Given The Following Balanced Reaction Between Nitrogen Gas And Oxygen Gas To Produce Nitrous Oxide Gas, How Many Moles Of Nitrous Oxide Gas Are Produced From 1.65 Moles Of Nitrogen Gas? N 2 ( G ) + O 2 ( G ) → 2 N O ( G N_2(g) + O_2(g) \rightarrow 2 NO(g N 2 ​ ( G ) + O 2 ​ ( G ) → 2 NO ( G ]

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Introduction

In chemistry, understanding the stoichiometry of chemical reactions is crucial for determining the amount of products formed from a given amount of reactants. The balanced chemical equation between nitrogen gas (N2) and oxygen gas (O2) to produce nitrous oxide gas (NO) is a fundamental reaction in chemistry. In this article, we will discuss how to calculate the number of moles of nitrous oxide gas produced from a given amount of nitrogen gas.

Understanding the Balanced Chemical Equation

The balanced chemical equation for the reaction between nitrogen gas and oxygen gas to produce nitrous oxide gas is:

N2(g)+O2(g)→2NO(g)N_2(g) + O_2(g) \rightarrow 2 NO(g)

From the balanced equation, we can see that 1 mole of nitrogen gas reacts with 1/2 mole of oxygen gas to produce 2 moles of nitrous oxide gas.

Calculating Moles of Nitrous Oxide Gas

To calculate the number of moles of nitrous oxide gas produced from 1.65 moles of nitrogen gas, we need to follow the stoichiometry of the reaction. According to the balanced equation, 1 mole of nitrogen gas produces 2 moles of nitrous oxide gas. Therefore, we can set up a proportion to calculate the number of moles of nitrous oxide gas produced from 1.65 moles of nitrogen gas:

1 mole N22 moles NO=1.65 moles N2x moles NO\frac{1 \text{ mole } N_2}{2 \text{ moles } NO} = \frac{1.65 \text{ moles } N_2}{x \text{ moles } NO}

Solving for x, we get:

x=1.65 moles N2×2 moles NO1 mole N2x = \frac{1.65 \text{ moles } N_2 \times 2 \text{ moles } NO}{1 \text{ mole } N_2}

x=3.30 moles NOx = 3.30 \text{ moles } NO

Therefore, 1.65 moles of nitrogen gas will produce 3.30 moles of nitrous oxide gas.

Conclusion

In conclusion, understanding the stoichiometry of chemical reactions is crucial for determining the amount of products formed from a given amount of reactants. By following the balanced chemical equation and setting up a proportion, we can calculate the number of moles of nitrous oxide gas produced from 1.65 moles of nitrogen gas.

Additional Information

  • The balanced chemical equation for the reaction between nitrogen gas and oxygen gas to produce nitrous oxide gas is: $N_2(g) + O_2(g) \rightarrow 2 NO(g)$
  • The stoichiometry of the reaction is 1 mole of nitrogen gas to 1/2 mole of oxygen gas to 2 moles of nitrous oxide gas.
  • To calculate the number of moles of nitrous oxide gas produced from a given amount of nitrogen gas, we need to follow the stoichiometry of the reaction and set up a proportion.

References

  • Chemistry: An Atoms First Approach, by Steven S. Zumdahl
  • General Chemistry: Principles and Modern Applications, by Linus Pauling

Frequently Asked Questions

  • Q: What is the balanced chemical equation for the reaction between nitrogen gas and oxygen gas to produce nitrous oxide gas? A: The balanced chemical equation is: $N_2(g) + O_2(g) \rightarrow 2 NO(g)$
  • Q: How many moles of nitrous oxide gas are produced from 1.65 moles of nitrogen gas? A: 3.30 moles of nitrous oxide gas are produced from 1.65 moles of nitrogen gas.

Related Topics

  • Stoichiometry of chemical reactions
  • Balanced chemical equations
  • Moles of reactants and products

Chemistry Resources

  • Chemistry: An Atoms First Approach, by Steven S. Zumdahl
  • General Chemistry: Principles and Modern Applications, by Linus Pauling
  • Chemistry Online Resources: Khan Academy, Chemistry LibreTexts
    Nitrogen Gas and Oxygen Gas Reaction: Q&A =============================================

Q: What is the balanced chemical equation for the reaction between nitrogen gas and oxygen gas to produce nitrous oxide gas?

A: The balanced chemical equation is:

N2(g)+O2(g)→2NO(g)N_2(g) + O_2(g) \rightarrow 2 NO(g)

Q: How many moles of nitrous oxide gas are produced from 1.65 moles of nitrogen gas?

A: 3.30 moles of nitrous oxide gas are produced from 1.65 moles of nitrogen gas.

Q: What is the stoichiometry of the reaction between nitrogen gas and oxygen gas to produce nitrous oxide gas?

A: The stoichiometry of the reaction is 1 mole of nitrogen gas to 1/2 mole of oxygen gas to 2 moles of nitrous oxide gas.

Q: How do I calculate the number of moles of nitrous oxide gas produced from a given amount of nitrogen gas?

A: To calculate the number of moles of nitrous oxide gas produced from a given amount of nitrogen gas, you need to follow the stoichiometry of the reaction and set up a proportion. The proportion is:

1 mole N22 moles NO=x moles N2y moles NO\frac{1 \text{ mole } N_2}{2 \text{ moles } NO} = \frac{x \text{ moles } N_2}{y \text{ moles } NO}

Where x is the number of moles of nitrogen gas and y is the number of moles of nitrous oxide gas.

Q: What is the relationship between the number of moles of nitrogen gas and the number of moles of nitrous oxide gas?

A: The number of moles of nitrous oxide gas is twice the number of moles of nitrogen gas.

Q: Can I use this reaction to produce nitrous oxide gas on a large scale?

A: Yes, this reaction can be used to produce nitrous oxide gas on a large scale. However, you need to consider the safety and environmental implications of producing nitrous oxide gas on a large scale.

Q: What are some common applications of nitrous oxide gas?

A: Nitrous oxide gas is commonly used as an anesthetic in medical procedures, as a propellant in aerosol cans, and as a fuel in rocket engines.

Q: Can I use this reaction to produce other gases?

A: No, this reaction is specific to producing nitrous oxide gas from nitrogen gas and oxygen gas. However, you can use this reaction as a starting point to produce other gases by modifying the reaction conditions or using different reactants.

Q: What are some common mistakes to avoid when working with this reaction?

A: Some common mistakes to avoid when working with this reaction include:

  • Not following the stoichiometry of the reaction
  • Not using the correct reactants
  • Not controlling the reaction conditions
  • Not handling the reactants and products safely

Q: Where can I find more information about this reaction?

A: You can find more information about this reaction in chemistry textbooks, online resources, and scientific articles.

Q: Can I use this reaction to produce nitrous oxide gas in a laboratory setting?

A: Yes, you can use this reaction to produce nitrous oxide gas in a laboratory setting. However, you need to follow proper laboratory safety protocols and obtain any necessary permits or approvals.

Q: What are some common laboratory techniques used to produce nitrous oxide gas?

A: Some common laboratory techniques used to produce nitrous oxide gas include:

  • Using a gas generator to produce nitrous oxide gas
  • Using a reaction vessel to produce nitrous oxide gas
  • Using a gas chromatograph to analyze the nitrous oxide gas

Q: Can I use this reaction to produce nitrous oxide gas in a industrial setting?

A: Yes, you can use this reaction to produce nitrous oxide gas in an industrial setting. However, you need to follow proper industrial safety protocols and obtain any necessary permits or approvals.

Q: What are some common industrial techniques used to produce nitrous oxide gas?

A: Some common industrial techniques used to produce nitrous oxide gas include:

  • Using a gas generator to produce nitrous oxide gas
  • Using a reaction vessel to produce nitrous oxide gas
  • Using a gas compressor to compress the nitrous oxide gas

Q: Can I use this reaction to produce other gases in an industrial setting?

A: Yes, you can use this reaction as a starting point to produce other gases in an industrial setting. However, you need to modify the reaction conditions or use different reactants to produce the desired gas.