How Many Grams Of L I 3 N Li_3N L I 3 ​ N Can Be Formed From 1.75 Moles Of L I Li L I ? Assume An Excess Of Nitrogen.${ 6 \text{ Li(s)} + \text{N}_2\text{(g)} \rightarrow 2 \text{ Li}_3\text{N(s)} }$\text{moles Li}$

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1.1 Introduction

In this problem, we are tasked with determining the amount of lithium nitride (Li3NLi_3N) that can be formed from a given quantity of lithium (LiLi). The reaction between lithium and nitrogen is a highly exothermic process, resulting in the formation of lithium nitride. To solve this problem, we will need to use the concept of stoichiometry, which is the study of the quantitative relationships between reactants and products in chemical reactions.

1.2 The Reaction

The reaction between lithium and nitrogen is as follows:

6 Li(s)+N2(g)→2 Li3N(s){ 6 \text{ Li(s)} + \text{N}_2\text{(g)} \rightarrow 2 \text{ Li}_3\text{N(s)} }

From this equation, we can see that 6 moles of lithium are required to react with 1 mole of nitrogen to produce 2 moles of lithium nitride.

1.3 Stoichiometry

To determine the amount of lithium nitride that can be formed from 1.75 moles of lithium, we need to use the concept of stoichiometry. We can start by identifying the mole ratio between lithium and lithium nitride in the reaction equation.

From the reaction equation, we can see that 6 moles of lithium are required to produce 2 moles of lithium nitride. This means that the mole ratio between lithium and lithium nitride is 6:2 or 3:1.

1.4 Calculating the Amount of Lithium Nitride

Now that we have identified the mole ratio between lithium and lithium nitride, we can use this information to calculate the amount of lithium nitride that can be formed from 1.75 moles of lithium.

We can start by multiplying the number of moles of lithium by the mole ratio between lithium and lithium nitride.

1.75 mol Li×2 mol Li3N6 mol Li=0.583 mol Li3N{ 1.75 \text{ mol Li} \times \frac{2 \text{ mol Li}_3\text{N}}{6 \text{ mol Li}} = 0.583 \text{ mol Li}_3\text{N} }

1.5 Converting Moles to Grams

Now that we have calculated the amount of lithium nitride in moles, we need to convert this value to grams. To do this, we need to know the molar mass of lithium nitride.

The molar mass of lithium nitride is 73.89 g/mol. We can use this value to convert the amount of lithium nitride from moles to grams.

0.583 mol Li3N×73.89 g/mol=43.01 g Li3N{ 0.583 \text{ mol Li}_3\text{N} \times 73.89 \text{ g/mol} = 43.01 \text{ g Li}_3\text{N} }

1.6 Conclusion

In this problem, we were tasked with determining the amount of lithium nitride that can be formed from 1.75 moles of lithium. We used the concept of stoichiometry to calculate the amount of lithium nitride in moles, and then converted this value to grams using the molar mass of lithium nitride. The result is that 43.01 grams of lithium nitride can be formed from 1.75 moles of lithium.

1.7 References

  • "General Chemistry" by Linus Pauling
  • "Chemistry: An Atoms First Approach" by Steven S. Zumdahl

1.8 Additional Resources

  • Khan Academy: Stoichiometry
  • Chemistry LibreTexts: Stoichiometry

1.9 Final Answer

The final answer is: 43.01\boxed{43.01}

2.1 Introduction

In the previous article, we discussed how to calculate the amount of lithium nitride that can be formed from a given quantity of lithium. In this article, we will answer some frequently asked questions related to the formation of lithium nitride.

2.2 Q&A

2.2.1 Q: What is the molar mass of lithium nitride?

A: The molar mass of lithium nitride is 73.89 g/mol.

2.2.2 Q: How many moles of lithium are required to produce 1 mole of lithium nitride?

A: According to the reaction equation, 6 moles of lithium are required to produce 2 moles of lithium nitride. Therefore, 3 moles of lithium are required to produce 1 mole of lithium nitride.

2.2.3 Q: What is the mole ratio between lithium and lithium nitride?

A: The mole ratio between lithium and lithium nitride is 6:2 or 3:1.

2.2.4 Q: How can I calculate the amount of lithium nitride that can be formed from a given quantity of lithium?

A: To calculate the amount of lithium nitride that can be formed from a given quantity of lithium, you need to multiply the number of moles of lithium by the mole ratio between lithium and lithium nitride.

2.2.5 Q: What is the difference between lithium nitride and lithium?

A: Lithium nitride is a compound that consists of lithium and nitrogen, while lithium is a pure element.

2.2.6 Q: Can lithium nitride be used as a fuel?

A: Lithium nitride is not typically used as a fuel. However, it can be used as a source of lithium, which can be used as a fuel in certain applications.

2.2.7 Q: What are some common applications of lithium nitride?

A: Lithium nitride is used in a variety of applications, including:

  • Lithium-ion batteries
  • Catalysts
  • Electrodes
  • Semiconductors

2.3 Conclusion

In this article, we answered some frequently asked questions related to the formation of lithium nitride. We hope that this information is helpful to you.

2.4 References

  • "General Chemistry" by Linus Pauling
  • "Chemistry: An Atoms First Approach" by Steven S. Zumdahl

2.5 Additional Resources

  • Khan Academy: Stoichiometry
  • Chemistry LibreTexts: Stoichiometry

2.6 Final Answer

The final answer is: 43.01\boxed{43.01}