.23196 \, \text{g}
\]
Therefore, you should weigh approximately 3.23 grams of lead (II) chromate on the scale.
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