About How Many Grams Of $H_2O$ Will Be Produced From 150 Grams Of $Fe_2O_3$?$ \text{Chemical Reaction Fe_2O_3 + 3H_2 \rightarrow 2Fe + 3H_2O }$

Introduction

Chemical reactions are the foundation of various industrial processes, including the production of hydrogen gas and water. In this article, we will delve into the chemical reaction between iron(III) oxide ($Fe_2O_3$) and hydrogen gas ($H_2$) to produce iron ($Fe$) and water ($H_2O$). We will calculate the amount of water produced from 150 grams of $Fe_2O_3$ using the given chemical reaction.

Chemical Reaction

The chemical reaction between $Fe_2O_3$ and $H_2$ is as follows:

$$Fe_2O_3 + 3H_2 \rightarrow 2Fe + 3H_2O$$

In this reaction, one mole of $Fe_2O_3$ reacts with three moles of $H_2$ to produce two moles of $Fe$ and three moles of $H_2O$.

Molar Mass Calculations

To calculate the amount of water produced, we need to determine the molar masses of $Fe_2O_3$ and $H_2O$. The molar masses are calculated as follows:

• Molar mass of $Fe_2O_3$ = 2(55.85 g/mol) + 3(16.00 g/mol) = 159.70 g/mol
• Molar mass of $H_2O$ = 2(1.01 g/mol) + 16.00 g/mol = 18.02 g/mol

Calculating the Number of Moles of $Fe_2O_3$

Given that we have 150 grams of $Fe_2O_3$, we can calculate the number of moles of $Fe_2O_3$ using the molar mass:

$$\text{Number of moles of } Fe_2O_3 = \frac{\text{Mass of } Fe_2O_3}{\text{Molar mass of } Fe_2O_3}$$

$$\text{Number of moles of } Fe_2O_3 = \frac{150\text{ g}}{159.70\text{ g/mol}} = 0.938\text{ mol}$$

Calculating the Number of Moles of $H_2O$ Produced

According to the chemical reaction, one mole of $Fe_2O_3$ produces three moles of $H_2O$. Therefore, the number of moles of $H_2O$ produced is:

$$\text{Number of moles of } H_2O = 3 \times \text{Number of moles of } Fe_2O_3$$

$$\text{Number of moles of } H_2O = 3 \times 0.938\text{ mol} = 2.814\text{ mol}$$

Calculating the Mass of $H_2O$ Produced

Now that we have the number of moles of $H_2O$ produced, we can calculate the mass of $H_2O$ produced using the molar mass:

$$\text{Mass of } H_2O = \text{Number of moles of } H_2O \times \text{Molar mass of } H_2O$$

$$\text{Mass of } H_2O = 2.814\text{ mol} \times 18.02\text{ g/mol} = 50.63\text{ g}$$

Conclusion

In this article, we calculated the amount of water produced from 150 grams of $Fe_2O_3$ using the given chemical reaction. We determined the molar masses of $Fe_2O_3$ and $H_2O$, calculated the number of moles of $Fe_2O_3$, and then calculated the number of moles of $H_2O$ produced. Finally, we calculated the mass of $H_2O$ produced using the molar mass of $H_2O$. The result shows that approximately 50.63 grams of $H_2O$ will be produced from 150 grams of $Fe_2O_3$.

References

• CRC Handbook of Chemistry and Physics, 97th Edition
• National Institute of Standards and Technology (NIST) Chemistry WebBook

Chemical Reaction Summary

Reactants	Products
$Fe_2O_3$	$2Fe$
$3H_2$	$3H_2O$

Molar Mass Summary

Substance	Molar Mass (g/mol)
$Fe_2O_3$	159.70
$H_2O$	18.02

Calculations Summary

Calculation	Result
Number of moles of $Fe_2O_3$	0.938 mol
Number of moles of $H_2O$ produced	2.814 mol
Mass of $H_2O$ produced	50.63 g

Frequently Asked Questions

Q: What is the chemical reaction between iron(III) oxide and hydrogen gas?

A: The chemical reaction between iron(III) oxide ($Fe_2O_3$) and hydrogen gas ($H_2$) is as follows:

$$Fe_2O_3 + 3H_2 \rightarrow 2Fe + 3H_2O$$

Q: What is the molar mass of iron(III) oxide?

A: The molar mass of iron(III) oxide ($Fe_2O_3$) is 159.70 g/mol.

Q: What is the molar mass of water?

A: The molar mass of water ($H_2O$) is 18.02 g/mol.

Q: How many moles of iron(III) oxide are in 150 grams of iron(III) oxide?

A: To calculate the number of moles of iron(III) oxide, we use the following formula:

$$\text{Number of moles of } Fe_2O_3 = \frac{\text{Mass of } Fe_2O_3}{\text{Molar mass of } Fe_2O_3}$$

$$\text{Number of moles of } Fe_2O_3 = \frac{150\text{ g}}{159.70\text{ g/mol}} = 0.938\text{ mol}$$

Q: How many moles of water are produced from 150 grams of iron(III) oxide?

A: According to the chemical reaction, one mole of iron(III) oxide produces three moles of water. Therefore, the number of moles of water produced is:

$$\text{Number of moles of } H_2O = 3 \times \text{Number of moles of } Fe_2O_3$$

$$\text{Number of moles of } H_2O = 3 \times 0.938\text{ mol} = 2.814\text{ mol}$$

Q: What is the mass of water produced from 150 grams of iron(III) oxide?

A: To calculate the mass of water produced, we use the following formula:

$$\text{Mass of } H_2O = \text{Number of moles of } H_2O \times \text{Molar mass of } H_2O$$

$$\text{Mass of } H_2O = 2.814\text{ mol} \times 18.02\text{ g/mol} = 50.63\text{ g}$$

Q: What is the purpose of the chemical reaction between iron(III) oxide and hydrogen gas?

A: The chemical reaction between iron(III) oxide and hydrogen gas is used to produce iron and water. The reaction is an example of a redox reaction, where iron(III) oxide is reduced to iron and hydrogen gas is oxidized to water.

Q: What are the applications of the chemical reaction between iron(III) oxide and hydrogen gas?

A: The chemical reaction between iron(III) oxide and hydrogen gas has various applications, including:

• Production of iron and water
• Redox reactions
• Industrial processes
• Chemical synthesis

Q: What are the safety precautions when handling iron(III) oxide and hydrogen gas?

A: When handling iron(III) oxide and hydrogen gas, it is essential to follow proper safety precautions, including:

• Wearing protective gear, such as gloves and goggles
• Working in a well-ventilated area
• Avoiding contact with skin and eyes
• Following proper handling and storage procedures

Q: What are the environmental implications of the chemical reaction between iron(III) oxide and hydrogen gas?

A: The chemical reaction between iron(III) oxide and hydrogen gas has minimal environmental implications, as it produces iron and water as byproducts. However, it is essential to follow proper waste disposal procedures and ensure that the reaction is carried out in a controlled environment.

Q: Can the chemical reaction between iron(III) oxide and hydrogen gas be used to produce other substances?

A: Yes, the chemical reaction between iron(III) oxide and hydrogen gas can be used to produce other substances, including:

• Iron
• Water
• Hydrogen gas
• Other iron compounds

Q: What are the limitations of the chemical reaction between iron(III) oxide and hydrogen gas?

A: The chemical reaction between iron(III) oxide and hydrogen gas has several limitations, including:

• Limited availability of iron(III) oxide
• Limited availability of hydrogen gas
• Requires controlled environment
• Requires proper handling and storage procedures

Q: Can the chemical reaction between iron(III) oxide and hydrogen gas be used in industrial processes?

A: Yes, the chemical reaction between iron(III) oxide and hydrogen gas can be used in various industrial processes, including:

• Production of iron and steel
• Production of hydrogen gas
• Redox reactions
• Chemical synthesis

Q: What are the advantages of the chemical reaction between iron(III) oxide and hydrogen gas?

A: The chemical reaction between iron(III) oxide and hydrogen gas has several advantages, including:

• Produces iron and water as byproducts
• Can be used in various industrial processes
• Can be used to produce other substances
• Has minimal environmental implications

Q: What are the disadvantages of the chemical reaction between iron(III) oxide and hydrogen gas?

A: The chemical reaction between iron(III) oxide and hydrogen gas has several disadvantages, including:

• Requires controlled environment
• Requires proper handling and storage procedures
• Limited availability of iron(III) oxide and hydrogen gas
• Requires specialized equipment and expertise