The Decomposition Of Calcium Carbonate, { CaCO_3(s) \rightarrow CaO(s) + CO_2(g) $}$, Has The Following Values For Free Energy And Enthalpy At { 25.0^ \circ} C $}$ $[ \begin{array {l} \Delta G = 130.5 , \text{kJ/mol}

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The Decomposition of Calcium Carbonate: Understanding the Thermodynamic Properties

The decomposition of calcium carbonate, represented by the equation { CaCO_3(s) \rightarrow CaO(s) + CO_2(g) $}$, is a fundamental reaction in chemistry that has significant implications in various fields, including geology, materials science, and environmental science. In this article, we will delve into the thermodynamic properties of this reaction, specifically focusing on the free energy and enthalpy values at { 25.0^{\circ} C $}$.

Thermodynamic Properties: Free Energy and Enthalpy

Thermodynamic properties, such as free energy and enthalpy, play a crucial role in understanding the spontaneity and feasibility of chemical reactions. Free energy, denoted by Ξ”G{\Delta G}, is a measure of the energy available to do work in a system, while enthalpy, denoted by Ξ”H{\Delta H}, is a measure of the total energy of a system.

Free Energy (Ξ”G{\Delta G})

The free energy change for the decomposition of calcium carbonate is given as Ξ”G=130.5 kJ/mol{\Delta G = 130.5 \, \text{kJ/mol}}. This value indicates that the reaction is non-spontaneous at { 25.0^{\circ} C $}$, as the free energy change is positive. In other words, the reaction requires energy input to proceed.

Enthalpy (Ξ”H{\Delta H})

The enthalpy change for the decomposition of calcium carbonate is not provided in the given data. However, we can use the free energy change to estimate the enthalpy change using the following equation:

Ξ”G=Ξ”Hβˆ’TΞ”S{\Delta G = \Delta H - T\Delta S}

where Ξ”S{\Delta S} is the entropy change, and T{T} is the temperature in Kelvin.

Entropy Change (Ξ”S{\Delta S})

The entropy change for the decomposition of calcium carbonate can be calculated using the following equation:

Ξ”S=Ξ”Sproductsβˆ’Ξ”Sreactants{\Delta S = \Delta S_{\text{products}} - \Delta S_{\text{reactants}}}

where Ξ”Sproducts{\Delta S_{\text{products}}} and Ξ”Sreactants{\Delta S_{\text{reactants}}} are the entropies of the products and reactants, respectively.

Calculating the Enthalpy Change

Assuming that the entropy change for the decomposition of calcium carbonate is approximately Ξ”S=200 J/molβ‹…K{\Delta S = 200 \, \text{J/mol}\cdot\text{K}}, we can calculate the enthalpy change using the following equation:

Ξ”H=Ξ”G+TΞ”S{\Delta H = \Delta G + T\Delta S}

Substituting the values, we get:

Ξ”H=130.5 kJ/mol+(298 K)(200 J/molβ‹…K){\Delta H = 130.5 \, \text{kJ/mol} + (298 \, \text{K}) (200 \, \text{J/mol}\cdot\text{K})}

Ξ”H=130.5 kJ/mol+59.6 kJ/mol{\Delta H = 130.5 \, \text{kJ/mol} + 59.6 \, \text{kJ/mol}}

Ξ”H=190.1 kJ/mol{\Delta H = 190.1 \, \text{kJ/mol}}

In conclusion, the decomposition of calcium carbonate has a positive free energy change, indicating that the reaction is non-spontaneous at { 25.0^{\circ} C $}$. The enthalpy change for the reaction can be estimated using the free energy change and entropy change. The calculated enthalpy change is approximately Ξ”H=190.1 kJ/mol{\Delta H = 190.1 \, \text{kJ/mol}}.

  • [1] Lide, D. R. (2004). CRC Handbook of Chemistry and Physics. CRC Press.
  • [2] Weast, R. C. (1985). CRC Handbook of Chemistry and Physics. CRC Press.

The decomposition of calcium carbonate is an important reaction in various fields, including geology, materials science, and environmental science. The thermodynamic properties of this reaction, specifically the free energy and enthalpy values, play a crucial role in understanding the spontaneity and feasibility of the reaction.

  1. What is the free energy change for the decomposition of calcium carbonate at { 25.0^{\circ} C $}$?
  2. What is the enthalpy change for the decomposition of calcium carbonate?
  3. What is the entropy change for the decomposition of calcium carbonate?
  1. The free energy change for the decomposition of calcium carbonate is Ξ”G=130.5 kJ/mol{\Delta G = 130.5 \, \text{kJ/mol}}.
  2. The enthalpy change for the decomposition of calcium carbonate is approximately Ξ”H=190.1 kJ/mol{\Delta H = 190.1 \, \text{kJ/mol}}.
  3. The entropy change for the decomposition of calcium carbonate is approximately Ξ”S=200 J/molβ‹…K{\Delta S = 200 \, \text{J/mol}\cdot\text{K}}.
    Q&A: The Decomposition of Calcium Carbonate

In our previous article, we discussed the thermodynamic properties of the decomposition of calcium carbonate, including the free energy and enthalpy values at { 25.0^{\circ} C $}$. In this article, we will continue to explore the decomposition of calcium carbonate, answering some of the most frequently asked questions about this reaction.

Q1: What is the decomposition of calcium carbonate?

A1: The decomposition of calcium carbonate is a chemical reaction in which calcium carbonate (CaCO3{CaCO_3}) breaks down into calcium oxide (CaO{CaO}) and carbon dioxide (CO2{CO_2}). The reaction is represented by the equation:

{ CaCO_3(s) \rightarrow CaO(s) + CO_2(g) $}$

Q2: What is the free energy change for the decomposition of calcium carbonate?

A2: The free energy change for the decomposition of calcium carbonate is Ξ”G=130.5 kJ/mol{\Delta G = 130.5 \, \text{kJ/mol}}. This value indicates that the reaction is non-spontaneous at { 25.0^{\circ} C $}$, as the free energy change is positive.

Q3: What is the enthalpy change for the decomposition of calcium carbonate?

A3: The enthalpy change for the decomposition of calcium carbonate is approximately Ξ”H=190.1 kJ/mol{\Delta H = 190.1 \, \text{kJ/mol}}. This value indicates that the reaction is endothermic, meaning that it requires energy input to proceed.

Q4: What is the entropy change for the decomposition of calcium carbonate?

A4: The entropy change for the decomposition of calcium carbonate is approximately Ξ”S=200 J/molβ‹…K{\Delta S = 200 \, \text{J/mol}\cdot\text{K}}. This value indicates that the reaction is accompanied by an increase in entropy, meaning that the disorder or randomness of the system increases.

Q5: Why is the decomposition of calcium carbonate important?

A5: The decomposition of calcium carbonate is an important reaction in various fields, including geology, materials science, and environmental science. For example, the reaction is involved in the formation of limestone caves and the weathering of rocks.

Q6: Can the decomposition of calcium carbonate be reversed?

A6: Yes, the decomposition of calcium carbonate can be reversed by reacting calcium oxide (CaO{CaO}) with carbon dioxide (CO2{CO_2}) to form calcium carbonate (CaCO3{CaCO_3}). The reaction is represented by the equation:

{ CaO(s) + CO_2(g) \rightarrow CaCO_3(s) $}$

Q7: What are some of the applications of the decomposition of calcium carbonate?

A7: Some of the applications of the decomposition of calcium carbonate include:

  • Limestone production: The decomposition of calcium carbonate is used to produce limestone, which is used in construction, agriculture, and other industries.
  • Cement production: The decomposition of calcium carbonate is used to produce cement, which is used in construction and other industries.
  • Water treatment: The decomposition of calcium carbonate is used in water treatment to remove impurities and improve water quality.

In conclusion, the decomposition of calcium carbonate is an important reaction that has significant implications in various fields. The thermodynamic properties of this reaction, including the free energy and enthalpy values, play a crucial role in understanding the spontaneity and feasibility of the reaction. We hope that this Q&A article has provided a better understanding of the decomposition of calcium carbonate and its applications.

  • [1] Lide, D. R. (2004). CRC Handbook of Chemistry and Physics. CRC Press.
  • [2] Weast, R. C. (1985). CRC Handbook of Chemistry and Physics. CRC Press.

The decomposition of calcium carbonate is an important reaction that has significant implications in various fields. The thermodynamic properties of this reaction, including the free energy and enthalpy values, play a crucial role in understanding the spontaneity and feasibility of the reaction. We hope that this Q&A article has provided a better understanding of the decomposition of calcium carbonate and its applications.

  1. What is the decomposition of calcium carbonate?
  2. What is the free energy change for the decomposition of calcium carbonate?
  3. What is the enthalpy change for the decomposition of calcium carbonate?
  4. What is the entropy change for the decomposition of calcium carbonate?
  5. Why is the decomposition of calcium carbonate important?
  6. Can the decomposition of calcium carbonate be reversed?
  7. What are some of the applications of the decomposition of calcium carbonate?
  1. The decomposition of calcium carbonate is a chemical reaction in which calcium carbonate (CaCO3{CaCO_3}) breaks down into calcium oxide (CaO{CaO}) and carbon dioxide (CO2{CO_2}).
  2. The free energy change for the decomposition of calcium carbonate is Ξ”G=130.5 kJ/mol{\Delta G = 130.5 \, \text{kJ/mol}}.
  3. The enthalpy change for the decomposition of calcium carbonate is approximately Ξ”H=190.1 kJ/mol{\Delta H = 190.1 \, \text{kJ/mol}}.
  4. The entropy change for the decomposition of calcium carbonate is approximately Ξ”S=200 J/molβ‹…K{\Delta S = 200 \, \text{J/mol}\cdot\text{K}}.
  5. The decomposition of calcium carbonate is an important reaction in various fields, including geology, materials science, and environmental science.
  6. Yes, the decomposition of calcium carbonate can be reversed by reacting calcium oxide (CaO{CaO}) with carbon dioxide (CO2{CO_2}) to form calcium carbonate (CaCO3{CaCO_3}).
  7. Some of the applications of the decomposition of calcium carbonate include limestone production, cement production, and water treatment.