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To determine how many grams of NaCl would be produced from 507 grams of FeClâ‚‚, let's go through the problem step-by-step.
### Step 1: Determine the molar masses
First, we need to calculate the molar masses of the compounds involved.
- For FeClâ‚‚:
- The atomic mass of Fe (iron) is approximately 55.845 g/mol.
- The atomic mass of Cl (chlorine) is approximately 35.453 g/mol.
- Therefore, the molar mass of FeClâ‚‚ is:
[tex]\[ \text{Molar mass of FeCl}_2 = 55.845 + 2 \times 35.453 = 126.751 \, \text{g/mol} \][/tex]
- For NaCl:
- The atomic mass of Na (sodium) is approximately 22.99 g/mol.
- The atomic mass of Cl (chlorine) is approximately 35.453 g/mol.
- Thus, the molar mass of NaCl is:
[tex]\[ \text{Molar mass of NaCl} = 22.99 + 35.453 = 58.443 \, \text{g/mol} \][/tex]
### Step 2: Calculate the moles of FeClâ‚‚
We have 507 grams of FeClâ‚‚. To determine the number of moles of FeClâ‚‚, use the formula:
[tex]\[ \text{moles of FeCl}_2 = \frac{\text{mass}}{\text{molar mass}} \][/tex]
[tex]\[ \text{moles of FeCl}_2 = \frac{507 \, \text{g}}{126.751 \, \text{g/mol}} \approx 3.999968 \, \text{moles} \][/tex]
### Step 3: Use stoichiometry to find moles of NaCl produced
According to the balanced chemical equation:
[tex]\[ FeCl_2 + 2NaOH \rightarrow Fe(OH)_2(s) + 2NaCl \][/tex]
1 mole of FeClâ‚‚ produces 2 moles of NaCl. Therefore, the moles of NaCl produced will be:
[tex]\[ \text{moles of NaCl} = 2 \times \text{moles of FeCl}_2 = 2 \times 3.999968 = 7.999936 \, \text{moles} \][/tex]
### Step 4: Calculate the mass of NaCl produced
Finally, convert the moles of NaCl to grams using its molar mass:
[tex]\[ \text{mass of NaCl} = \text{moles of NaCl} \times \text{molar mass of NaCl} \][/tex]
[tex]\[ \text{mass of NaCl} = 7.999936 \, \text{moles} \times 58.443 \, \text{g/mol} \approx 467.52 \, \text{g} \][/tex]
### Conclusion
The mass of NaCl produced from 507 grams of FeClâ‚‚ is approximately 467.52 grams. Therefore, the correct answer is:
B. [tex]\(467.52 \, \text{g} \)[/tex] NaCl
### Step 1: Determine the molar masses
First, we need to calculate the molar masses of the compounds involved.
- For FeClâ‚‚:
- The atomic mass of Fe (iron) is approximately 55.845 g/mol.
- The atomic mass of Cl (chlorine) is approximately 35.453 g/mol.
- Therefore, the molar mass of FeClâ‚‚ is:
[tex]\[ \text{Molar mass of FeCl}_2 = 55.845 + 2 \times 35.453 = 126.751 \, \text{g/mol} \][/tex]
- For NaCl:
- The atomic mass of Na (sodium) is approximately 22.99 g/mol.
- The atomic mass of Cl (chlorine) is approximately 35.453 g/mol.
- Thus, the molar mass of NaCl is:
[tex]\[ \text{Molar mass of NaCl} = 22.99 + 35.453 = 58.443 \, \text{g/mol} \][/tex]
### Step 2: Calculate the moles of FeClâ‚‚
We have 507 grams of FeClâ‚‚. To determine the number of moles of FeClâ‚‚, use the formula:
[tex]\[ \text{moles of FeCl}_2 = \frac{\text{mass}}{\text{molar mass}} \][/tex]
[tex]\[ \text{moles of FeCl}_2 = \frac{507 \, \text{g}}{126.751 \, \text{g/mol}} \approx 3.999968 \, \text{moles} \][/tex]
### Step 3: Use stoichiometry to find moles of NaCl produced
According to the balanced chemical equation:
[tex]\[ FeCl_2 + 2NaOH \rightarrow Fe(OH)_2(s) + 2NaCl \][/tex]
1 mole of FeClâ‚‚ produces 2 moles of NaCl. Therefore, the moles of NaCl produced will be:
[tex]\[ \text{moles of NaCl} = 2 \times \text{moles of FeCl}_2 = 2 \times 3.999968 = 7.999936 \, \text{moles} \][/tex]
### Step 4: Calculate the mass of NaCl produced
Finally, convert the moles of NaCl to grams using its molar mass:
[tex]\[ \text{mass of NaCl} = \text{moles of NaCl} \times \text{molar mass of NaCl} \][/tex]
[tex]\[ \text{mass of NaCl} = 7.999936 \, \text{moles} \times 58.443 \, \text{g/mol} \approx 467.52 \, \text{g} \][/tex]
### Conclusion
The mass of NaCl produced from 507 grams of FeClâ‚‚ is approximately 467.52 grams. Therefore, the correct answer is:
B. [tex]\(467.52 \, \text{g} \)[/tex] NaCl
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