Determine How Many Grams Of Hydrogen Are Needed To Produce 28.65 G Of Ammonia In The Following Reaction:$\[ N_2(g) + 3H_2(g) \rightarrow 2NH_3(g) \\]

Understanding the Chemical Reaction

In this article, we will explore the chemical reaction between nitrogen and hydrogen to produce ammonia. The reaction is as follows:

${ N_2(g) + 3H_2(g) \rightarrow 2NH_3(g) }$

This reaction is a classic example of a synthesis reaction, where two reactants combine to form a single product. In this case, nitrogen gas (N2) reacts with hydrogen gas (H2) to produce ammonia gas (NH3).

Balancing the Chemical Equation

Before we can determine the amount of hydrogen needed to produce ammonia, we need to balance the chemical equation. The balanced equation is:

${ N_2(g) + 3H_2(g) \rightarrow 2NH_3(g) }$

This equation shows that 1 mole of nitrogen gas reacts with 3 moles of hydrogen gas to produce 2 moles of ammonia gas.

Determining the Molar Mass of Ammonia

To determine the amount of hydrogen needed to produce ammonia, we need to know the molar mass of ammonia. The molar mass of ammonia is the sum of the atomic masses of nitrogen and hydrogen.

The atomic mass of nitrogen is 14.01 g/mol. The atomic mass of hydrogen is 1.01 g/mol.

The molar mass of ammonia is:

${ M_{NH_3} = 14.01 + 3(1.01) = 17.04 \, g/mol }$

Determining the Number of Moles of Ammonia

We are given that 28.65 g of ammonia is produced. To determine the number of moles of ammonia, we can use the formula:

${ n = \frac{m}{M} }$

where n is the number of moles, m is the mass of ammonia, and M is the molar mass of ammonia.

Plugging in the values, we get:

${ n = \frac{28.65}{17.04} = 1.68 \, mol }$

Determining the Number of Moles of Hydrogen

Since 3 moles of hydrogen gas are required to produce 2 moles of ammonia gas, we can determine the number of moles of hydrogen needed by multiplying the number of moles of ammonia by 3/2.

${ n_{H_2} = \frac{3}{2} n_{NH_3} = \frac{3}{2} (1.68) = 2.52 \, mol }$

Determining the Mass of Hydrogen

To determine the mass of hydrogen needed, we can use the formula:

${ m = nM }$

where m is the mass of hydrogen, n is the number of moles of hydrogen, and M is the molar mass of hydrogen.

The molar mass of hydrogen is 2.02 g/mol.

Plugging in the values, we get:

${ m = 2.52(2.02) = 5.12 \, g }$

Conclusion

In this article, we have determined the amount of hydrogen needed to produce 28.65 g of ammonia in the reaction:

${ N_2(g) + 3H_2(g) \rightarrow 2NH_3(g) }$

We have balanced the chemical equation, determined the molar mass of ammonia, determined the number of moles of ammonia, determined the number of moles of hydrogen, and determined the mass of hydrogen needed.

The results show that 5.12 g of hydrogen is needed to produce 28.65 g of ammonia.

References

• Chemistry: An Atoms First Approach. (2017). Cengage Learning.
• General Chemistry: Principles and Modern Applications. (2017). Cengage Learning.

Additional Resources

• Khan Academy: Chemical Reactions and Equations
• Chemistry LibreTexts: Chemical Reactions and Equations
  Frequently Asked Questions (FAQs) About Determining the Amount of Hydrogen Needed to Produce Ammonia =============================================================================================

Q: What is the chemical reaction between nitrogen and hydrogen to produce ammonia?

A: The chemical reaction between nitrogen and hydrogen to produce ammonia is:

${ N_2(g) + 3H_2(g) \rightarrow 2NH_3(g) }$

Q: Why is it necessary to balance the chemical equation?

A: Balancing the chemical equation is necessary to ensure that the number of atoms of each element is the same on both the reactant and product sides of the equation. This is important because it allows us to determine the correct stoichiometry of the reaction.

Q: How do you determine the molar mass of ammonia?

A: The molar mass of ammonia is determined by adding the atomic masses of nitrogen and hydrogen. The atomic mass of nitrogen is 14.01 g/mol, and the atomic mass of hydrogen is 1.01 g/mol. Therefore, the molar mass of ammonia is:

${ M_{NH_3} = 14.01 + 3(1.01) = 17.04 \, g/mol }$

Q: How do you determine the number of moles of ammonia produced?

A: To determine the number of moles of ammonia produced, we can use the formula:

${ n = \frac{m}{M} }$

where n is the number of moles, m is the mass of ammonia, and M is the molar mass of ammonia.

Q: How do you determine the number of moles of hydrogen needed?

A: Since 3 moles of hydrogen gas are required to produce 2 moles of ammonia gas, we can determine the number of moles of hydrogen needed by multiplying the number of moles of ammonia by 3/2.

${ n_{H_2} = \frac{3}{2} n_{NH_3} }$

Q: How do you determine the mass of hydrogen needed?

A: To determine the mass of hydrogen needed, we can use the formula:

${ m = nM }$

where m is the mass of hydrogen, n is the number of moles of hydrogen, and M is the molar mass of hydrogen.

Q: What is the significance of the stoichiometry of the reaction?

A: The stoichiometry of the reaction is important because it determines the ratio of reactants to products. In this case, the stoichiometry of the reaction is 1:3:2 (N2:H2:NH3). This means that for every 1 mole of nitrogen gas, 3 moles of hydrogen gas are required to produce 2 moles of ammonia gas.

Q: What are some common applications of ammonia?

A: Ammonia is a common industrial chemical that has many applications. Some of the most common applications of ammonia include:

• Fertilizers: Ammonia is used as a fertilizer in agriculture to promote plant growth.
• Cleaning agents: Ammonia is used as a cleaning agent in many household and industrial applications.
• Refrigeration: Ammonia is used as a refrigerant in some industrial applications.
• Pharmaceuticals: Ammonia is used as an intermediate in the production of some pharmaceuticals.

Q: What are some common hazards associated with ammonia?

A: Ammonia is a hazardous chemical that can cause a number of health and environmental problems. Some of the most common hazards associated with ammonia include:

• Respiratory problems: Ammonia can cause respiratory problems, including irritation of the eyes, nose, and throat.
• Skin and eye irritation: Ammonia can cause skin and eye irritation, including burns and ulcers.
• Environmental hazards: Ammonia can contaminate water and soil, causing environmental problems.

Q: How can I safely handle and store ammonia?

A: Ammonia is a hazardous chemical that requires careful handling and storage. Some of the most important safety precautions to take when handling and storing ammonia include:

• Wear protective clothing and equipment, including gloves, goggles, and a face mask.
• Store ammonia in a well-ventilated area, away from heat sources and open flames.
• Use a spill kit to clean up any spills or leaks.
• Follow all local, state, and federal regulations for the handling and storage of ammonia.