Write The Molar Ratios For The Following Reaction:$\[ 4 \text{NH}_3 + 3 \text{O}_2 \rightarrow 2 \text{N}_2 + 6 \text{H}_2\text{O} \\]Determine The Molar Ratios For:1. \[$\text{NH}_3\$\] To \[$\text{N}_2\$\]2.

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Molar ratios are a fundamental concept in chemistry that describe the quantitative relationship between the reactants and products in a chemical reaction. In this article, we will explore the molar ratios for a given reaction and discuss how to determine them.

The Reaction

The given reaction is:

4NH3+3O2→2N2+6H2O{ 4 \text{NH}_3 + 3 \text{O}_2 \rightarrow 2 \text{N}_2 + 6 \text{H}_2\text{O} }

This reaction involves the combustion of ammonia (NH3) in the presence of oxygen (O2) to produce nitrogen gas (N2) and water (H2O).

Determining Molar Ratios

To determine the molar ratios for the given reaction, we need to identify the number of moles of each reactant and product. The molar ratio is then calculated by dividing the number of moles of one substance by the number of moles of another substance.

1. Molar Ratio of NH3 to N2

To determine the molar ratio of NH3 to N2, we need to identify the number of moles of each substance in the reaction.

  • NH3: 4 moles
  • N2: 2 moles

The molar ratio of NH3 to N2 is calculated by dividing the number of moles of NH3 by the number of moles of N2:

Molar Ratio of NH3 to N2=4 moles NH32 moles N2=2:1{ \text{Molar Ratio of NH}_3 \text{ to N}_2 = \frac{4 \text{ moles NH}_3}{2 \text{ moles N}_2} = 2:1 }

This means that for every 2 moles of N2 produced, 4 moles of NH3 are required.

2. Molar Ratio of NH3 to H2O

To determine the molar ratio of NH3 to H2O, we need to identify the number of moles of each substance in the reaction.

  • NH3: 4 moles
  • H2O: 6 moles

The molar ratio of NH3 to H2O is calculated by dividing the number of moles of NH3 by the number of moles of H2O:

Molar Ratio of NH3 to H2O=4 moles NH36 moles H2O=2:3{ \text{Molar Ratio of NH}_3 \text{ to H}_2\text{O} = \frac{4 \text{ moles NH}_3}{6 \text{ moles H}_2\text{O}} = 2:3 }

This means that for every 3 moles of H2O produced, 2 moles of NH3 are required.

3. Molar Ratio of O2 to N2

To determine the molar ratio of O2 to N2, we need to identify the number of moles of each substance in the reaction.

  • O2: 3 moles
  • N2: 2 moles

The molar ratio of O2 to N2 is calculated by dividing the number of moles of O2 by the number of moles of N2:

Molar Ratio of O2 to N2=3 moles O22 moles N2=1.5:1{ \text{Molar Ratio of O}_2 \text{ to N}_2 = \frac{3 \text{ moles O}_2}{2 \text{ moles N}_2} = 1.5:1 }

This means that for every 1 mole of N2 produced, 1.5 moles of O2 are required.

4. Molar Ratio of O2 to H2O

To determine the molar ratio of O2 to H2O, we need to identify the number of moles of each substance in the reaction.

  • O2: 3 moles
  • H2O: 6 moles

The molar ratio of O2 to H2O is calculated by dividing the number of moles of O2 by the number of moles of H2O:

Molar Ratio of O2 to H2O=3 moles O26 moles H2O=1:2{ \text{Molar Ratio of O}_2 \text{ to H}_2\text{O} = \frac{3 \text{ moles O}_2}{6 \text{ moles H}_2\text{O}} = 1:2 }

This means that for every 2 moles of H2O produced, 1 mole of O2 is required.

Conclusion

In conclusion, the molar ratios for the given reaction are:

  • NH3 to N2: 2:1
  • NH3 to H2O: 2:3
  • O2 to N2: 1.5:1
  • O2 to H2O: 1:2

These molar ratios provide a quantitative relationship between the reactants and products in the reaction, which is essential for understanding the stoichiometry of the reaction.

Applications of Molar Ratios

Molar ratios have numerous applications in chemistry, including:

  • Stoichiometry: Molar ratios are used to calculate the amount of reactants and products required for a chemical reaction.
  • Chemical Equilibrium: Molar ratios are used to determine the equilibrium constant (K) for a chemical reaction.
  • Chemical Reactions: Molar ratios are used to predict the products and reactants of a chemical reaction.
  • Chemical Synthesis: Molar ratios are used to optimize the yield and purity of a chemical product.

Limitations of Molar Ratios

While molar ratios are a powerful tool in chemistry, they have some limitations:

  • Assumes Ideal Behavior: Molar ratios assume that the reactants and products behave ideally, which is not always the case.
  • Does Not Account for Impurities: Molar ratios do not account for impurities in the reactants and products.
  • Does Not Account for Temperature and Pressure: Molar ratios do not account for changes in temperature and pressure.

Future Directions

In conclusion, molar ratios are a fundamental concept in chemistry that provides a quantitative relationship between the reactants and products in a chemical reaction. While molar ratios have numerous applications, they also have some limitations. Future research should focus on developing more accurate and comprehensive models that account for the complexities of chemical reactions.

References

  • Chemical Equilibrium: Atkins, P. W., & de Paula, J. (2010). Physical Chemistry (9th ed.). Oxford University Press.
  • Chemical Reactions: Brown, T. E., LeMay, H. E., Bursten, B. E., & Murphy, C. (2012). Chemistry: The Central Science (12th ed.). Pearson Education.
  • Chemical Synthesis: Smith, J. G., & March, J. (2007). March's Advanced Organic Chemistry: Reactions, Mechanisms, and Structure (7th ed.). Wiley-Interscience.