The Following Balanced Equation Shows The Formation Of Ammonia. N 2 + 3 H 2 → 2 N H 3 N_2 + 3 H_2 \rightarrow 2 NH_3 N 2 + 3 H 2 → 2 N H 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

Mar 7, 2025 by ADMIN 279 views

**The Formation of Ammonia: Balancing Chemical Equations and Stoichiometry**

Understanding the Balanced Equation

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

$N_2 + 3 H_2 \rightarrow 2 NH_3$

This equation indicates that one mole of nitrogen gas ( $N_2$ ) reacts with three moles of hydrogen gas ( $H_2$ ) to produce two moles of ammonia ( $NH_3$ ).

Stoichiometry and Mole Ratios

To solve this problem, we need to apply the concept of stoichiometry, which is the study of the quantitative relationships between reactants and products in chemical reactions. In this case, we are given the amount of hydrogen gas (6.34 mol) and asked to find the amount of nitrogen gas needed to completely convert it.

From the balanced equation, we can see that the mole ratio of hydrogen to nitrogen is 3:1. This means that for every 3 moles of hydrogen, 1 mole of nitrogen is required.

Calculating the Moles of Nitrogen Needed

To find the moles of nitrogen needed, we can use the mole ratio and the given amount of hydrogen.

Let's start by dividing the given amount of hydrogen (6.34 mol) by the mole ratio of hydrogen to nitrogen (3).

$6.34 \, \text{mol} \, H_2 \div 3 = 2.11 \, \text{mol} \, H_2$

Since the mole ratio is 3:1, we can multiply the result by 1 to find the moles of nitrogen needed.

$2.11 \, \text{mol} \, H_2 \times 1 = 2.11 \, \text{mol} \, N_2$

Therefore, the moles of nitrogen needed to completely convert 6.34 mol of hydrogen is 2.11 mol.

Conclusion

In conclusion, the balanced equation for the formation of ammonia shows that one mole of nitrogen gas reacts with three moles of hydrogen gas to produce two moles of ammonia. By applying the concept of stoichiometry and mole ratios, we can calculate the moles of nitrogen needed to completely convert a given amount of hydrogen. In this case, we found that 2.11 mol of nitrogen is needed to convert 6.34 mol of hydrogen.

Answer

The correct answer is B. 2.11 mol.

Additional Practice Problems

How many moles of ammonia are produced when 4.23 mol of nitrogen gas reacts with 12.69 mol of hydrogen gas?
How many moles of hydrogen gas are required to produce 5.67 mol of ammonia?
How many moles of nitrogen gas are needed to completely convert 8.45 mol of hydrogen gas?

Solutions

$N_2 + 3 H_2 \rightarrow 2 NH_3$ $4.23 \, \text{mol} \, N_2 \times 2 = 8.46 \, \text{mol} \, NH_3$
$N_2 + 3 H_2 \rightarrow 2 NH_3$ $5.67 \, \text{mol} \, NH_3 \div 2 = 2.835 \, \text{mol} \, N_2$ $2.835 \, \text{mol} \, N_2 \times 3 = 8.505 \, \text{mol} \, H_2$
$N_2 + 3 H_2 \rightarrow 2 NH_3$ $8.45 \, \text{mol} \, H_2 \div 3 = 2.817 \, \text{mol} \, H_2$ $2.817 \, \text{mol} \, H_2 \times 1 = 2.817 \, \text{mol} \, N_2$
The Formation of Ammonia: Q&A ================================

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

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

$N_2 + 3 H_2 \rightarrow 2 NH_3$

Q: What is the mole ratio of hydrogen to nitrogen in the balanced equation?

A: The mole ratio of hydrogen to nitrogen is 3:1. This means that for every 3 moles of hydrogen, 1 mole of nitrogen is required.

Q: How many moles of nitrogen are needed to completely convert 6.34 mol of hydrogen?

A: To find the moles of nitrogen needed, we can use the mole ratio and the given amount of hydrogen.

Let's start by dividing the given amount of hydrogen (6.34 mol) by the mole ratio of hydrogen to nitrogen (3).

$6.34 \, \text{mol} \, H_2 \div 3 = 2.11 \, \text{mol} \, H_2$

Since the mole ratio is 3:1, we can multiply the result by 1 to find the moles of nitrogen needed.

$2.11 \, \text{mol} \, H_2 \times 1 = 2.11 \, \text{mol} \, N_2$

Therefore, the moles of nitrogen needed to completely convert 6.34 mol of hydrogen is 2.11 mol.

Q: How many moles of ammonia are produced when 4.23 mol of nitrogen gas reacts with 12.69 mol of hydrogen gas?

A: To find the moles of ammonia produced, we can use the mole ratio and the given amounts of nitrogen and hydrogen.

From the balanced equation, we can see that the mole ratio of nitrogen to ammonia is 1:2. This means that for every 1 mole of nitrogen, 2 moles of ammonia are produced.

Let's start by dividing the given amount of nitrogen (4.23 mol) by the mole ratio of nitrogen to ammonia (1).

$4.23 \, \text{mol} \, N_2 \div 1 = 4.23 \, \text{mol} \, NH_3$

Since the mole ratio is 1:2, we can multiply the result by 2 to find the moles of ammonia produced.

$4.23 \, \text{mol} \, N_2 \times 2 = 8.46 \, \text{mol} \, NH_3$

Therefore, the moles of ammonia produced when 4.23 mol of nitrogen gas reacts with 12.69 mol of hydrogen gas is 8.46 mol.

Q: How many moles of hydrogen gas are required to produce 5.67 mol of ammonia?

A: To find the moles of hydrogen gas required, we can use the mole ratio and the given amount of ammonia.

From the balanced equation, we can see that the mole ratio of ammonia to hydrogen is 2:3. This means that for every 2 moles of ammonia, 3 moles of hydrogen are required.

Let's start by dividing the given amount of ammonia (5.67 mol) by the mole ratio of ammonia to hydrogen (2).

$5.67 \, \text{mol} \, NH_3 \div 2 = 2.835 \, \text{mol} \, NH_3$

Since the mole ratio is 2:3, we can multiply the result by 3 to find the moles of hydrogen gas required.

$2.835 \, \text{mol} \, NH_3 \times 3 = 8.505 \, \text{mol} \, H_2$

Therefore, the moles of hydrogen gas required to produce 5.67 mol of ammonia is 8.505 mol.

Q: How many moles of nitrogen gas are needed to completely convert 8.45 mol of hydrogen gas?

A: To find the moles of nitrogen gas needed, we can use the mole ratio and the given amount of hydrogen.

From the balanced equation, we can see that the mole ratio of hydrogen to nitrogen is 3:1. This means that for every 3 moles of hydrogen, 1 mole of nitrogen is required.

Let's start by dividing the given amount of hydrogen (8.45 mol) by the mole ratio of hydrogen to nitrogen (3).

$8.45 \, \text{mol} \, H_2 \div 3 = 2.817 \, \text{mol} \, H_2$

Since the mole ratio is 3:1, we can multiply the result by 1 to find the moles of nitrogen gas needed.

$2.817 \, \text{mol} \, H_2 \times 1 = 2.817 \, \text{mol} \, N_2$

Therefore, the moles of nitrogen gas needed to completely convert 8.45 mol of hydrogen gas is 2.817 mol.

Conclusion

In conclusion, the balanced equation for the formation of ammonia shows that one mole of nitrogen gas reacts with three moles of hydrogen gas to produce two moles of ammonia. By applying the concept of stoichiometry and mole ratios, we can calculate the moles of nitrogen needed to completely convert a given amount of hydrogen. We can also use the mole ratio to find the moles of ammonia produced when a given amount of nitrogen and hydrogen react.

Additional Practice Problems

How many moles of ammonia are produced when 3.14 mol of nitrogen gas reacts with 9.42 mol of hydrogen gas?
How many moles of hydrogen gas are required to produce 4.23 mol of ammonia?
How many moles of nitrogen gas are needed to completely convert 6.67 mol of hydrogen gas?

Solutions

$N_2 + 3 H_2 \rightarrow 2 NH_3$ $3.14 \, \text{mol} \, N_2 \times 2 = 6.28 \, \text{mol} \, NH_3$
$N_2 + 3 H_2 \rightarrow 2 NH_3$ $4.23 \, \text{mol} \, NH_3 \div 2 = 2.115 \, \text{mol} \, NH_3$ $2.115 \, \text{mol} \, NH_3 \times 3 = 6.345 \, \text{mol} \, H_2$
$N_2 + 3 H_2 \rightarrow 2 NH_3$ $6.67 \, \text{mol} \, H_2 \div 3 = 2.223 \, \text{mol} \, H_2$ $2.223 \, \text{mol} \, H_2 \times 1 = 2.223 \, \text{mol} \, N_2$