Question
2Li+F2->2LiF
Show that 31g of lithium produces approximately 115g of lithiium florine
Show that 31g of lithium produces approximately 115g of lithiium florine
Answers
Answer
Redoubler à l'école est une pratique encore relativement répandue en
France mais pratiquement inconnue en Grande-Bretagne. Celle-ci
consiste à refaire une année précise du cursus scolaire pour des
raisons variées: soucis de santé, manque de travail ou de maturité, etc.
On peut y voir aussi bien des avantages que des inconvénients:
permettre à un élève en difficulté de s'améliorer mais aussi, dans
certains cas, être stigmatisé et séparé de ses pairs.
Translate into English
France mais pratiquement inconnue en Grande-Bretagne. Celle-ci
consiste à refaire une année précise du cursus scolaire pour des
raisons variées: soucis de santé, manque de travail ou de maturité, etc.
On peut y voir aussi bien des avantages que des inconvénients:
permettre à un élève en difficulté de s'améliorer mais aussi, dans
certains cas, être stigmatisé et séparé de ses pairs.
Translate into English
Answered by
GPT-4o mini
To show that 31 g of lithium produces approximately 115 g of lithium fluoride (LiF), we can use stoichiometry based on the balanced chemical reaction:
\[ 2 \text{Li} + \text{F}_2 \rightarrow 2 \text{LiF} \]
**Step 1: Determine the molar mass of lithium (Li) and lithium fluoride (LiF).**
- The molar mass of lithium (Li) is approximately \( 6.94 \, \text{g/mol} \).
- The molar mass of fluorine (F) is approximately \( 19.00 \, \text{g/mol} \).
- Therefore, the molar mass of lithium fluoride (LiF) is:
\[
\text{Molar mass of LiF} = \text{Molar mass of Li} + \text{Molar mass of F} = 6.94 \, \text{g/mol} + 19.00 \, \text{g/mol} = 25.94 \, \text{g/mol}
\]
**Step 2: Calculate the number of moles of lithium.**
Using the mass of lithium given (31 g):
\[
\text{Number of moles of Li} = \frac{\text{mass}}{\text{molar mass}} = \frac{31 \, \text{g}}{6.94 \, \text{g/mol}} \approx 4.47 \, \text{mol}
\]
**Step 3: Determine the moles of lithium fluoride produced.**
From the balanced equation, we see that 2 moles of Li produce 2 moles of LiF. Therefore, the number of moles of LiF produced will be equal to the number of moles of Li used:
\[
\text{Moles of LiF} = \text{Moles of Li} = 4.47 \, \text{mol}
\]
**Step 4: Calculate the mass of lithium fluoride produced.**
Using the molar mass of LiF:
\[
\text{Mass of LiF} = \text{Number of moles} \times \text{Molar mass} = 4.47 \, \text{mol} \times 25.94 \, \text{g/mol} \approx 116.54 \, \text{g}
\]
**Conclusion:**
Approximately 116.54 g of lithium fluoride is produced from 31 g of lithium, which rounds to approximately 115 g. Thus, we have shown that 31 g of lithium produces approximately 115 g of lithium fluoride.
\[ 2 \text{Li} + \text{F}_2 \rightarrow 2 \text{LiF} \]
**Step 1: Determine the molar mass of lithium (Li) and lithium fluoride (LiF).**
- The molar mass of lithium (Li) is approximately \( 6.94 \, \text{g/mol} \).
- The molar mass of fluorine (F) is approximately \( 19.00 \, \text{g/mol} \).
- Therefore, the molar mass of lithium fluoride (LiF) is:
\[
\text{Molar mass of LiF} = \text{Molar mass of Li} + \text{Molar mass of F} = 6.94 \, \text{g/mol} + 19.00 \, \text{g/mol} = 25.94 \, \text{g/mol}
\]
**Step 2: Calculate the number of moles of lithium.**
Using the mass of lithium given (31 g):
\[
\text{Number of moles of Li} = \frac{\text{mass}}{\text{molar mass}} = \frac{31 \, \text{g}}{6.94 \, \text{g/mol}} \approx 4.47 \, \text{mol}
\]
**Step 3: Determine the moles of lithium fluoride produced.**
From the balanced equation, we see that 2 moles of Li produce 2 moles of LiF. Therefore, the number of moles of LiF produced will be equal to the number of moles of Li used:
\[
\text{Moles of LiF} = \text{Moles of Li} = 4.47 \, \text{mol}
\]
**Step 4: Calculate the mass of lithium fluoride produced.**
Using the molar mass of LiF:
\[
\text{Mass of LiF} = \text{Number of moles} \times \text{Molar mass} = 4.47 \, \text{mol} \times 25.94 \, \text{g/mol} \approx 116.54 \, \text{g}
\]
**Conclusion:**
Approximately 116.54 g of lithium fluoride is produced from 31 g of lithium, which rounds to approximately 115 g. Thus, we have shown that 31 g of lithium produces approximately 115 g of lithium fluoride.
Answered by
GPT-4o mini
Repeating a year at school is still a relatively common practice in France but is practically unknown in Great Britain. This involves going through a specific year of the school curriculum again for various reasons: health issues, lack of effort, or maturity, etc. There can be both advantages and disadvantages to this practice: it can allow a struggling student to improve, but it can also, in some cases, lead to stigmatization and separation from their peers.