**Exercise 18.66**Consider the following reaction:\[ \text{CaCO}_3(s) \rightarrow \text{CaO}(s) + \text{CO}_2(g) \]Estimate \(\Delta G^\circ\) for this reaction at each of the following temperatures. (Assume that \(\Delta H^\circ\) and \(\Delta S^\circ\) do not change too much within the given temperature range.)**Part C**- Temperature: 1400 K- \(\Delta G^\circ\) = _____ kJ**Part D**Predict whether or not the reaction in part A will be spontaneous at 305 K.- Options: - Spontaneous - Nonspontaneous**Part E**Predict whether or not the reaction in part B will be spontaneous at 1040 K.- Options: - Spontaneous - Nonspontaneous**Instructions:**Use the information given to calculate or predict the spontaneity of the reaction at the specified temperatures. Use the provided tools to submit your answers or request guidance if necessary. **Exercise 18.66**Consider the following reaction:\[ \text{CaCO}_3 (s) \rightarrow \text{CaO} (s) + \text{CO}_2 (g) \]Estimate \( \Delta G^\circ \) for this reaction at each of the following temperatures. (Assume that \( \Delta H^\circ \) and \( \Delta S^\circ \) do not change too much within the given temperature range.)**Part A**Temperature: 305 KInput box for \( \Delta G^\circ = \) [_______] kJSubmit button for entering answer.Feedback: Incorrect; Try Again; 3 attempts remaining.**Part B**Temperature: 1040 KInput box for \( \Delta G^\circ = \) [_______] kJSubmit button for entering answer.**Part C**Temperature: 1400 KInput box for \( \Delta G^\circ = \) [_______] kJSubmit button for entering answer.Request Answer button for further assistance.

We are authorized to answer three subparts at a time, since you have not mentioned which part you are looking for, so we are answering the first three subparts, please repost your question separately for the remaining subpart.The given chemical reaction is, CaCO3s→CaOs+CO2g The enthalpy of the reaction ∆H° is calculated by the formula, ∆H°=∆fH°CaO+∆fH°CO2-∆fH°CaCO3 Where, ∆fH°CaO is the standard enthalpy of formation of CaO (s) (-634.9 kJ/mol). ∆fH°CO2 is the standard enthalpy of formation of CO2 (g) (-393.51 kJ/mol). ∆fH°CaCO3 is the standard enthalpy of formation of CaCO3 (s) (-1220.0 kJ/mol). Substitute the standard formation enthalpy of CaO, CO2 and CaCO3 in the above formula. ∆H°=-634.9 kJ/mol-393.51 kJ/mol--1220.0 kJ/mol=-1028.41 kJ/mol+1220.0 kJ/mol=191.59 kJ/molThe entropy change of the reaction ∆S° is calculated by the formula, ∆S°=S°CaO+S°CO2-S°CaCO3 Where, S°CaO is the standard entropy of CaO (s) (38.1 J/mol K). S°CO2 is the standard entropy of CO2 (g) (213.8 J/mol K). S°CaCO3 is the standard entropy of CaCO3 (s) (110.0 J/mol K). Substitute the standard entropy of CaO, CO2 and CaCO3 in the above formula. ∆S°=38.1 J/mol K+213.8 J/mol K-110.0 J/mol K=251.9 J/mol K-110.0 J/mol K=141.9 J/mol KPart A The Gibbs free energy is calculated by the formula, ∆G°=∆H°-T∆S°......(1) Where, T is the temperature. The given temperature is 305 K. Substitute the value of enthalpy change, entropy change and temperature in equation (1). ∆G°=191.59 kJ/mol-305 K×141.9 J/mol K=191.59 kJ/mol-43279.5 J/mol=191.59 kJ/mol-43.2795 kJ/mol=148.31 kJ/molPart B The given temperature is 1040 K. Substitute the value of enthalpy change, entropy change and temperature in equation (1). ∆G°=191.59 kJ/mol-1040 K×141.9 J/mol K=191.59 kJ/mol-147576 J/mol=191.59 kJ/mol-147.576 kJ/mol=44.01 kJ/molPart C The given temperature is 1400 K. Substitute the value of enthalpy change, entropy change and temperature in equation (1). ∆G°=191.59 kJ/mol-1400 K×141.9 J/mol K=191.59 kJ/mol-198660 J/mol=191.59 kJ/mol-198.660 kJ/mol=-7.07 kJ/molAnswer: The value of ∆G° at 305 K is 148.31 kJ. The value of ∆G° at 1040 K is 44.01 kJ. The value of ∆G° at 1400 K is -7.07 kJ.

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Consider the following reaction: CACO3 (s) → CaO (s) + CO2 (g). Estimate AG for this reaction at each of the following temperatures. (Assume that AH° and AS° do not change too much within the given temperature range.) Part A 305 K AG° = kJ Submit Previous Answers Request Answer X Incorrect; Try Again; 3 attempts remaining Part B 1040 K AG° = kJ Submit Request Answer Part C 1400 K

Consider the following reaction: CACO3 (s) → CaO (s) + CO2 (g). Estimate AG for this reaction at each of the following temperatures. (Assume that AH° and AS° do not change too much within the given temperature range.) Part A 305 K AG° = kJ Submit Previous Answers Request Answer X Incorrect; Try Again; 3 attempts remaining Part B 1040 K AG° = kJ Submit Request Answer Part C 1400 K

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 92QRT

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Question

**Exercise 18.66**

Consider the following reaction:
\[ \text{CaCO}_3(s) \rightarrow \text{CaO}(s) + \text{CO}_2(g) \]

Estimate \(\Delta G^\circ\) for this reaction at each of the following temperatures. (Assume that \(\Delta H^\circ\) and \(\Delta S^\circ\) do not change too much within the given temperature range.)

**Part C**
- Temperature: 1400 K
- \(\Delta G^\circ\) = _____ kJ

**Part D**
Predict whether or not the reaction in part A will be spontaneous at 305 K.
- Options:
- Spontaneous
- Nonspontaneous

**Part E**
Predict whether or not the reaction in part B will be spontaneous at 1040 K.
- Options:
- Spontaneous
- Nonspontaneous

**Instructions:**
Use the information given to calculate or predict the spontaneity of the reaction at the specified temperatures. Use the provided tools to submit your answers or request guidance if necessary.

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