Calculate The Enthalpy In K J / M O L KJ/mol K J / M O L Of The Following Reaction Using The Standard Enthalpies Of Formation Provided:$[ \begin{array}{c} C_2H_4(g) + 3O_2(g) \rightarrow 2CO_2(g) + 2H_2O(g) \ \Delta H_f^{\circ} C_2H_4(g) = 52.4 ,

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Introduction

In chemistry, the enthalpy of a reaction is a measure of the total energy change that occurs during the reaction. It is an important concept in thermodynamics and is used to predict the spontaneity of a reaction. The standard enthalpy of formation ($\Delta H_f^{\circ}$) is a measure of the enthalpy change that occurs when one mole of a substance is formed from its constituent elements in their standard states. In this article, we will calculate the enthalpy in $kJ/mol$ of the following reaction using the standard enthalpies of formation provided:

$$C_2H_4(g) + 3O_2(g) \rightarrow 2CO_2(g) + 2H_2O(g)$$

Standard Enthalpies of Formation

The standard enthalpies of formation of the reactants and products are given as follows:

Substance	$\Delta H_f^{\circ}$ (kJ/mol)
$C_2H_4(g)$	52.4
$O_2(g)$	0
$CO_2(g)$	-393.5
$H_2O(g)$	-241.8

Calculating the Enthalpy of the Reaction

To calculate the enthalpy of the reaction, we need to use the following equation:

$$\Delta H_{rxn}^{\circ} = \sum \Delta H_f^{\circ} (\text{products}) - \sum \Delta H_f^{\circ} (\text{reactants})$$

where $\Delta H_{rxn}^{\circ}$ is the standard enthalpy of the reaction, and $\Delta H_f^{\circ}$ is the standard enthalpy of formation of each substance.

Step 1: Calculate the Enthalpy of the Products

The products of the reaction are $2CO_2(g)$ and $2H_2O(g)$. We need to calculate the enthalpy of each product and then multiply it by 2.

$$\Delta H_f^{\circ} (2CO_2(g)) = 2 \times \Delta H_f^{\circ} (CO_2(g)) = 2 \times (-393.5) = -787.0 \, kJ/mol$$

$$\Delta H_f^{\circ} (2H_2O(g)) = 2 \times \Delta H_f^{\circ} (H_2O(g)) = 2 \times (-241.8) = -483.6 \, kJ/mol$$

Step 2: Calculate the Enthalpy of the Reactants

The reactants of the reaction are $C_2H_4(g)$ and $3O_2(g)$. We need to calculate the enthalpy of each reactant and then multiply it by 1 and 3, respectively.

$$\Delta H_f^{\circ} (C_2H_4(g)) = \Delta H_f^{\circ} (C_2H_4(g)) = 52.4 \, kJ/mol$$

$$\Delta H_f^{\circ} (3O_2(g)) = 3 \times \Delta H_f^{\circ} (O_2(g)) = 3 \times 0 = 0 \, kJ/mol$$

Step 3: Calculate the Enthalpy of the Reaction

Now that we have calculated the enthalpy of the products and reactants, we can calculate the enthalpy of the reaction using the following equation:

$$\Delta H_{rxn}^{\circ} = \sum \Delta H_f^{\circ} (\text{products}) - \sum \Delta H_f^{\circ} (\text{reactants})$$

$$\Delta H_{rxn}^{\circ} = \Delta H_f^{\circ} (2CO_2(g)) + \Delta H_f^{\circ} (2H_2O(g)) - \Delta H_f^{\circ} (C_2H_4(g)) - \Delta H_f^{\circ} (3O_2(g))$$

$$\Delta H_{rxn}^{\circ} = -787.0 \, kJ/mol + (-483.6 \, kJ/mol) - 52.4 \, kJ/mol - 0 \, kJ/mol$$

$$\Delta H_{rxn}^{\circ} = -1323.0 \, kJ/mol$$

Conclusion

In this article, we calculated the enthalpy in $kJ/mol$ of the following reaction using the standard enthalpies of formation provided:

$$C_2H_4(g) + 3O_2(g) \rightarrow 2CO_2(g) + 2H_2O(g)$$

We used the following equation to calculate the enthalpy of the reaction:

$$\Delta H_{rxn}^{\circ} = \sum \Delta H_f^{\circ} (\text{products}) - \sum \Delta H_f^{\circ} (\text{reactants})$$

We calculated the enthalpy of the products and reactants and then used the equation to calculate the enthalpy of the reaction. The result was:

$$\Delta H_{rxn}^{\circ} = -1323.0 \, kJ/mol$$

$$

Introduction

In our previous article, we calculated the enthalpy in $kJ/mol$ of the following reaction using the standard enthalpies of formation provided:

$$C_2H_4(g) + 3O_2(g) \rightarrow 2CO_2(g) + 2H_2O(g)$$

In this article, we will answer some frequently asked questions about calculating enthalpy in $kJ/mol$ of a chemical reaction.

Q: What is enthalpy?

A: Enthalpy is a measure of the total energy change that occurs during a chemical reaction. It is an important concept in thermodynamics and is used to predict the spontaneity of a reaction.

Q: What is the standard enthalpy of formation?

A: The standard enthalpy of formation ($\Delta H_f^{\circ}$) is a measure of the enthalpy change that occurs when one mole of a substance is formed from its constituent elements in their standard states.

Q: How do I calculate the enthalpy of a reaction?

A: To calculate the enthalpy of a reaction, you need to use the following equation:

$$\Delta H_{rxn}^{\circ} = \sum \Delta H_f^{\circ} (\text{products}) - \sum \Delta H_f^{\circ} (\text{reactants})$$

Q: What are the units of enthalpy?

A: The units of enthalpy are typically measured in $kJ/mol$.

Q: Can I use this method to calculate the enthalpy of any reaction?

A: Yes, you can use this method to calculate the enthalpy of any reaction, as long as you have the standard enthalpies of formation of the reactants and products.

Q: What if I don't have the standard enthalpies of formation of the reactants and products?

A: If you don't have the standard enthalpies of formation of the reactants and products, you can use other methods to estimate the enthalpy of the reaction, such as using the bond energies of the reactants and products.

Q: Can I use this method to calculate the enthalpy of a reaction that involves gases?

A: Yes, you can use this method to calculate the enthalpy of a reaction that involves gases, as long as you have the standard enthalpies of formation of the reactants and products.

Q: Can I use this method to calculate the enthalpy of a reaction that involves solids or liquids?

A: Yes, you can use this method to calculate the enthalpy of a reaction that involves solids or liquids, as long as you have the standard enthalpies of formation of the reactants and products.

Q: What are some common mistakes to avoid when calculating the enthalpy of a reaction?

A: Some common mistakes to avoid when calculating the enthalpy of a reaction include:

• Not using the correct units for enthalpy
• Not using the correct equation for calculating the enthalpy of a reaction
• Not accounting for the enthalpy of formation of the reactants and products
• Not considering the enthalpy of reaction of the reactants and products

Conclusion

In this article, we answered some frequently asked questions about calculating enthalpy in $kJ/mol$ of a chemical reaction. We hope that this article has been helpful in clarifying any confusion you may have had about this topic. If you have any further questions, please don't hesitate to ask.

Additional Resources

If you want to learn more about calculating enthalpy in $kJ/mol$ of a chemical reaction, we recommend checking out the following resources:

• "Thermodynamics: An Introduction to the Physical Chemistry of Chemical Processes" by Donald A. McQuarrie and John D. Simon
• "Chemical Thermodynamics: Principles and Applications" by Richard J. Silbey and Robert A. Alberty
• "Physical Chemistry: A Molecular Approach" by Peter Atkins and Julio de Paula

We hope that this article has been helpful in your studies of thermodynamics and chemical reactions. Good luck with your studies!