How Much Energy Is Released When 89 G Of Aluminum Is Reacted With 75 G Of Chlorine?$\[ \text{Reaction: } 2\text{Al} + 3\text{Cl}_2 \rightarrow 2\text{AlCl}_3 \quad \Delta H = -704 \text{ KJ} \\]

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Introduction

Chemical reactions involve the transformation of one substance into another, often accompanied by the release or absorption of energy. In this article, we will explore the energy released when 89 g of aluminum reacts with 75 g of chlorine. To determine the energy released, we need to calculate the number of moles of aluminum and chlorine present in the given masses and then use the given reaction equation to find the energy released.

Understanding the Reaction Equation

The reaction between aluminum and chlorine is represented by the following equation:

Reaction: 2Al+3Cl2→2AlCl3ΔH=−704 kJ{ \text{Reaction: } 2\text{Al} + 3\text{Cl}_2 \rightarrow 2\text{AlCl}_3 \quad \Delta H = -704 \text{ kJ} }

In this equation, 2 moles of aluminum react with 3 moles of chlorine to produce 2 moles of aluminum chloride. The energy released during this reaction is -704 kJ, indicating that the reaction is exothermic.

Calculating the Number of Moles of Aluminum and Chlorine

To calculate the number of moles of aluminum and chlorine, we need to know their molar masses. The molar mass of aluminum (Al) is 26.98 g/mol, and the molar mass of chlorine (Cl) is 35.45 g/mol.

Aluminum

The number of moles of aluminum can be calculated as follows:

Number of moles of Al=Mass of AlMolar mass of Al{ \text{Number of moles of Al} = \frac{\text{Mass of Al}}{\text{Molar mass of Al}} }

Number of moles of Al=89 g26.98 g/mol{ \text{Number of moles of Al} = \frac{89 \text{ g}}{26.98 \text{ g/mol}} }

Number of moles of Al=3.30 mol{ \text{Number of moles of Al} = 3.30 \text{ mol} }

Chlorine

The number of moles of chlorine can be calculated as follows:

Number of moles of Cl2=Mass of Cl2Molar mass of Cl2{ \text{Number of moles of Cl}_2 = \frac{\text{Mass of Cl}_2}{\text{Molar mass of Cl}_2} }

Number of moles of Cl2=75 g70.90 g/mol{ \text{Number of moles of Cl}_2 = \frac{75 \text{ g}}{70.90 \text{ g/mol}} }

Number of moles of Cl2=1.06 mol{ \text{Number of moles of Cl}_2 = 1.06 \text{ mol} }

Determining the Limiting Reactant

To determine the limiting reactant, we need to compare the mole ratio of aluminum to chlorine with the mole ratio in the balanced equation.

The mole ratio of aluminum to chlorine in the balanced equation is 2:3.

The mole ratio of aluminum to chlorine in the given reaction is:

3.30 mol1.06 mol=3.11{ \frac{3.30 \text{ mol}}{1.06 \text{ mol}} = 3.11 }

Since the mole ratio of aluminum to chlorine in the given reaction is greater than the mole ratio in the balanced equation, chlorine is the limiting reactant.

Calculating the Energy Released

Since chlorine is the limiting reactant, we can use the number of moles of chlorine to calculate the energy released.

The energy released per mole of chlorine is -704 kJ / 3 mol = -234.67 kJ/mol.

The energy released when 1.06 mol of chlorine reacts is:

Energy released=Number of moles of Cl2×Energy released per mole of Cl2{ \text{Energy released} = \text{Number of moles of Cl}_2 \times \text{Energy released per mole of Cl}_2 }

Energy released=1.06 mol×−234.67 kJ/mol{ \text{Energy released} = 1.06 \text{ mol} \times -234.67 \text{ kJ/mol} }

Energy released=−248.51 kJ{ \text{Energy released} = -248.51 \text{ kJ} }

Conclusion

In this article, we calculated the energy released when 89 g of aluminum reacts with 75 g of chlorine. We determined that chlorine is the limiting reactant and used the number of moles of chlorine to calculate the energy released. The energy released is -248.51 kJ.

References

  • [1] Petrucci, R. H., Harwood, W. S., & Herring, F. G. (2002). General chemistry: Principles and modern applications. Prentice Hall.
  • [2] Atkins, P. W., & De Paula, J. (2006). Physical chemistry. Oxford University Press.

Additional Information

  • The reaction between aluminum and chlorine is highly exothermic, releasing a significant amount of energy.
  • The energy released per mole of chlorine is -234.67 kJ/mol.
  • The energy released when 1.06 mol of chlorine reacts is -248.51 kJ.
    Q&A: Energy Released in Aluminum-Chlorine Reaction =====================================================

Introduction

In our previous article, we explored the energy released when 89 g of aluminum reacts with 75 g of chlorine. In this article, we will answer some frequently asked questions related to this topic.

Q: What is the molar mass of aluminum and chlorine?

A: The molar mass of aluminum (Al) is 26.98 g/mol, and the molar mass of chlorine (Cl) is 35.45 g/mol.

Q: How do you calculate the number of moles of aluminum and chlorine?

A: To calculate the number of moles of aluminum and chlorine, you need to divide the mass of each substance by its molar mass.

For aluminum:

Number of moles of Al=Mass of AlMolar mass of Al{ \text{Number of moles of Al} = \frac{\text{Mass of Al}}{\text{Molar mass of Al}} }

Number of moles of Al=89 g26.98 g/mol{ \text{Number of moles of Al} = \frac{89 \text{ g}}{26.98 \text{ g/mol}} }

Number of moles of Al=3.30 mol{ \text{Number of moles of Al} = 3.30 \text{ mol} }

For chlorine:

Number of moles of Cl2=Mass of Cl2Molar mass of Cl2{ \text{Number of moles of Cl}_2 = \frac{\text{Mass of Cl}_2}{\text{Molar mass of Cl}_2} }

Number of moles of Cl2=75 g70.90 g/mol{ \text{Number of moles of Cl}_2 = \frac{75 \text{ g}}{70.90 \text{ g/mol}} }

Number of moles of Cl2=1.06 mol{ \text{Number of moles of Cl}_2 = 1.06 \text{ mol} }

Q: What is the limiting reactant in the aluminum-chlorine reaction?

A: To determine the limiting reactant, you need to compare the mole ratio of aluminum to chlorine with the mole ratio in the balanced equation.

The mole ratio of aluminum to chlorine in the balanced equation is 2:3.

The mole ratio of aluminum to chlorine in the given reaction is:

3.30 mol1.06 mol=3.11{ \frac{3.30 \text{ mol}}{1.06 \text{ mol}} = 3.11 }

Since the mole ratio of aluminum to chlorine in the given reaction is greater than the mole ratio in the balanced equation, chlorine is the limiting reactant.

Q: How do you calculate the energy released in the aluminum-chlorine reaction?

A: To calculate the energy released, you need to multiply the number of moles of the limiting reactant (chlorine) by the energy released per mole of chlorine.

The energy released per mole of chlorine is -234.67 kJ/mol.

The energy released when 1.06 mol of chlorine reacts is:

Energy released=Number of moles of Cl2×Energy released per mole of Cl2{ \text{Energy released} = \text{Number of moles of Cl}_2 \times \text{Energy released per mole of Cl}_2 }

Energy released=1.06 mol×−234.67 kJ/mol{ \text{Energy released} = 1.06 \text{ mol} \times -234.67 \text{ kJ/mol} }

Energy released=−248.51 kJ{ \text{Energy released} = -248.51 \text{ kJ} }

Q: What is the significance of the energy released in the aluminum-chlorine reaction?

A: The energy released in the aluminum-chlorine reaction is significant because it can be used to power various devices, such as electrical generators or heating systems.

Q: Can you provide more information about the reaction between aluminum and chlorine?

A: Yes, the reaction between aluminum and chlorine is a highly exothermic reaction, releasing a significant amount of energy. The reaction is also highly reactive, releasing a large amount of heat and light.

Conclusion

In this article, we answered some frequently asked questions related to the energy released in the aluminum-chlorine reaction. We provided information on the molar mass of aluminum and chlorine, the calculation of the number of moles of each substance, the limiting reactant, and the energy released in the reaction. We also discussed the significance of the energy released and provided more information about the reaction between aluminum and chlorine.