The Following Balanced Equation Shows The Formation Of Ammonia:${ N_2 + 3H_2 \rightarrow 2NH_3 }$How Many Moles Of Nitrogen Are Needed To Completely Convert 6.34 Mol Of Hydrogen?A. 1.02 Mol B. 2.11 Mol C. 12.68 Mol D. 19.02 Mol

Understanding the Balanced Equation

The balanced equation for the formation of ammonia is given as:

${ N_2 + 3H_2 \rightarrow 2NH_3 }$

This equation shows that one mole of nitrogen gas (N2) reacts with three moles of hydrogen gas (H2) to produce two moles of ammonia (NH3).

Stoichiometry and Mole Ratios

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between reactants and products in chemical reactions. In this case, we are interested in the mole ratio between nitrogen and hydrogen.

From the balanced equation, we can see that 1 mole of N2 reacts with 3 moles of H2. This means that for every 1 mole of N2, 3 moles of H2 are required to produce 2 moles of NH3.

Calculating the Number of Moles of Nitrogen Needed

We are given that 6.34 mol of hydrogen (H2) is available. We need to calculate the number of moles of nitrogen (N2) required to completely convert this amount of hydrogen into ammonia.

To do this, we can use the mole ratio from the balanced equation. Since 3 moles of H2 are required to react with 1 mole of N2, we can set up a proportion to find the number of moles of N2 needed:

${ \frac{3 \text{ mol H}_2}{1 \text{ mol N}_2} = \frac{6.34 \text{ mol H}_2}{x \text{ mol N}_2} }$

Solving for x, we get:

${ x = \frac{6.34 \text{ mol H}_2 \times 1 \text{ mol N}_2}{3 \text{ mol H}_2} }$

${ x = 2.11 \text{ mol N}_2 }$

Conclusion

Therefore, 2.11 mol of nitrogen (N2) is needed to completely convert 6.34 mol of hydrogen (H2) into ammonia.

Discussion and Analysis

This problem requires a basic understanding of stoichiometry and mole ratios. The balanced equation provides the necessary information to calculate the number of moles of nitrogen required to react with a given amount of hydrogen.

In this case, the mole ratio from the balanced equation is used to set up a proportion and solve for the number of moles of nitrogen needed. This type of calculation is essential in chemistry, as it allows us to predict the amounts of reactants and products required in a chemical reaction.

Key Takeaways

• The balanced equation for the formation of ammonia is: N2 + 3H2 → 2NH3
• The mole ratio between nitrogen and hydrogen is 1:3
• To calculate the number of moles of nitrogen required, we can use the mole ratio and set up a proportion
• The number of moles of nitrogen needed to completely convert 6.34 mol of hydrogen is 2.11 mol

Additional Practice Problems

• If 4.21 mol of hydrogen is available, how many moles of nitrogen are required to completely convert it into ammonia?
• If 1.02 mol of nitrogen is available, how many moles of hydrogen are required to completely convert it into ammonia?

Solutions to Additional Practice Problems

• If 4.21 mol of hydrogen is available, we can use the mole ratio to calculate the number of moles of nitrogen required:

${ \frac{3 \text{ mol H}_2}{1 \text{ mol N}_2} = \frac{4.21 \text{ mol H}_2}{x \text{ mol N}_2} }$

Solving for x, we get:

${ x = \frac{4.21 \text{ mol H}_2 \times 1 \text{ mol N}_2}{3 \text{ mol H}_2} }$

${ x = 1.40 \text{ mol N}_2 }$

• If 1.02 mol of nitrogen is available, we can use the mole ratio to calculate the number of moles of hydrogen required:

${ \frac{3 \text{ mol H}_2}{1 \text{ mol N}_2} = \frac{y \text{ mol H}_2}{1.02 \text{ mol N}_2} }$

Solving for y, we get:

${ y = \frac{1.02 \text{ mol N}_2 \times 3 \text{ mol H}_2}{1 \text{ mol N}_2} }$

${ y = 3.06 \text{ mol H}_2 }$

Conclusion

In conclusion, the balanced equation for the formation of ammonia provides the necessary information to calculate the number of moles of nitrogen required to react with a given amount of hydrogen. The mole ratio from the balanced equation is used to set up a proportion and solve for the number of moles of nitrogen needed. This type of calculation is essential in chemistry, as it allows us to predict the amounts of reactants and products required in a chemical reaction.

Frequently Asked Questions

Q: What is the balanced equation for the formation of ammonia?

A: The balanced equation for the formation of ammonia is:

${ N_2 + 3H_2 \rightarrow 2NH_3 }$

Q: What is the mole ratio between nitrogen and hydrogen in the balanced equation?

A: The mole ratio between nitrogen and hydrogen is 1:3, meaning that 1 mole of nitrogen reacts with 3 moles of hydrogen.

Q: How do I calculate the number of moles of nitrogen required to react with a given amount of hydrogen?

A: To calculate the number of moles of nitrogen required, you can use the mole ratio from the balanced equation and set up a proportion. For example, if you have 6.34 mol of hydrogen, you can use the following proportion:

${ \frac{3 \text{ mol H}_2}{1 \text{ mol N}_2} = \frac{6.34 \text{ mol H}_2}{x \text{ mol N}_2} }$

Solving for x, you get:

${ x = \frac{6.34 \text{ mol H}_2 \times 1 \text{ mol N}_2}{3 \text{ mol H}_2} }$

${ x = 2.11 \text{ mol N}_2 }$

Q: What is the relationship between the number of moles of nitrogen and the number of moles of hydrogen in a chemical reaction?

A: In a chemical reaction, the number of moles of nitrogen and the number of moles of hydrogen are related by the mole ratio from the balanced equation. This means that for every 1 mole of nitrogen, 3 moles of hydrogen are required to react.

Q: How do I determine the limiting reactant in a chemical reaction?

A: To determine the limiting reactant in a chemical reaction, you need to compare the mole ratio of the reactants to the mole ratio from the balanced equation. The reactant that is present in the smallest amount relative to the mole ratio is the limiting reactant.

Q: What is the significance of stoichiometry in chemistry?

A: Stoichiometry is the branch of chemistry that deals with the quantitative relationships between reactants and products in chemical reactions. It is essential in chemistry because it allows us to predict the amounts of reactants and products required in a chemical reaction.

Q: How do I calculate the number of moles of a product in a chemical reaction?

A: To calculate the number of moles of a product in a chemical reaction, you need to know the mole ratio of the product to the reactant and the number of moles of the reactant. You can use the following proportion:

${ \frac{\text{mole ratio of product to reactant}}{\text{number of moles of reactant}} = \text{number of moles of product} }$

For example, if you have 2.11 mol of nitrogen and the mole ratio of ammonia to nitrogen is 2:1, you can calculate the number of moles of ammonia as follows:

${ \frac{2 \text{ mol NH}_3}{1 \text{ mol N}_2} = \frac{2.11 \text{ mol N}_2}{x \text{ mol NH}_3} }$

Solving for x, you get:

${ x = \frac{2.11 \text{ mol N}_2 \times 2 \text{ mol NH}_3}{1 \text{ mol N}_2} }$

${ x = 4.22 \text{ mol NH}_3 }$

Q: What is the difference between a limiting reactant and an excess reactant?

A: A limiting reactant is the reactant that is present in the smallest amount relative to the mole ratio, while an excess reactant is the reactant that is present in excess of the amount required to react with the limiting reactant.

Q: How do I determine the amount of excess reactant in a chemical reaction?

A: To determine the amount of excess reactant in a chemical reaction, you need to compare the mole ratio of the reactants to the mole ratio from the balanced equation. The reactant that is present in excess of the amount required to react with the limiting reactant is the excess reactant.

Q: What is the significance of excess reactant in a chemical reaction?

A: Excess reactant is the reactant that is present in excess of the amount required to react with the limiting reactant. It is not consumed in the reaction and is left over at the end of the reaction.

Q: How do I calculate the amount of excess reactant in a chemical reaction?

A: To calculate the amount of excess reactant in a chemical reaction, you need to know the mole ratio of the reactants to the product and the number of moles of the product. You can use the following proportion:

${ \frac{\text{mole ratio of reactants to product}}{\text{number of moles of product}} = \text{number of moles of excess reactant} }$

For example, if you have 4.22 mol of ammonia and the mole ratio of ammonia to nitrogen is 2:1, you can calculate the number of moles of excess nitrogen as follows:

${ \frac{2 \text{ mol N}_2}{1 \text{ mol NH}_3} = \frac{4.22 \text{ mol NH}_3}{x \text{ mol N}_2} }$

Solving for x, you get:

${ x = \frac{4.22 \text{ mol NH}_3 \times 2 \text{ mol N}_2}{1 \text{ mol NH}_3} }$

${ x = 8.44 \text{ mol N}_2 }$

The excess nitrogen is 8.44 mol - 2.11 mol = 6.33 mol.

Q: What is the difference between a product and a byproduct in a chemical reaction?

A: A product is the substance that is formed as a result of a chemical reaction, while a byproduct is a substance that is formed as a result of a side reaction or a secondary reaction.

Q: How do I determine the amount of product in a chemical reaction?

A: To determine the amount of product in a chemical reaction, you need to know the mole ratio of the reactants to the product and the number of moles of the reactants. You can use the following proportion:

${ \frac{\text{mole ratio of reactants to product}}{\text{number of moles of reactants}} = \text{number of moles of product} }$

For example, if you have 2.11 mol of nitrogen and the mole ratio of ammonia to nitrogen is 2:1, you can calculate the number of moles of ammonia as follows:

${ \frac{2 \text{ mol NH}_3}{1 \text{ mol N}_2} = \frac{2.11 \text{ mol N}_2}{x \text{ mol NH}_3} }$

Solving for x, you get:

${ x = \frac{2.11 \text{ mol N}_2 \times 2 \text{ mol NH}_3}{1 \text{ mol N}_2} }$

${ x = 4.22 \text{ mol NH}_3 }$

Q: What is the significance of the mole ratio in a chemical reaction?

A: The mole ratio is the ratio of the number of moles of one substance to the number of moles of another substance in a chemical reaction. It is essential in chemistry because it allows us to predict the amounts of reactants and products required in a chemical reaction.

Q: How do I calculate the mole ratio in a chemical reaction?

A: To calculate the mole ratio in a chemical reaction, you need to know the number of moles of the reactants and the number of moles of the products. You can use the following proportion:

${ \frac{\text{number of moles of reactant 1}}{\text{number of moles of reactant 2}} = \frac{\text{number of moles of product 1}}{\text{number of moles of product 2}} }$

For example, if you have 2.11 mol of nitrogen and 4.22 mol of ammonia, you can calculate the mole ratio as follows:

${ \frac{2.11 \text{ mol N}_2}{4.22 \text{ mol NH}_3} = \frac{1}{2} }$

This means that the mole ratio of nitrogen to ammonia is 1:2.

Q: What is the significance of the mole ratio in a chemical reaction?

A: The mole ratio is the ratio of the number of moles of one substance to the number of moles of another substance in a chemical reaction. It is essential in chemistry because it allows us to predict the amounts of reactants and products required in a chemical reaction.

Q: How do I determine the limiting reactant in a chemical reaction?

A: To determine the limiting reactant in a chemical reaction, you need to compare the mole ratio of the reactants to the mole ratio from the balanced equation. The reactant that is present in the smallest amount relative to the mole ratio is the limiting reactant.

Q: What is the significance of the limiting reactant in a chemical reaction?

A: The limiting reactant is the reactant that is present in the smallest amount relative to the mole ratio. It is the reactant that determines the amount of product that can be formed in a chemical reaction.

Q: How do I calculate the amount of product