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 be discussing 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 or more substances combine to form a new compound. 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:

${ N_2(g) + 6H_2(g) \rightarrow 4NH_3(g) }$

However, in this problem, we are given the unbalanced equation:

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

We will use this equation to determine the amount of hydrogen needed to produce ammonia.

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, and the atomic mass of hydrogen is 1.01 g/mol. Therefore, the molar mass of ammonia is:

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

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:

${ n_{NH_3} = \frac{28.65}{17.04} = 1.68 \, mol }$

Determining the Number of Moles of Hydrogen

From the balanced equation, we can see that 6 moles of hydrogen are needed to produce 4 moles of ammonia. Therefore, the number of moles of hydrogen needed to produce 1.68 moles of ammonia is:

${ n_{H_2} = \frac{6}{4} \times 1.68 = 2.52 \, mol }$

Determining the Mass of Hydrogen

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

${ m = n \times M }$

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:

${ m_{H_2} = 2.52 \times 2.02 = 5.10 \, g }$

Therefore, 5.10 g of hydrogen is needed to produce 28.65 g of ammonia.

Conclusion

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

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

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 important to balance the chemical equation?

A: Balancing the chemical equation is important because it ensures that the number of atoms of each element is the same on both the reactant and product sides of the equation. This is necessary to accurately determine the amount of reactants and products involved in the reaction.

Q: How do you determine the molar mass of a compound?

A: To determine the molar mass of a compound, you need to add up the atomic masses of all the atoms in the compound. For example, the molar mass of ammonia (NH3) is:

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

Q: How do you determine the number of moles of a substance?

A: To determine the number of moles of a substance, you can use the formula:

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

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

Q: What is the difference between a mole and a gram?

A: A mole is a unit of measurement that represents 6.022 x 10^23 particles (atoms or molecules), while a gram is a unit of mass. For example, 1 mole of hydrogen gas has a mass of 2.02 grams.

Q: How do you determine the mass of a substance from its number of moles?

A: To determine the mass of a substance from its number of moles, you can use the formula:

${ m = n \times M }$

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

Q: What is the significance of the balanced chemical equation in this problem?

A: The balanced chemical equation is significant because it allows us to accurately determine the amount of reactants and products involved in the reaction. In this problem, the balanced equation is:

${ N_2(g) + 6H_2(g) \rightarrow 4NH_3(g) }$

However, we are given the unbalanced equation:

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

We use this equation to determine the amount of hydrogen needed to produce ammonia.

Q: What is the final answer to the problem?

A: The final answer to the problem is that 5.10 g of hydrogen is needed to produce 28.65 g of ammonia.

Q: What are some real-world applications of the chemical reaction between nitrogen and hydrogen to produce ammonia?

A: The chemical reaction between nitrogen and hydrogen to produce ammonia has many real-world applications, including:

• Fertilizer production: Ammonia is used as a fertilizer in agriculture to promote plant growth.
• Power generation: Ammonia can be used as a fuel source in power plants to generate electricity.
• Chemical synthesis: Ammonia is used as a reactant in the synthesis of many chemicals, including plastics and pharmaceuticals.

Q: What are some potential hazards associated with the chemical reaction between nitrogen and hydrogen to produce ammonia?

A: Some potential hazards associated with the chemical reaction between nitrogen and hydrogen to produce ammonia include:

• Explosion: The reaction can be explosive if not handled properly.
• Fire: The reaction can produce heat and flames if not controlled.
• Toxicity: Ammonia is toxic and can cause respiratory problems if inhaled.

It is essential to handle the reaction with caution and follow proper safety protocols to avoid any potential hazards.