Calculating the Molar Mass of CO

Oct 13, 2025 by wbrum.org 33 views

Introduction

Chemical reactions involve the transformation of one or more substances into new substances, often accompanied by the release or absorption of heat energy. In this article, we will examine a specific chemical reaction and determine the amount of heat required to produce a given quantity of a product.

The Chemical Reaction

The given chemical reaction is:

${ H_2 + CO_2 + 9800 \text{ cal} \rightarrow H_2O + CO }$

This reaction involves the combination of hydrogen gas (H2) and carbon dioxide (CO2) to produce water (H2O) and carbon monoxide (CO). The reaction is exothermic, meaning that it releases heat energy, which is represented by the 9800 calories.

Calculating the Molar Mass of CO

To determine the amount of heat required to produce 2.0 grams of CO, we need to calculate the molar mass of CO. The atomic masses of carbon (C) and oxygen (O) are 12.01 g/mol and 16.00 g/mol, respectively.

The molar mass of CO is:

${ \text{Molar mass of CO} = 12.01 \text{ g/mol} + 16.00 \text{ g/mol} = 28.01 \text{ g/mol} }$

Determining the Number of Moles of CO

We are given that we want to produce 2.0 grams of CO. To determine the number of moles of CO, we can divide the given mass by the molar mass:

${ \text{Number of moles of CO} = \frac{2.0 \text{ g}}{28.01 \text{ g/mol}} = 0.0714 \text{ mol} }$

Calculating the Heat Required

The heat required to produce 2.0 grams of CO can be calculated using the following equation:

${ \text{Heat required} = \frac{\text{Number of moles of CO} \times \text{Heat of reaction}}{\text{Number of moles of CO produced per unit of heat}} }$

However, we are not given the heat of reaction or the number of moles of CO produced per unit of heat. Instead, we are given the total heat released in the reaction (9800 calories) and the mass of CO produced (2.0 grams).

To determine the heat required, we need to calculate the number of moles of CO produced per unit of heat. We can do this by dividing the number of moles of CO produced by the total heat released:

${ \text{Number of moles of CO produced per unit of heat} = \frac{0.0714 \text{ mol}}{9800 \text{ cal}} = 7.29 \times 10^{-6} \text{ mol/cal} }$

Now, we can calculate the heat required to produce 2.0 grams of CO:

${ \text{Heat required} = \frac{0.0714 \text{ mol} \times 9800 \text{ cal}}{7.29 \times 10^{-6} \text{ mol/cal}} = 700 \text{ cal} }$

Conclusion

In conclusion, the amount of heat required to produce 2.0 grams of CO is 700 calories. This is the correct answer.

Discussion

This problem requires a good understanding of chemical reactions, molar masses, and heat calculations. The key to solving this problem is to calculate the number of moles of CO produced per unit of heat and then use this value to determine the heat required to produce 2.0 grams of CO.

References

Chemistry textbook (e.g. "Chemistry: An Atoms First Approach" by Steven S. Zumdahl)
Online resources (e.g. Khan Academy, Chemistry LibreTexts)

Additional Resources

For more information on chemical reactions and heat calculations, see the following resources:

Khan Academy: Chemical Reactions and Stoichiometry
Chemistry LibreTexts: Chemical Reactions and Stoichiometry
Chemistry textbook (e.g. "Chemistry: An Atoms First Approach" by Steven S. Zumdahl)
Q&A: Understanding the Chemical Reaction and Heat Requirements ================================================================

Frequently Asked Questions

Q: What is the chemical reaction given in the problem?

A: The chemical reaction given in the problem is:

${ H_2 + CO_2 + 9800 \text{ cal} \rightarrow H_2O + CO }$

This reaction involves the combination of hydrogen gas (H2) and carbon dioxide (CO2) to produce water (H2O) and carbon monoxide (CO).

Q: What is the molar mass of CO?

A: The molar mass of CO is 28.01 g/mol.

Q: How do I calculate the number of moles of CO produced per unit of heat?

A: To calculate the number of moles of CO produced per unit of heat, you need to divide the number of moles of CO produced by the total heat released. In this case, the number of moles of CO produced is 0.0714 mol and the total heat released is 9800 cal.

${ \text{Number of moles of CO produced per unit of heat} = \frac{0.0714 \text{ mol}}{9800 \text{ cal}} = 7.29 \times 10^{-6} \text{ mol/cal} }$

Q: How do I calculate the heat required to produce 2.0 grams of CO?

A: To calculate the heat required to produce 2.0 grams of CO, you need to multiply the number of moles of CO produced by the heat of reaction. However, since we are not given the heat of reaction, we can use the number of moles of CO produced per unit of heat to calculate the heat required.

${ \text{Heat required} = \frac{0.0714 \text{ mol} \times 9800 \text{ cal}}{7.29 \times 10^{-6} \text{ mol/cal}} = 700 \text{ cal} }$

Q: What is the correct answer to the problem?

A: The correct answer to the problem is 700 calories.

Q: What is the significance of the heat of reaction in this problem?

A: The heat of reaction is the amount of heat released or absorbed during a chemical reaction. In this problem, the heat of reaction is 9800 cal. This value is used to calculate the number of moles of CO produced per unit of heat.

Q: How do I determine the number of moles of CO produced per unit of heat?

A: To determine the number of moles of CO produced per unit of heat, you need to divide the number of moles of CO produced by the total heat released.

Q: What is the relationship between the number of moles of CO produced and the heat required?

A: The number of moles of CO produced is directly proportional to the heat required. This means that as the number of moles of CO produced increases, the heat required also increases.

Q: How do I calculate the heat required to produce a given quantity of CO?

A: To calculate the heat required to produce a given quantity of CO, you need to multiply the number of moles of CO produced by the heat of reaction. However, since we are not given the heat of reaction, we can use the number of moles of CO produced per unit of heat to calculate the heat required.

Q: What is the significance of the molar mass of CO in this problem?

A: The molar mass of CO is used to calculate the number of moles of CO produced. This value is also used to determine the heat required to produce a given quantity of CO.

Q: How do I determine the number of moles of CO produced?

A: To determine the number of moles of CO produced, you need to divide the given mass of CO by the molar mass of CO.

Q: What is the relationship between the heat required and the number of moles of CO produced?

A: The heat required is directly proportional to the number of moles of CO produced. This means that as the number of moles of CO produced increases, the heat required also increases.

Q: How do I calculate the heat required to produce a given quantity of CO?

Q: What is the significance of the heat of reaction in this problem?

Q: How do I determine the number of moles of CO produced per unit of heat?

A: To determine the number of moles of CO produced per unit of heat, you need to divide the number of moles of CO produced by the total heat released.

Q: What is the relationship between the number of moles of CO produced and the heat required?

A: The number of moles of CO produced is directly proportional to the heat required. This means that as the number of moles of CO produced increases, the heat required also increases.

Q: How do I calculate the heat required to produce a given quantity of CO?

Q: What is the significance of the molar mass of CO in this problem?

A: The molar mass of CO is used to calculate the number of moles of CO produced. This value is also used to determine the heat required to produce a given quantity of CO.

Q: How do I determine the number of moles of CO produced?

A: To determine the number of moles of CO produced, you need to divide the given mass of CO by the molar mass of CO.

Q: What is the relationship between the heat required and the number of moles of CO produced?

A: The heat required is directly proportional to the number of moles of CO produced. This means that as the number of moles of CO produced increases, the heat required also increases.

Q: How do I calculate the heat required to produce a given quantity of CO?

Q: What is the significance of the heat of reaction in this problem?

Q: How do I determine the number of moles of CO produced per unit of heat?

A: To determine the number of moles of CO produced per unit of heat, you need to divide the number of moles of CO produced by the total heat released.

Q: What is the relationship between the number of moles of CO produced and the heat required?

A: The number of moles of CO produced is directly proportional to the heat required. This means that as the number of moles of CO produced increases, the heat required also increases.

Q: How do I calculate the heat required to produce a given quantity of CO?

Q: What is the significance of the molar mass of CO in this problem?

A: The molar mass of CO is used to calculate the number of moles of CO produced. This value is also used to determine the heat required to produce a given quantity of CO.

Q: How do I determine the number of moles of CO produced?

A: To determine the number of moles of CO produced, you need to divide the given mass of CO by the molar mass of CO.

Q: What is the relationship between the heat required and the number of moles of CO produced?

A: The heat required is directly proportional to the number of moles of CO produced. This means that as the number of moles of CO produced increases, the heat required also increases.