Reversing the First Equation

Oct 13, 2025 by magicalceylontours.com 104 views

Understanding the Reaction

The given reaction is: $C(s) + H_2O(g) \rightarrow CO(g) + H_2(g)$

This reaction involves the combustion of carbon in the presence of water vapor, resulting in the formation of carbon monoxide and hydrogen gas. To calculate the final equation for this reaction, we need to consider the thermodynamic properties of the reactants and products.

Thermodynamic Properties

The thermodynamic properties of a reaction, such as enthalpy (ΔH), entropy (ΔS), and Gibbs free energy (ΔG), play a crucial role in determining the spontaneity and feasibility of the reaction. In this case, we are interested in the enthalpy change (ΔH) of the reaction.

Enthalpy Change

The enthalpy change (ΔH) of a reaction is a measure of the energy change that occurs during the reaction. A negative ΔH value indicates an exothermic reaction, where energy is released, while a positive ΔH value indicates an endothermic reaction, where energy is absorbed.

Reversing the First Equation

To calculate the final equation for the reaction, we need to reverse the first equation and change the sign of the enthalpy. This is because the reverse reaction has the opposite sign of the enthalpy change.

Reversing the Second Equation

We also need to reverse the second equation and change the sign of the enthalpy. This is because the reverse reaction has the opposite sign of the enthalpy change.

Adding the Two Reversed Equations

Once we have reversed both equations and changed the sign of the enthalpy, we can add the two equations together to get the final equation for the reaction.

Step-by-Step Procedure

Here is the step-by-step procedure to calculate the final equation for the reaction:

Reverse the first equation: $C(s) + H_2O(g) \rightarrow CO(g) + H_2(g)$ becomes $CO(g) + H_2(g) \rightarrow C(s) + H_2O(g)$
Change the sign of the enthalpy: ΔH becomes -ΔH
Reverse the second equation: $C(s) + H_2O(g) \rightarrow CO(g) + H_2(g)$ becomes $CO(g) + H_2(g) \rightarrow C(s) + H_2O(g)$
Change the sign of the enthalpy: ΔH becomes -ΔH
Add the two reversed equations: $CO(g) + H_2(g) \rightarrow C(s) + H_2O(g)$ + $CO(g) + H_2(g) \rightarrow C(s) + H_2O(g)$

Final Equation

The final equation for the reaction is: $2CO(g) + 2H_2(g) \rightarrow 2C(s) + 2H_2O(g)$

Conclusion

In conclusion, to calculate the final equation for the reaction $C(s) + H_2O(g) \rightarrow CO(g) + H_2(g)$ , we need to reverse the first equation and change the sign of the enthalpy, then reverse the second equation and change the sign of the enthalpy, and finally add the two reversed equations together. The final equation for the reaction is $2CO(g) + 2H_2(g) \rightarrow 2C(s) + 2H_2O(g)$ .

Importance of Thermodynamic Properties

The thermodynamic properties of a reaction, such as enthalpy, entropy, and Gibbs free energy, play a crucial role in determining the spontaneity and feasibility of the reaction. In this case, the enthalpy change (ΔH) of the reaction is a measure of the energy change that occurs during the reaction.

Applications of Thermodynamic Properties

The thermodynamic properties of a reaction have numerous applications in various fields, such as chemistry, physics, and engineering. For example, the enthalpy change (ΔH) of a reaction can be used to determine the energy required to initiate a reaction, which is essential in designing and optimizing chemical processes.

Limitations of Thermodynamic Properties

While the thermodynamic properties of a reaction are essential in determining the spontaneity and feasibility of the reaction, they have some limitations. For example, the thermodynamic properties of a reaction do not take into account the kinetic factors that affect the reaction rate.

Conclusion

In conclusion, the thermodynamic properties of a reaction, such as enthalpy, entropy, and Gibbs free energy, play a crucial role in determining the spontaneity and feasibility of the reaction. The enthalpy change (ΔH) of the reaction is a measure of the energy change that occurs during the reaction, and it has numerous applications in various fields.

References

Atkins, P. W., & De Paula, J. (2010). Physical chemistry (9th ed.). Oxford University Press.
Chang, R. (2010). Chemistry (10th ed.). McGraw-Hill.
Levine, I. N. (2012). Physical chemistry (6th ed.). McGraw-Hill.

Glossary

Enthalpy: A measure of the total energy of a system, including the internal energy and the energy associated with the pressure and volume of a system.
Entropy: A measure of the disorder or randomness of a system.
Gibbs free energy: A measure of the energy available to do work in a system.
Thermodynamic properties: Properties of a system that are related to the energy and entropy of the system.

Online Resources

Khan Academy: Thermodynamics
MIT OpenCourseWare: Thermodynamics
University of California, Berkeley: Thermodynamics

Conclusion

Q: What is the purpose of reversing the first equation and changing the sign of the enthalpy?

A: The purpose of reversing the first equation and changing the sign of the enthalpy is to obtain the correct equation for the reaction. Reversing the equation changes the direction of the reaction, and changing the sign of the enthalpy ensures that the energy change is correctly accounted for.

Q: Why do we need to reverse the second equation and change the sign of the enthalpy?

A: We need to reverse the second equation and change the sign of the enthalpy because the second equation is also part of the overall reaction. Reversing the second equation and changing the sign of the enthalpy ensures that the energy change is correctly accounted for in the overall reaction.

Q: What is the final equation for the reaction?

A: The final equation for the reaction is: $2CO(g) + 2H_2(g) \rightarrow 2C(s) + 2H_2O(g)$

Q: What is the significance of the enthalpy change (ΔH) in the reaction?

A: The enthalpy change (ΔH) is a measure of the energy change that occurs during the reaction. A negative ΔH value indicates an exothermic reaction, where energy is released, while a positive ΔH value indicates an endothermic reaction, where energy is absorbed.

Q: How do we determine the spontaneity and feasibility of a reaction?

A: We determine the spontaneity and feasibility of a reaction by considering the thermodynamic properties of the reaction, such as the enthalpy change (ΔH), entropy change (ΔS), and Gibbs free energy change (ΔG).

Q: What are the applications of thermodynamic properties in chemistry?

A: Thermodynamic properties have numerous applications in chemistry, including the design and optimization of chemical processes, the prediction of reaction rates, and the understanding of reaction mechanisms.

Q: What are the limitations of thermodynamic properties?

A: The limitations of thermodynamic properties include the fact that they do not take into account kinetic factors that affect the reaction rate, and that they are based on equilibrium conditions, which may not be representative of real-world conditions.

Q: How do we calculate the final equation for a reaction?

A: To calculate the final equation for a reaction, we need to reverse the first equation and change the sign of the enthalpy, then reverse the second equation and change the sign of the enthalpy, and finally add the two reversed equations together.

Q: What is the importance of thermodynamic properties in understanding chemical reactions?

A: Thermodynamic properties are essential in understanding chemical reactions because they provide a quantitative measure of the energy and entropy changes that occur during the reaction.

Q: How do we determine the energy required to initiate a reaction?

A: We determine the energy required to initiate a reaction by considering the enthalpy change (ΔH) of the reaction.

Q: What are the implications of thermodynamic properties on the design and optimization of chemical processes?

A: Thermodynamic properties have significant implications on the design and optimization of chemical processes, including the prediction of reaction rates, the understanding of reaction mechanisms, and the optimization of reaction conditions.

Q: How do we predict the spontaneity and feasibility of a reaction?

A: We predict the spontaneity and feasibility of a reaction by considering the thermodynamic properties of the reaction, such as the enthalpy change (ΔH), entropy change (ΔS), and Gibbs free energy change (ΔG).

Q: What are the key factors that affect the reaction rate?

A: The key factors that affect the reaction rate include the concentration of reactants, the temperature, and the presence of catalysts.

Q: How do we understand the reaction mechanism?

A: We understand the reaction mechanism by considering the thermodynamic properties of the reaction, such as the enthalpy change (ΔH), entropy change (ΔS), and Gibbs free energy change (ΔG), and by analyzing the reaction kinetics.

Q: What are the implications of thermodynamic properties on the understanding of chemical reactions?

A: Thermodynamic properties have significant implications on the understanding of chemical reactions, including the prediction of reaction rates, the understanding of reaction mechanisms, and the optimization of reaction conditions.

Q: How do we determine the energy required to initiate a reaction?

A: We determine the energy required to initiate a reaction by considering the enthalpy change (ΔH) of the reaction.

Q: What are the key factors that affect the reaction rate?

A: The key factors that affect the reaction rate include the concentration of reactants, the temperature, and the presence of catalysts.

Q: How do we understand the reaction mechanism?

Q: What are the implications of thermodynamic properties on the understanding of chemical reactions?

Q: How do we determine the energy required to initiate a reaction?

A: We determine the energy required to initiate a reaction by considering the enthalpy change (ΔH) of the reaction.

Q: What are the key factors that affect the reaction rate?

A: The key factors that affect the reaction rate include the concentration of reactants, the temperature, and the presence of catalysts.