Using The Thermodynamic Quantities Table Reference Document, Determine Δ G Rxn \Delta G_{\text{rxn}} Δ G Rxn ​ For The Following Reaction At 298 K. (Given: Δ G F 0 \Delta G^0_f Δ G F 0 ​ For H C N ( G ) = 120.0 KJ/mol HCN(g) = 120.0 \, \text{kJ/mol} H CN ( G ) = 120.0 KJ/mol ). Answer To 1 Decimal Place

Introduction

In chemistry, the free energy change of a reaction is a crucial parameter that determines the spontaneity of the reaction. The free energy change, denoted by $\Delta G_{\text{rxn}}$, is a measure of the energy change that occurs during a reaction. In this article, we will use the thermodynamic quantities table to calculate the reaction free energy for a given reaction at 298 K.

Understanding the Thermodynamic Quantities Table

The thermodynamic quantities table is a reference document that provides the standard Gibbs free energy of formation, $\Delta G^0_f$, for various substances. The standard Gibbs free energy of formation is the change in Gibbs free energy that occurs when one mole of a substance is formed from its constituent elements in their standard states.

Calculating Reaction Free Energy

To calculate the reaction free energy, we need to know the standard Gibbs free energy of formation for the reactants and products. Let's consider the following reaction:

$$\text{H}_2(\text{g}) + \text{N}_2(\text{g}) \rightleftharpoons 2\text{HCN}(\text{g})$$

We are given that the standard Gibbs free energy of formation for HCN(g) is 120.0 kJ/mol. We need to find the standard Gibbs free energy of formation for H2(g) and N2(g).

Standard Gibbs Free Energy of Formation for H2(g) and N2(g)

The standard Gibbs free energy of formation for H2(g) and N2(g) can be found in the thermodynamic quantities table. The values are:

• $\Delta G^0_f$ for H2(g) = 0 kJ/mol
• $\Delta G^0_f$ for N2(g) = 0 kJ/mol

Calculating Reaction Free Energy

Now that we have the standard Gibbs free energy of formation for all the substances involved in the reaction, we can calculate the reaction free energy using the following equation:

\Delta G_{\text{rxn}} = \sum \nu_i \Delta G^0_f_i

where $\nu_i$ is the stoichiometric coefficient of the $i$th substance, and \Delta G^0_f_i is the standard Gibbs free energy of formation of the $i$th substance.

For the given reaction, the stoichiometric coefficients are:

• $\nu_{\text{H}_2} = 1$
• $\nu_{\text{N}_2} = 1$
• $\nu_{\text{HCN}} = 2$

The standard Gibbs free energy of formation for the reactants and products are:

• \Delta G^0_f_{\text{H}_2} = 0 kJ/mol
• \Delta G^0_f_{\text{N}_2} = 0 kJ/mol
• \Delta G^0_f_{\text{HCN}} = 120.0 kJ/mol

Substituting these values into the equation, we get:

$$\Delta G_{\text{rxn}} = (1 \times 0) + (1 \times 0) + (2 \times 120.0)$$

$$\Delta G_{\text{rxn}} = 240.0 \, \text{kJ/mol}$$

Conclusion

In this article, we used the thermodynamic quantities table to calculate the reaction free energy for a given reaction at 298 K. We found that the reaction free energy is 240.0 kJ/mol. This value indicates that the reaction is non-spontaneous at 298 K.

References

• Thermodynamic Quantities Table
• Chemistry Textbook

Note

Introduction

In our previous article, we discussed how to calculate the reaction free energy using the thermodynamic quantities table. In this article, we will answer some frequently asked questions related to calculating reaction free energy.

Q: What is the standard Gibbs free energy of formation?

A: The standard Gibbs free energy of formation, denoted by $\Delta G^0_f$, is the change in Gibbs free energy that occurs when one mole of a substance is formed from its constituent elements in their standard states.

Q: How do I find the standard Gibbs free energy of formation for a substance?

A: The standard Gibbs free energy of formation can be found in the thermodynamic quantities table. You can also calculate it using the following equation:

$$\Delta G^0_f = \Delta H^0_f - T \Delta S^0_f$$

where $\Delta H^0_f$ is the standard enthalpy of formation, $T$ is the temperature in Kelvin, and $\Delta S^0_f$ is the standard entropy of formation.

Q: What is the difference between $\Delta G^0_f$ and $\Delta G_{\text{rxn}}$?

A: $\Delta G^0_f$ is the standard Gibbs free energy of formation, which is the change in Gibbs free energy that occurs when one mole of a substance is formed from its constituent elements in their standard states. $\Delta G_{\text{rxn}}$ is the reaction free energy, which is the change in Gibbs free energy that occurs during a reaction.

Q: How do I calculate the reaction free energy using the thermodynamic quantities table?

A: To calculate the reaction free energy using the thermodynamic quantities table, you need to know the standard Gibbs free energy of formation for the reactants and products. You can then use the following equation:

\Delta G_{\text{rxn}} = \sum \nu_i \Delta G^0_f_i

where $\nu_i$ is the stoichiometric coefficient of the $i$th substance, and \Delta G^0_f_i is the standard Gibbs free energy of formation of the $i$th substance.

Q: What is the significance of the reaction free energy?

A: The reaction free energy is a measure of the energy change that occurs during a reaction. It is a crucial parameter that determines the spontaneity of the reaction. A negative reaction free energy indicates that the reaction is spontaneous, while a positive reaction free energy indicates that the reaction is non-spontaneous.

Q: Can I calculate the reaction free energy at a temperature other than 298 K?

A: Yes, you can calculate the reaction free energy at a temperature other than 298 K. You will need to know the standard enthalpy of formation and standard entropy of formation for the reactants and products at the desired temperature.

Q: What are some common mistakes to avoid when calculating reaction free energy?

A: Some common mistakes to avoid when calculating reaction free energy include:

• Not using the correct values for the standard Gibbs free energy of formation
• Not using the correct stoichiometric coefficients
• Not considering the temperature dependence of the reaction free energy

Conclusion

In this article, we answered some frequently asked questions related to calculating reaction free energy. We hope that this article has been helpful in clarifying any doubts you may have had about calculating reaction free energy. If you have any further questions, please don't hesitate to ask.

References

• Thermodynamic Quantities Table
• Chemistry Textbook

Note

Calculating reaction free energy is an important concept in chemistry that can help you understand the spontaneity of a reaction. By following the steps outlined in this article, you can calculate the reaction free energy for a given reaction at a desired temperature.