At Westonci.ca, we connect you with the best answers from a community of experienced and knowledgeable individuals. Experience the convenience of finding accurate answers to your questions from knowledgeable professionals on our platform. Join our platform to connect with experts ready to provide precise answers to your questions in different areas.
Sagot :
### Step-by-Step Solution:
#### 1. Which has a higher molecular weight: [tex]\( \text{NaCl} \)[/tex] or [tex]\( \text{CaCl}_2 \)[/tex]?
To determine the molecular weights, we sum the atomic weights of the elements in each compound:
- For [tex]\( \text{NaCl} \)[/tex]:
- Sodium (Na) has an atomic weight of 23.
- Chlorine (Cl) has an atomic weight of 35.5.
- Hence, the molecular weight of NaCl is [tex]\( 23 + 35.5 = 58.5 \)[/tex] g/mol.
- For [tex]\( \text{CaCl}_2 \)[/tex]:
- Calcium (Ca) has an atomic weight of 40.
- Chlorine (Cl) has an atomic weight of 35.5, and there are two chlorine atoms.
- Hence, the molecular weight of [tex]\( \text{CaCl}_2 \)[/tex] is [tex]\( 40 + 2 \times 35.5 = 111 \)[/tex] g/mol.
Therefore, [tex]\( \text{CaCl}_2 \)[/tex] has a higher molecular weight of 111 g/mol compared to [tex]\( \text{NaCl} \)[/tex] which has a molecular weight of 58.5 g/mol.
#### 2. How many ions does [tex]\( \text{NaCl} \)[/tex] dissociate into? How many ions does [tex]\( \text{CaCl}_2 \)[/tex] dissociate into?
- [tex]\( \text{NaCl} \)[/tex] dissociates into:
- One sodium ion (Na[tex]\(^+\)[/tex])
- One chloride ion (Cl[tex]\(^-\)[/tex])
- Total: [tex]\( 2 \)[/tex] ions.
- [tex]\( \text{CaCl}_2 \)[/tex] dissociates into:
- One calcium ion (Ca[tex]\(^2+\)[/tex])
- Two chloride ions (2Cl[tex]\(^-\)[/tex])
- Total: [tex]\( 3 \)[/tex] ions.
#### 3. About how many moles of [tex]\( \text{NaCl} \)[/tex] are in a cc (approximately 1.1 g) of [tex]\( \text{NaCl} \)[/tex]?
To find the moles of [tex]\( \text{NaCl} \)[/tex], we use the formula:
[tex]\[ \text{Moles} = \frac{\text{Mass (g)}}{\text{Molar Mass (g/mol)}} \][/tex]
For [tex]\( \text{NaCl} \)[/tex]:
- Mass = 1.1 g
- Molar Mass = 58.5 g/mol
Hence,
[tex]\[ \text{Moles of NaCl} = \frac{1.1 \text{ g}}{58.5 \text{ g/mol}} \approx 0.0188 \text{ moles} \][/tex]
#### 4. About how many moles of [tex]\( \text{CaCl}_2 \)[/tex] are in a cc (approximately 1.3 g) of [tex]\( \text{CaCl}_2 \)[/tex]?
Using the same formula, for [tex]\( \text{CaCl}_2 \)[/tex]:
- Mass = 1.3 g
- Molar Mass = 111 g/mol
Hence,
[tex]\[ \text{Moles of CaCl}_2 = \frac{1.3 \text{ g}}{111 \text{ g/mol}} \approx 0.0117 \text{ moles} \][/tex]
### Summary of Answers:
1. The compound with the higher molecular weight is [tex]\( \text{CaCl}_2 \)[/tex].
2.
- [tex]\( \text{NaCl} \)[/tex] dissociates into 2 ions.
- [tex]\( \text{CaCl}_2 \)[/tex] dissociates into 3 ions.
3. There are approximately 0.0188 moles of [tex]\( \text{NaCl} \)[/tex] in 1 cc (1.1 g) of [tex]\( \text{NaCl} \)[/tex].
4. There are approximately 0.0117 moles of [tex]\( \text{CaCl}_2 \)[/tex] in 1 cc (1.3 g) of [tex]\( \text{CaCl}_2 \)[/tex].
#### 1. Which has a higher molecular weight: [tex]\( \text{NaCl} \)[/tex] or [tex]\( \text{CaCl}_2 \)[/tex]?
To determine the molecular weights, we sum the atomic weights of the elements in each compound:
- For [tex]\( \text{NaCl} \)[/tex]:
- Sodium (Na) has an atomic weight of 23.
- Chlorine (Cl) has an atomic weight of 35.5.
- Hence, the molecular weight of NaCl is [tex]\( 23 + 35.5 = 58.5 \)[/tex] g/mol.
- For [tex]\( \text{CaCl}_2 \)[/tex]:
- Calcium (Ca) has an atomic weight of 40.
- Chlorine (Cl) has an atomic weight of 35.5, and there are two chlorine atoms.
- Hence, the molecular weight of [tex]\( \text{CaCl}_2 \)[/tex] is [tex]\( 40 + 2 \times 35.5 = 111 \)[/tex] g/mol.
Therefore, [tex]\( \text{CaCl}_2 \)[/tex] has a higher molecular weight of 111 g/mol compared to [tex]\( \text{NaCl} \)[/tex] which has a molecular weight of 58.5 g/mol.
#### 2. How many ions does [tex]\( \text{NaCl} \)[/tex] dissociate into? How many ions does [tex]\( \text{CaCl}_2 \)[/tex] dissociate into?
- [tex]\( \text{NaCl} \)[/tex] dissociates into:
- One sodium ion (Na[tex]\(^+\)[/tex])
- One chloride ion (Cl[tex]\(^-\)[/tex])
- Total: [tex]\( 2 \)[/tex] ions.
- [tex]\( \text{CaCl}_2 \)[/tex] dissociates into:
- One calcium ion (Ca[tex]\(^2+\)[/tex])
- Two chloride ions (2Cl[tex]\(^-\)[/tex])
- Total: [tex]\( 3 \)[/tex] ions.
#### 3. About how many moles of [tex]\( \text{NaCl} \)[/tex] are in a cc (approximately 1.1 g) of [tex]\( \text{NaCl} \)[/tex]?
To find the moles of [tex]\( \text{NaCl} \)[/tex], we use the formula:
[tex]\[ \text{Moles} = \frac{\text{Mass (g)}}{\text{Molar Mass (g/mol)}} \][/tex]
For [tex]\( \text{NaCl} \)[/tex]:
- Mass = 1.1 g
- Molar Mass = 58.5 g/mol
Hence,
[tex]\[ \text{Moles of NaCl} = \frac{1.1 \text{ g}}{58.5 \text{ g/mol}} \approx 0.0188 \text{ moles} \][/tex]
#### 4. About how many moles of [tex]\( \text{CaCl}_2 \)[/tex] are in a cc (approximately 1.3 g) of [tex]\( \text{CaCl}_2 \)[/tex]?
Using the same formula, for [tex]\( \text{CaCl}_2 \)[/tex]:
- Mass = 1.3 g
- Molar Mass = 111 g/mol
Hence,
[tex]\[ \text{Moles of CaCl}_2 = \frac{1.3 \text{ g}}{111 \text{ g/mol}} \approx 0.0117 \text{ moles} \][/tex]
### Summary of Answers:
1. The compound with the higher molecular weight is [tex]\( \text{CaCl}_2 \)[/tex].
2.
- [tex]\( \text{NaCl} \)[/tex] dissociates into 2 ions.
- [tex]\( \text{CaCl}_2 \)[/tex] dissociates into 3 ions.
3. There are approximately 0.0188 moles of [tex]\( \text{NaCl} \)[/tex] in 1 cc (1.1 g) of [tex]\( \text{NaCl} \)[/tex].
4. There are approximately 0.0117 moles of [tex]\( \text{CaCl}_2 \)[/tex] in 1 cc (1.3 g) of [tex]\( \text{CaCl}_2 \)[/tex].
Thank you for trusting us with your questions. We're here to help you find accurate answers quickly and efficiently. We appreciate your visit. Our platform is always here to offer accurate and reliable answers. Return anytime. Thank you for trusting Westonci.ca. Don't forget to revisit us for more accurate and insightful answers.
