What Mass, In Grams, Of NO Will Be Produced From 28.0 G Of N O 2 NO_2 N O 2 ​ Reacted With Excess Water In The Following Chemical Reaction?${ 3 , NO_2(g) + H_2O(l) \rightarrow 2 , HNO_3(g) + NO(g) }$

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What Mass of NO Will Be Produced from NO2 Reacted with Excess Water?

Understanding the Chemical Reaction

The given chemical reaction is: 3 NO2(g)+H2O(l)→2 HNO3(g)+NO(g){ 3 \, NO_2(g) + H_2O(l) \rightarrow 2 \, HNO_3(g) + NO(g) }

In this reaction, nitrogen dioxide (NO2NO_2) reacts with water (H2OH_2O) to produce nitric acid (HNO3HNO_3) and nitrogen monoxide (NONO). The reaction is as follows:

  • 3 moles of NO2NO_2 react with 1 mole of H2OH_2O to produce 2 moles of HNO3HNO_3 and 1 mole of NONO.

Calculating the Mass of NO Produced

To calculate the mass of NONO produced from 28.0 g of NO2NO_2, we need to follow these steps:

  1. Determine the Molar Mass of NO2 and NO

The molar mass of NO2NO_2 is 46.01 g/mol (14.01 g/mol for nitrogen and 32.00 g/mol for oxygen).

The molar mass of NONO is 30.01 g/mol (14.01 g/mol for nitrogen and 16.00 g/mol for oxygen).

  1. Calculate the Number of Moles of NO2

We can calculate the number of moles of NO2NO_2 using the given mass (28.0 g) and the molar mass (46.01 g/mol).

Number of moles of NO2=Mass of NO2Molar mass of NO2{ \text{Number of moles of } NO_2 = \frac{\text{Mass of } NO_2}{\text{Molar mass of } NO_2} }

Number of moles of NO2=28.0 g46.01 g/mol{ \text{Number of moles of } NO_2 = \frac{28.0 \, \text{g}}{46.01 \, \text{g/mol}} }

Number of moles of NO2=0.609 mol{ \text{Number of moles of } NO_2 = 0.609 \, \text{mol} }

  1. Determine the Mole Ratio of NO2 to NO

From the balanced chemical equation, we can see that 3 moles of NO2NO_2 produce 1 mole of NONO. Therefore, the mole ratio of NO2NO_2 to NONO is 3:1.

  1. Calculate the Number of Moles of NO Produced

We can calculate the number of moles of NONO produced using the number of moles of NO2NO_2 and the mole ratio.

Number of moles of NO=Number of moles of NO23{ \text{Number of moles of } NO = \frac{\text{Number of moles of } NO_2}{3} }

Number of moles of NO=0.609 mol3{ \text{Number of moles of } NO = \frac{0.609 \, \text{mol}}{3} }

Number of moles of NO=0.203 mol{ \text{Number of moles of } NO = 0.203 \, \text{mol} }

  1. Calculate the Mass of NO Produced

We can calculate the mass of NONO produced using the number of moles of NONO and the molar mass of NONO.

Mass of NO=Number of moles of NO×Molar mass of NO{ \text{Mass of } NO = \text{Number of moles of } NO \times \text{Molar mass of } NO }

Mass of NO=0.203 mol×30.01 g/mol{ \text{Mass of } NO = 0.203 \, \text{mol} \times 30.01 \, \text{g/mol} }

Mass of NO=6.11 g{ \text{Mass of } NO = 6.11 \, \text{g} }

Conclusion

In conclusion, the mass of NONO produced from 28.0 g of NO2NO_2 reacted with excess water is 6.11 g.

Additional Information

  • The balanced chemical equation shows that 3 moles of NO2NO_2 react with 1 mole of H2OH_2O to produce 2 moles of HNO3HNO_3 and 1 mole of NONO.
  • The mole ratio of NO2NO_2 to NONO is 3:1.
  • The molar mass of NO2NO_2 is 46.01 g/mol, and the molar mass of NONO is 30.01 g/mol.

References

  • Chemistry textbook by Brown, LeMay, and Bursten
  • Online resources for chemistry calculations and conversions
    Q&A: What Mass of NO Will Be Produced from NO2 Reacted with Excess Water?

Frequently Asked Questions

Q: What is the chemical reaction between NO2 and H2O?

A: The chemical reaction between NO2NO_2 and H2OH_2O is: 3 NO2(g)+H2O(l)→2 HNO3(g)+NO(g){ 3 \, NO_2(g) + H_2O(l) \rightarrow 2 \, HNO_3(g) + NO(g) }

Q: What is the mole ratio of NO2 to NO in the reaction?

A: The mole ratio of NO2NO_2 to NONO in the reaction is 3:1.

Q: How do I calculate the mass of NO produced from a given mass of NO2?

A: To calculate the mass of NONO produced from a given mass of NO2NO_2, you need to follow these steps:

  1. Determine the molar mass of NO2NO_2 and NONO.
  2. Calculate the number of moles of NO2NO_2 using the given mass and the molar mass.
  3. Determine the mole ratio of NO2NO_2 to NONO.
  4. Calculate the number of moles of NONO produced using the number of moles of NO2NO_2 and the mole ratio.
  5. Calculate the mass of NONO produced using the number of moles of NONO and the molar mass.

Q: What is the molar mass of NO2 and NO?

A: The molar mass of NO2NO_2 is 46.01 g/mol, and the molar mass of NONO is 30.01 g/mol.

Q: How do I calculate the number of moles of NO2 from a given mass?

A: To calculate the number of moles of NO2NO_2 from a given mass, you can use the following formula:

Number of moles of NO2=Mass of NO2Molar mass of NO2{ \text{Number of moles of } NO_2 = \frac{\text{Mass of } NO_2}{\text{Molar mass of } NO_2} }

Q: What is the mass of NO produced from 28.0 g of NO2?

A: The mass of NONO produced from 28.0 g of NO2NO_2 is 6.11 g.

Q: Can I use this calculation for other masses of NO2?

A: Yes, you can use this calculation for other masses of NO2NO_2 by following the same steps and using the correct mass of NO2NO_2.

Q: What are the limitations of this calculation?

A: The limitations of this calculation are:

  • The calculation assumes that the reaction is carried out under ideal conditions, with no losses or impurities.
  • The calculation assumes that the molar masses of NO2NO_2 and NONO are accurate.
  • The calculation assumes that the mole ratio of NO2NO_2 to NONO is 3:1.

Q: How can I improve the accuracy of this calculation?

A: To improve the accuracy of this calculation, you can:

  • Use more accurate values for the molar masses of NO2NO_2 and NONO.
  • Account for any losses or impurities in the reaction.
  • Use a more precise method for calculating the number of moles of NO2NO_2.

Conclusion

In conclusion, the mass of NONO produced from 28.0 g of NO2NO_2 reacted with excess water is 6.11 g. This calculation can be used for other masses of NO2NO_2 by following the same steps and using the correct mass of NO2NO_2. However, the accuracy of this calculation depends on the accuracy of the molar masses of NO2NO_2 and NONO, as well as any losses or impurities in the reaction.