Lithium and nitrogen undergo the following reaction: 6 Li (s) + N₂(g) → 2 Li³N (s) Calculate the mass of nitrogen needed for 0.450 moles of Lithium to react. Select one: O a. 28g N₂ O b. 2.10 g N₂ O c. 1.05g N₂ O d. 12.6 g N₂
Lithium and nitrogen undergo the following reaction: 6 Li (s) + N₂(g) → 2 Li³N (s) Calculate the mass of nitrogen needed for 0.450 moles of Lithium to react. Select one: O a. 28g N₂ O b. 2.10 g N₂ O c. 1.05g N₂ O d. 12.6 g N₂
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![### Chemical Reaction Between Lithium and Nitrogen
In a chemical reaction, lithium and nitrogen combine according to the equation:
\[ 6 \text{Li (s)} + \text{N}_2 \text{(g)} \rightarrow 2 \text{Li}_3\text{N (s)} \]
To solve the problem provided on your educational platform, read the following information carefully:
**Problem Statement:**
Calculate the mass of nitrogen (N\(_2\)) needed for 0.450 moles of lithium (Li) to react.
**Options Provided:**
- a. 28g N\(_2\)
- b. 2.10g N\(_2\)
- c. 1.05g N\(_2\)
- d. 12.6g N\(_2\)
**Explanation:**
To determine the correct answer, you will need to use stoichiometry, a key concept in chemistry that involves the quantitative relationships between reactants and products in a chemical reaction.
**Steps to Calculate:**
1. **Identify the molar ratio from the balanced chemical equation:**
\[ 6 \text{Li (s)} + \text{N}_2 \text{(g)} \rightarrow 2 \text{Li}_3\text{N (s)} \]
From this, 6 moles of lithium react with 1 mole of nitrogen gas (N\(_2\)).
2. **Use the molar ratio to find moles of nitrogen (N\(_2\)) needed for 0.450 moles of lithium:**
\[ \text{Moles of N}_2 = \frac{0.450 \text{ moles Li} \times 1 \text{ mole N}_2}{6 \text{ moles Li}} = 0.075 \text{ moles N}_2 \]
3. **Calculate the mass of nitrogen gas (N\(_2\)):**
- Molar mass of N\(_2\) = 2 × 14.01 g/mol = 28.02 g/mol
\[ \text{Mass of N}_2 = 0.075 \text{ moles} \times 28.02 \text{ g/mol} = 2.1015 \text{ g} \approx 2.10 \text{ g}](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F60284858-4488-4a01-ab4b-8c5c4b90a41d%2F13468d6c-513d-45bd-a89b-80d4af668116%2Fmhn20am_processed.png&w=3840&q=75)
Transcribed Image Text:### Chemical Reaction Between Lithium and Nitrogen
In a chemical reaction, lithium and nitrogen combine according to the equation:
\[ 6 \text{Li (s)} + \text{N}_2 \text{(g)} \rightarrow 2 \text{Li}_3\text{N (s)} \]
To solve the problem provided on your educational platform, read the following information carefully:
**Problem Statement:**
Calculate the mass of nitrogen (N\(_2\)) needed for 0.450 moles of lithium (Li) to react.
**Options Provided:**
- a. 28g N\(_2\)
- b. 2.10g N\(_2\)
- c. 1.05g N\(_2\)
- d. 12.6g N\(_2\)
**Explanation:**
To determine the correct answer, you will need to use stoichiometry, a key concept in chemistry that involves the quantitative relationships between reactants and products in a chemical reaction.
**Steps to Calculate:**
1. **Identify the molar ratio from the balanced chemical equation:**
\[ 6 \text{Li (s)} + \text{N}_2 \text{(g)} \rightarrow 2 \text{Li}_3\text{N (s)} \]
From this, 6 moles of lithium react with 1 mole of nitrogen gas (N\(_2\)).
2. **Use the molar ratio to find moles of nitrogen (N\(_2\)) needed for 0.450 moles of lithium:**
\[ \text{Moles of N}_2 = \frac{0.450 \text{ moles Li} \times 1 \text{ mole N}_2}{6 \text{ moles Li}} = 0.075 \text{ moles N}_2 \]
3. **Calculate the mass of nitrogen gas (N\(_2\)):**
- Molar mass of N\(_2\) = 2 × 14.01 g/mol = 28.02 g/mol
\[ \text{Mass of N}_2 = 0.075 \text{ moles} \times 28.02 \text{ g/mol} = 2.1015 \text{ g} \approx 2.10 \text{ g}
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