**Gibbs Free Energy: Spontaneity**Gibbs free energy is a measure of the spontaneity of a chemical reaction. It is the chemical potential for a reaction and is minimized at equilibrium. The change in Gibbs free energy can be calculated by:\[\Delta G^\circ_{\text{rxn}} = \Delta H^\circ_{\text{rxn}} - T\Delta S^\circ_{\text{rxn}}\]where \(\Delta G^\circ_{\text{rxn}}\) is the standard Gibbs free energy change for a reaction, \(\Delta H^\circ_{\text{rxn}}\) is the standard enthalpy change for a reaction, \(T\) is the temperature in kelvins, and \(\Delta S^\circ_{\text{rxn}}\) is the standard entropy change for a reaction.For a reaction at equilibrium, \(\Delta G^\circ_{\text{rxn}}\) is equal to zero. For negative values, the reaction is spontaneous, and for positive values, the reaction is nonspontaneous.**Elemental Carbon Forms**Elemental carbon usually exists in one of two forms: graphite or diamond. It is generally believed that diamonds last forever. The table shows the standard enthalpy of formation \((\Delta H^\circ_f)\) and the standard molar entropy \((S^\circ)\) values for diamond and graphite.| Substance | \(\Delta H^\circ_f\) (kJ/mol) | \(S^\circ\) (J/mol·K) ||-------------|-------------------------------|-----------------------|| \(C_{\text{graphite}}\) | 0 | 5.740 || \(C_{\text{diamond}}\) | 1.897 | 2.38 |**Part A**What is the standard Gibbs free energy for the transformation of diamond to graphite at 298 K?\[ C_{\text{diamond}} \rightarrow C_{\text{graphite}} \]Express your answer to three significant figures and include the appropriate units.- **Answer Box:** \(\Delta G^\circ_{\text{rxn}} = [ \text{Value} \quad \text{Units} ]\)- **Submit Button**: Submit- **Feedback**: Incorrect; Try Again, 5 attempts remainingFor hints and templates, click "View Available

Answered: Image /qna-images/answer/4cb976d5-0e8d-4bd8-a8f0-a16667f85db3.jpg

Elemental carbon usually exists in one of two forms: graphite or diamond. It is generally believed that diamonds last forever. The table shows the standard enthalpy of formation ( AHP) and the standard molar entropy (S) values for diamond and graphite. Part A AGion= What is the standard Gibbs free energy for the transformation of diamond to graphite at 298 K? Cdiamond graphite Express your answer to three significant figures and include the appropriate units. ▸ View Available Hint(s) Submit Substance Cgraphite Cdiamond Previous Answers ΔΗ} (kJ/mol) 0 1.897 Templates Symbols undo regio Teset keyboard shortcuts help V Value Units S (J/mol. K) 5.740 2.38

Elemental carbon usually exists in one of two forms: graphite or diamond. It is generally believed that diamonds last forever. The table shows the standard enthalpy of formation ( AHP) and the standard molar entropy (S) values for diamond and graphite. Part A AGion= What is the standard Gibbs free energy for the transformation of diamond to graphite at 298 K? Cdiamond graphite Express your answer to three significant figures and include the appropriate units. ▸ View Available Hint(s) Submit Substance Cgraphite Cdiamond Previous Answers ΔΗ} (kJ/mol) 0 1.897 Templates Symbols undo regio Teset keyboard shortcuts help V Value Units S (J/mol. K) 5.740 2.38

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

NO.2 AH fusion for water at o°C is 1436 cal mol·1. Cp value for solid and liquid H,O is 8.9 and 18.0 cal K-1 mol-1 respectively. Determine molar enthalpy and molar entropy for this process. Н,О (5, -10°C) Н,о (1, 0°C)
Calculate the standard entropy change for the following process: H2 O(g) ⟶ H2 O(l)
What is the change in Gibb's Free Energy for a reaction that has an enthalpy change of -17.9 kJ/mol and a entropy change of -138.3 J/(mol K) at 56.7 °C? Your Answer: Answer units
The heat of vaporization AH, of heptane (C-H₁6) is 31.2 kJ/mol. Calculate the change in entropy AS when 736. g of heptane condenses at 98.4 °C. Be sure your answer contains a unit symbol. Round your answer to 3 significant digits. x10 ロ・ロ X H ■
Ip acellus_engine.html?ClassID=D1653724337# Calculate the entropy of the phase change of uranium hexafluoride from gas to solid. UF6(g) → UF6(s) Substance S° (J/mol-K) UF (s) UF (g) ASiep = [ ? ] J/mol - K 228 380 Enter either a + or - sign AND the magnitude in your answer. Enter
For the following reaction (the detonation of nitroglycerin), is it spontaneous under standard conditions and how can you tell? 4 C4H5N3O9(l) (arrow >) 12 CO2(g) + 10 H2O(g) + 6 N2(g) + O2(g) ΔH = -5678 kJ
Use the observations about each chemical reaction in the table below to decide the sign (positive or negative) of the reaction enthalpy AH and reaction entropy AS. Note: if you have not been given enough information to decide a sign, select the "unknown" option. reaction observations conclusions ΔΗ is (pick one) A The reverse of this reaction is always spontaneous. As is (pick one) ΔΗ is (pick one) B This reaction is spontaneous only below 20. °C. As is (pick one) с This reaction is spontaneous except below 85. °C but proceeds at a slower rate below ΔΗ is (pick one) 129. °C. As is (pick one) ×
The heat of fusion AH, of acetic acid (HCH₂CO₂) is 11.7 kJ/mol. Calculate the change in entropy AS when 5.7 g of acetic acid melts at 17.0 °C. Be sure your answer contains a unit symbol. Round your answer to 2 significant digits.
.The heat of vaporization AH, of diethyl ether ((CH), (CH), 0) is 26.7 kJ/mol. Calculate the change in entropy AS when 877. g of diethyl ether boils at 34.6 °C. Be sure your answer contains a unit symbol and the correct number of significant digits. 0.0 μ X 号 5 D
Use the observations about each chemical reaction in the table below to decide the sign (positive or negative) of the reaction enthalpy AH and reaction entropy AS. Note: if you have not been given enough information to decide a sign, select the "unknown" option. reaction observations conclusions AH is A This reaction is always spontaneous, but proceeds slower at temperatures below 45. °C. AS is ΔΗ is This reaction is spontaneous only above 150. °C but proceeds at a faster rate above 180. °C. AS is ΔΗ is This reaction is exothermic and proceeds slower at temperatures below 67. °C. AS is X C (pick one) (pick one) (pick one) (pick one) ✓ (pick one) (pick one) Ś ?
Please don't provide handwriting solution