The ΔH° for a reaction is 80.0 kJ mol⁻¹ and ΔS° is 0.213 kJ mol⁻¹ K⁻¹. Calculate the ΔG° for this reaction at 298 K.**Explanation:**To calculate ΔG° (Gibbs free energy change) at a temperature of 298 K (25°C), we can use the Gibbs free energy equation:\[ \Delta G° = \Delta H° - T\Delta S° \]Where:- \( \Delta G° \) is the change in Gibbs free energy,- \( \Delta H° \) is the change in enthalpy (80.0 kJ/mol),- \( T \) is the temperature in Kelvin (298 K),- \( \Delta S° \) is the change in entropy (0.213 kJ/mol·K).Substituting the given values:\[ \Delta G° = 80.0 \, \text{kJ/mol} - (298 \, \text{K} \times 0.213 \, \text{kJ/mol·K}) \]Calculate to find the value of \( \Delta G° \).

Answered: Image /qna-images/answer/5c771f5d-ff95-4a63-8284-bceb8d5d242f.jpg

Answered: The AHⓇ for a reaction is 80.0 kJ mol-¹…

Science

Chemistry

The AHⓇ for a reaction is 80.0 kJ mol-¹ and AS is 0.213 kJ mol¹ K1¹. Calculate the AG° for this reaction at 298 K.

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

Related questions

Q: Use standard thermodynamic data (in the Chemistry References) to calculate AG at 298.15 K for the…

A: Given, Pressure of all gases 12.59mmHg 2SO2(g) + O2(g) -------> 2SO3(g)

Q: Use the data in table 4 to calculate the ΔH⁰ and ΔS⁰ for the dissolution of KNO3. Show your workwith…

A: The problem is asking us to calculate the enthalpy change (ΔH⁰) and entropy change (ΔS⁰) for the…

Q: Consider the reaction: A (aq) B (aq) at 295 K under standard conditions. If AG° is -5.83 kJ at this…

A: The objective of the question is to determine the concentration of reactant "A" that would change…

Q: 7) Ethanol, is produced by fermentation of the glucose in fruit or grain. The reaction is: C,H1206…

Q: True or False? For any non spontaneous reaction. As the free gibbs energy decreases , the reaction…

A: Explanation to the correct answer is given below.

Q: determine whether the following reactions are spontaneous under standard conditions. (a) Cu1s2 + 2…

A: Concept introduction: Spontaneous reaction: It is the reaction which occurs without any specific…

Q: For the reaction 2NH3(g) + 3N₂O(g) → 4N₂ (9) + 3H₂O(g) = -879.5 kJ and AS = 288.1 J/K The standard…

A: According to the second law of thermodynamics, the spontaneous nature of the reaction is determined…

Q: The value of ΔGo for the precipitation reaction, Ca2+(aq) + CO32-(aq) CaCO3(s) is -48.1 kJ at 298…

Q: (a) Calculate AGixn for the dissolution of AgCl(s). kJ . mol- (b) Calculate the solubility-product…

A: We have calculated the ΔG°rxn and Ksp of dissolution of AgCl and AgBr.

Q: 30. When H₂SO4 dissolves in water, SO2 and Hare formed and the temperature of the solution…

A: The dissolution of H2SO4 in water involves the formation of (SO4)2- and H+ ions and is exothermic,…

Q: Adenosine triphosphate (ATP) is a compound that provides energy for biomechanical reactions in the…

A: Given: ΔH = -20.0 KJ/mol = -20000 J/mol. And ΔS = 34.0 J/K.

Q: Use the data given here to calculate the values of AGin at 25 °C for the reaction described by the…

A: Gibbs free energy is a thermodynamical quantity that measures the feasibility of the reaction Here…

Q: Use the data in table 4 to calculate the ΔH⁰ and ΔS⁰ for the dissolution of KNO3. Show your workwith…

A: The problem is asking us to calculate the enthalpy change (ΔH⁰) and the entropy change (ΔS⁰) for the…

Q: For the reaction Fe3O4(s) + 4H2(g)- →3F€(s) + 4H20(g) AH° = 151.2 kJ and AS° = 169.4 J/K The…

A: Standard free energy change for the reaction is given by the expression ∆Go=∆Ho-T∆So

Q: Use the data given here to calculate the values of AGan at 25 °C for the Compound AG; (kJ/mol)…

Q: A student determines the value of the equilibrium constant to be 1.08×106 for the following…

A: Equilibrium Constant, Keq = 1.08 × 106 Temperature, T = 298 K Gas constant, R = 8.314 J K-1 mol-1…

Q: Determine AG° for a reaction when AG = -171.0 kJ/mol and Q = 0.043 at 298 K. (R = 8.314 J/mol K) ●

A: G = -171.0 KJ /mol = -171.0 x 103 J/molQ = 0.043 at 298 KR = 8.314 J/ mol .K

Q: Calculate AG ° of the following reaction: 2 C (s) + H2 (g) → C2H2 (g) AG2 + Use Hess' Law, AG°= AG¡…

Q: For a certain chemical reaction, the standard Gibbs free energy of reaction is -104. kJ. Calculate…

Q: Use the data given in the table to calculate the value of AGxn at 25° C for the reaction described…

A: Step 1:Given reaction:A+B⇌CGibbs free energy change for this reaction will be equal to the…

Q: Use the data given in the table to calculate the value of AGixn at 25° C for the reaction described…

A: Gibbs free energy can be defined as the amount of energy required to do useful work during a…

Q: Calculate AG° and K, at 25 °C for the reaction 2 SO3(g) – 2 SO2(g) + O2(g) Is the reaction…

A: The chemical reaction is: 2SO3(g) → 2SO2(g) + O2(g) Given, G0f (SO3(g)) = -371.06 kJ/mol G0f…

Q: Calculate Ecer in V at 298 K when [Cr(NO:):] is 0.125 M, the pressure of H2(g) is 1.50 atm, and the…

A: Given: The concentration of [Cr(NO3)]=0.125 M. The pressure of H2(g)=1.50 atm. The pH = 9.463= - log…

Q: For a spontaneous endothermic chemical reaction with ArxnH°= +20.6 kJ/mol, the equilibrium constant…

Q: e the solubility-product constant of AgCl. AG¡X for the dissolution of AgBr(s). e the…

A: The question is based on the concept of chemical thermodynamics. we have to calculate solubility…

Q: Determine AG° for the the reaction 2 NO2(g) → 2 NO(g) + O2(g) at 25°C. Substance AGt (kJ/mol) NO2…

A: ∆G°f for NO2 (g) = 51.3 KJ/mol ∆G°f for NO (g) = 86.6 KJ/mol ∆G°f for O2 (g) = 0 ( The standard…

Q: The value of Ke for the reaction A= B is 0.425 at 50.0°C and 0.625 at 100.0°C. Calculate AH° for the…

A: Given reaction A <--> B Kc = 0.425 at T1 = 50°C = 323 K Kc = 0.625 at T2 = 100°C = 373 K

Q: The standard reaction free energy AG-835. kJ for this reaction: 2 Al(s) + Fe₂O3(s)-Al₂O3(s) + 2…

A: Answer: Given chemical reaction: 2Al(s)+Fe2O3(s)→Al2O3(s)+2Fe(s) Gibbs free energy change for this…

Q: Use the data given in the table to calculate the value of AGin at 25° C Compound AG (kJ/mol) rxn for…

A: Hello. Since your question has multiple parts, we will solve the first question for you. If you want…

Q: None

Q: Solve the following problems. Write your solution and box your final answer.

A: Standard free energy change for the given reaction can be calculated from the standard enthalpy of…

Q: Determine the value of AG° at 25 °C for the reaction below given the following data: CH,(g) AG = 68…

Q: calculate the ▲G0 for a reaction with a Keq of 1.0 X 103 at 298 K.

A: The equation connecting free energy change and equilibrium constant is given below: ΔG0 = -RTlnKeq…

Q: Consider the reaction 3 CH4(g)----->C3H8(g) + 2 H2(g).(a) Calculate ΔG° at 298 K.(b) Calculate ΔG…

A: 3CH4g ↔ C3H8g + 2H2g (a) ∆ Go = ∆ Gproducts - ∆ Greactants ∆G (H2) = 0 kJ/mol ∆G (C3H8) = -23.47…

Q: For the reaction 4HCI(g) + O2(g)- →2H2O(g) + 2C1½(g) AH° = -114.4 kJ and AS° = -128.9 J/K The…

A: Thermodynamic is the branch of chemistry that mainly deals with the heat transfer between system and…

Q: For the reaction Co(g) + 3H2(g)– CH4(g) + H2O(g) AH° = -206.1 kJ and AS° = -214.7 J/K The standard…

A: In Part-A we will determine the ∆G° value and direction of Reaction. But, in Part-B we will…

Q: For an ideal solution containing 500 g toluene (92.14 g/mol) and 300 g xylene (106.16 g/mol)…

A: No of moles of toluene and xylene are calculated as follows: ntoulene=500 g92.14 g/mol=5.4265…

Q: Use the data given here to calculate the values of AGixn at 25 °C for the reaction described by the…

A: Given A + B ⇔ C ∆Grxn0 = To be determined Compound ∆Gf0 (kJ/mole) A +387.7 B -596.8 C…

Q: For the reaction CHĄ(g) + H,O(g)–→3H,(g) + CO(g) AH° = 206.1 kJ and AS° = 214.7 J/K The standard…

Question

The ΔH° for a reaction is 80.0 kJ mol⁻¹ and ΔS° is 0.213 kJ mol⁻¹ K⁻¹. Calculate the ΔG° for this reaction at 298 K.

**Explanation:**

To calculate ΔG° (Gibbs free energy change) at a temperature of 298 K (25°C), we can use the Gibbs free energy equation:

\[ \Delta G° = \Delta H° - T\Delta S° \]

Where:
- \( \Delta G° \) is the change in Gibbs free energy,
- \( \Delta H° \) is the change in enthalpy (80.0 kJ/mol),
- \( T \) is the temperature in Kelvin (298 K),
- \( \Delta S° \) is the change in entropy (0.213 kJ/mol·K).

Substituting the given values:

\[ \Delta G° = 80.0 \, \text{kJ/mol} - (298 \, \text{K} \times 0.213 \, \text{kJ/mol·K}) \]

Calculate to find the value of \( \Delta G° \).

Expert Solution

Step 1: Concept

Step by step

Solved in 3 steps with 3 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Use the data in table 4 to calculate the ΔH⁰ and ΔS⁰ for the dissolution of KNO3. Show your workwith annotated calculations.
A student determines the value of the equilibrium constant to be 8.14x10-37 for the following reaction. H,S(g) + 2H,0(1)–→3H,(g) + SO>(g) Based on this value of Keg AG° for this reaction is expected to be (greater, less) than zero. Calculate the free energy change for the reaction of 2.03 moles of H,S(g) at standard conditions at 298K. AG°rxn kJ Ixn
The combustion of acetylene is used in welder's torches because it produces a very hot flame: 5 C₂ H2(g) + O2(g) → 2 CO₂ (g) + H₂O(g) AH = -1255.5 kJ Substance Sº (J mol-¹ K-¹) C₂ H₂(g) 200.8 O₂(g) CO₂(g) H₂O(g) 205.0 213.6 188.7
Use the data provided in the table to calculate the change in Gibbs Free-Energy at 25 degrees Celsius for the reaction given. Ag+ (aq) Cl- (aq) AgCl (s) S0 (J K-1 mole-1) 72.68 56.4 96.2 Delta H Kj/mol 105.58 -167.2 -127.07 Group of answer choices -75.2 kJ +55.7 kJ +32.5 kJ -75.2 kJ -55.7 kJ
A student determines the value of the equilibrium constant to be 6.29×104 for the following reaction.S(s,rhombic) + 2CO(g)SO2(g) + 2C(s,graphite)Based on this value of Keq:G° for this reaction is expected to be (greater, less) fill in the blank than zero.Calculate the free energy change for the reaction of 1.85 moles of S(s,rhombic) at standard conditions at 298K. G°rxn = _____ kJ
14
Under the conditions shown below for the following reaction. Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g) AG° = -28.0 kJ P(CO) = 4.2 atm, P(CO2) = 1.8 atm Calculate AGrxn at 298 K, and indicate if the reaction is more or less spontaneous under these conditions than under standard conditions?
What is the standard free energy change for the ionization of H2O2 acid, if its Ka is 2.40e-12. 66.326 kJ -66.326 kJ -152.749 kJ 152.749 kJ
Determine AG (in kJ) for the following reaction at 325 K when the concentrations of the species are as follows: NO₂= 10.00 M, N₂O4 = 14.3 M. AG°f (NO₂) = 51 kJ/mol, AG (N₂O4) = 97.7 kJ/mol. 2 NO2(8) N₂O4(8)
For the reaction A(aq) ---> B(aq) the variation in the standard free enthalpy is 3.50 kJ at 25 oC and 4.64 kJ at 45 oC. Calculate the value of the equilibrium constant for this reaction at 75°C.
Determine the value of K for a reaction where AG° = -29.62 kJ/mol at 298 K. K =
Explain pleaseeeeeeeeeee