Hydrogen Reacts With Chlorine To Form Hydrogen Chloride H C L ( G HCl(g H Cl ( G ], With Δ H F = − 92.3 KJ \Delta H_{f} = -92.3 \text{ KJ} Δ H F ​ = − 92.3 KJ .${ H_2(g) + Cl_2(g) \rightarrow 2 HCl(g) }$Which Statement Is Correct?Use $\Delta H_{\text{rxn}} =

Introduction

Hydrogen and chlorine are two highly reactive elements that can form a compound known as hydrogen chloride (HCl). This compound is a colorless, corrosive gas with a strong, irritating odor. In this article, we will explore the reaction between hydrogen and chlorine to form hydrogen chloride, and examine the thermodynamic properties of this reaction.

The Reaction Between Hydrogen and Chlorine

The reaction between hydrogen and chlorine is a highly exothermic process, releasing a significant amount of energy in the form of heat. The balanced chemical equation for this reaction is:

${ H_2(g) + Cl_2(g) \rightarrow 2 HCl(g) }$

In this equation, hydrogen gas (H2) reacts with chlorine gas (Cl2) to form two molecules of hydrogen chloride gas (HCl). This reaction is highly favorable, with a negative enthalpy change (${\Delta H_{\text{rxn}}}$) indicating that energy is released during the reaction.

Thermodynamic Properties of the Reaction

The thermodynamic properties of a reaction, such as the enthalpy change (${\Delta H_{\text{rxn}}}$), are critical in understanding the energy changes that occur during the reaction. In this case, the enthalpy change for the formation of hydrogen chloride is given as ${\Delta H_{f} = -92.3 \text{ kJ}}$. This value indicates that the formation of hydrogen chloride is an exothermic process, releasing 92.3 kilojoules of energy per mole of hydrogen chloride formed.

Which Statement is Correct?

Given the information provided, we can now examine the possible statements that could be made about the reaction between hydrogen and chlorine.

• Statement 1: The reaction between hydrogen and chlorine is an endothermic process, releasing energy.
• Statement 2: The reaction between hydrogen and chlorine is an exothermic process, absorbing energy.
• Statement 3: The reaction between hydrogen and chlorine is a neutral process, neither releasing nor absorbing energy.

Based on the information provided, we can conclude that:

• Statement 1 is incorrect, as the reaction is exothermic, not endothermic.
• Statement 2 is correct, as the reaction is exothermic, releasing energy.
• Statement 3 is incorrect, as the reaction is exothermic, releasing energy.

Conclusion

In conclusion, the reaction between hydrogen and chlorine is a highly exothermic process, releasing a significant amount of energy in the form of heat. The thermodynamic properties of this reaction, such as the enthalpy change (${\Delta H_{\text{rxn}}}$), are critical in understanding the energy changes that occur during the reaction. By examining the possible statements that could be made about the reaction, we can conclude that the correct statement is that the reaction between hydrogen and chlorine is an exothermic process, releasing energy.

References

• National Institute of Standards and Technology (NIST). (2022). Standard Reference Data Program. Retrieved from https://www.nist.gov/pml/chemical-data
• CRC Handbook of Chemistry and Physics. (2022). CRC Press.
  Hydrogen Reacts with Chlorine: Understanding the Formation of Hydrogen Chloride ====================================================================================

Q&A: Hydrogen Reacts with Chlorine

Q: What is the balanced chemical equation for the reaction between hydrogen and chlorine?

A: The balanced chemical equation for the reaction between hydrogen and chlorine is:

${ H_2(g) + Cl_2(g) \rightarrow 2 HCl(g) }$

Q: What is the thermodynamic property of the reaction between hydrogen and chlorine?

A: The thermodynamic property of the reaction between hydrogen and chlorine is the enthalpy change (${\Delta H_{\text{rxn}}}$), which is given as ${\Delta H_{f} = -92.3 \text{ kJ}}$. This value indicates that the formation of hydrogen chloride is an exothermic process, releasing 92.3 kilojoules of energy per mole of hydrogen chloride formed.

Q: Is the reaction between hydrogen and chlorine an endothermic or exothermic process?

A: The reaction between hydrogen and chlorine is an exothermic process, releasing energy.

Q: What is the significance of the enthalpy change (${\Delta H_{\text{rxn}}}$) in the reaction between hydrogen and chlorine?

A: The enthalpy change (${\Delta H_{\text{rxn}}}$) is a critical thermodynamic property that indicates the energy changes that occur during the reaction. In this case, the negative enthalpy change (${\Delta H_{f} = -92.3 \text{ kJ}}$) indicates that the formation of hydrogen chloride is an exothermic process, releasing energy.

Q: What is the product of the reaction between hydrogen and chlorine?

A: The product of the reaction between hydrogen and chlorine is hydrogen chloride (HCl).

Q: What is the reactant of the reaction between hydrogen and chlorine?

A: The reactants of the reaction between hydrogen and chlorine are hydrogen gas (H2) and chlorine gas (Cl2).

Q: Is the reaction between hydrogen and chlorine a neutral process?

A: No, the reaction between hydrogen and chlorine is not a neutral process. It is an exothermic process, releasing energy.

Q: What is the energy released during the reaction between hydrogen and chlorine?

A: The energy released during the reaction between hydrogen and chlorine is 92.3 kilojoules per mole of hydrogen chloride formed.

Q: What is the significance of the reaction between hydrogen and chlorine in everyday life?

A: The reaction between hydrogen and chlorine is significant in everyday life, as it is used in the production of hydrogen chloride, which is a common industrial chemical.

Conclusion

In conclusion, the reaction between hydrogen and chlorine is a highly exothermic process, releasing a significant amount of energy in the form of heat. The thermodynamic properties of this reaction, such as the enthalpy change (${\Delta H_{\text{rxn}}}$), are critical in understanding the energy changes that occur during the reaction. By examining the possible statements that could be made about the reaction, we can conclude that the correct statement is that the reaction between hydrogen and chlorine is an exothermic process, releasing energy.

References

• National Institute of Standards and Technology (NIST). (2022). Standard Reference Data Program. Retrieved from https://www.nist.gov/pml/chemical-data
• CRC Handbook of Chemistry and Physics. (2022). CRC Press.