Sulfur Reacts With Oxygen To Form Sulfur Dioxide { \left( SO_2(g), \Delta H_f = -296.8 , \text{kJ/mol} \right)$} . . . { S(s) + O_2(g) \rightarrow SO_2(g) \} What Is The Enthalpy Change For The Reaction?Use [$\Delta H_{\text{rxn}}

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Introduction

In the world of chemistry, understanding the enthalpy change of a reaction is crucial in determining the energy changes that occur during a chemical process. The enthalpy change, denoted by ΔH, is a measure of the energy change that occurs when a chemical reaction takes place. In this article, we will explore the enthalpy change of the reaction between sulfur (S) and oxygen (O2) to form sulfur dioxide (SO2).

The Reaction

The reaction between sulfur and oxygen to form sulfur dioxide is represented by the following equation:

S(s)+O2(g)→SO2(g){ S(s) + O_2(g) \rightarrow SO_2(g) }

This reaction is an example of a combustion reaction, where sulfur reacts with oxygen to form a new compound. The enthalpy change of this reaction is denoted by ΔHrxn.

Enthalpy Change

The enthalpy change of a reaction is calculated using the following formula:

ΔHrxn=∑ΔHf(products)−∑ΔHf(reactants){ \Delta H_{\text{rxn}} = \sum \Delta H_f(\text{products}) - \sum \Delta H_f(\text{reactants}) }

In this case, the enthalpy change of the reaction is calculated as follows:

ΔHrxn=ΔHf(SO2(g))−ΔHf(S(s))−ΔHf(O2(g)){ \Delta H_{\text{rxn}} = \Delta H_f(SO_2(g)) - \Delta H_f(S(s)) - \Delta H_f(O_2(g)) }

The enthalpy of formation of SO2(g) is given as -296.8 kJ/mol. The enthalpy of formation of S(s) is zero, since it is an element in its standard state. The enthalpy of formation of O2(g) is also zero, since it is an element in its standard state.

Calculating the Enthalpy Change

Substituting the values into the formula, we get:

ΔHrxn=−296.8 kJ/mol−0−0{ \Delta H_{\text{rxn}} = -296.8 \, \text{kJ/mol} - 0 - 0 }

ΔHrxn=−296.8 kJ/mol{ \Delta H_{\text{rxn}} = -296.8 \, \text{kJ/mol} }

Therefore, the enthalpy change of the reaction between sulfur and oxygen to form sulfur dioxide is -296.8 kJ/mol.

Interpretation of the Enthalpy Change

The negative value of the enthalpy change indicates that the reaction is exothermic, meaning that it releases energy. This is consistent with the fact that sulfur reacts with oxygen to form a new compound, releasing energy in the process.

Conclusion

In conclusion, the enthalpy change of the reaction between sulfur and oxygen to form sulfur dioxide is -296.8 kJ/mol. This value indicates that the reaction is exothermic, releasing energy in the process. Understanding the enthalpy change of a reaction is crucial in determining the energy changes that occur during a chemical process.

References

  • Petrucci, R. H., Harwood, W. S., & Herring, F. G. (2006). General Chemistry: Principles and Modern Applications. Upper Saddle River, NJ: Pearson Prentice Hall.
  • Atkins, P. W., & De Paula, J. (2006). Physical Chemistry. Oxford University Press.

Further Reading

  • Enthalpy change: A measure of the energy change that occurs during a chemical reaction.
  • Combustion reaction: A type of chemical reaction where a substance reacts with oxygen to form a new compound.
  • Standard enthalpy of formation: The enthalpy change that occurs when one mole of a substance is formed from its elements in their standard states.
    Sulfur Reacts with Oxygen to Form Sulfur Dioxide: Q&A =====================================================

Introduction

In our previous article, we explored the enthalpy change of the reaction between sulfur (S) and oxygen (O2) to form sulfur dioxide (SO2). In this article, we will answer some frequently asked questions related to this reaction.

Q: What is the enthalpy change of the reaction between sulfur and oxygen to form sulfur dioxide?

A: The enthalpy change of the reaction between sulfur and oxygen to form sulfur dioxide is -296.8 kJ/mol.

Q: Is the reaction between sulfur and oxygen to form sulfur dioxide exothermic or endothermic?

A: The reaction between sulfur and oxygen to form sulfur dioxide is exothermic, meaning that it releases energy.

Q: What is the standard enthalpy of formation of sulfur dioxide?

A: The standard enthalpy of formation of sulfur dioxide is -296.8 kJ/mol.

Q: What is the standard enthalpy of formation of sulfur?

A: The standard enthalpy of formation of sulfur is zero, since it is an element in its standard state.

Q: What is the standard enthalpy of formation of oxygen?

A: The standard enthalpy of formation of oxygen is zero, since it is an element in its standard state.

Q: How is the enthalpy change of a reaction calculated?

A: The enthalpy change of a reaction is calculated using the following formula:

ΔHrxn=∑ΔHf(products)−∑ΔHf(reactants){ \Delta H_{\text{rxn}} = \sum \Delta H_f(\text{products}) - \sum \Delta H_f(\text{reactants}) }

Q: What is the difference between the enthalpy change of a reaction and the standard enthalpy of formation of a substance?

A: The enthalpy change of a reaction is the energy change that occurs during a chemical reaction, while the standard enthalpy of formation of a substance is the energy change that occurs when one mole of a substance is formed from its elements in their standard states.

Q: Why is it important to understand the enthalpy change of a reaction?

A: Understanding the enthalpy change of a reaction is crucial in determining the energy changes that occur during a chemical process. This information can be used to predict the feasibility of a reaction and to design more efficient chemical processes.

Q: Can you provide some examples of reactions that have a negative enthalpy change?

A: Yes, some examples of reactions that have a negative enthalpy change include:

  • Combustion reactions, such as the reaction between methane and oxygen to form carbon dioxide and water.
  • Neutralization reactions, such as the reaction between hydrochloric acid and sodium hydroxide to form water and sodium chloride.
  • Precipitation reactions, such as the reaction between silver nitrate and sodium chloride to form silver chloride and sodium nitrate.

Conclusion

In conclusion, the reaction between sulfur and oxygen to form sulfur dioxide is an exothermic reaction that releases energy. Understanding the enthalpy change of a reaction is crucial in determining the energy changes that occur during a chemical process. We hope that this Q&A article has provided you with a better understanding of this reaction and its importance in chemistry.

References

  • Petrucci, R. H., Harwood, W. S., & Herring, F. G. (2006). General Chemistry: Principles and Modern Applications. Upper Saddle River, NJ: Pearson Prentice Hall.
  • Atkins, P. W., & De Paula, J. (2006). Physical Chemistry. Oxford University Press.

Further Reading

  • Enthalpy change: A measure of the energy change that occurs during a chemical reaction.
  • Combustion reaction: A type of chemical reaction where a substance reacts with oxygen to form a new compound.
  • Standard enthalpy of formation: The enthalpy change that occurs when one mole of a substance is formed from its elements in their standard states.