Answered: Calculate ΔG^0 (in kJ/mol) given ΔG=…

Calculate ΔG^0 (in kJ/mol) given ΔG= -833.7 kJ/mol and R= 0.008314 kJ/mol K and T= 261.5 K and Q=0.623 ΔG=ΔG^0+RTlnQ A) -836 B) -833 C) -834 D) -833 E) -710

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

Chapter17: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 2ALQ: For a liquid, which would you expect to be larger, Sfusion or Sevaporation? Why?

See similar textbooks

Related questions

Q: Calculate AG°nxn: AG°rxn= kJ Part 3 Which phrase best describes this reaction under standard…

A: The standard enthalpy change and the entropy change of the reaction are given by: ∆H° = ∑∆H°f…

Q: 3) Consider the reaction: 3) _ N2(8) + 3 F2(g) -2 NF3(g) AH® = -249 kJ and AS = -278 J/K at 25°C %3D…

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

Q: For a particular reaction at 212.7 °C, ΔG=−843.71 kJ, and ΔS=603.37 J/K. Calculate ΔG for this…

A: Given : At temperature 212.7 °C, ΔG = -843.71 KJ = -843710 J…

Q: Consider the following reaction: CO2(g) + CC4 (g) = 2COC12(g) Calculate AG for this reaction at 25…

Q: Cite at least 3 examples of non-spontaneous phenomena.

A: This question belong to thermodynamics concept of spontaneity. We know that, ∆G = ∆H-T∆S…

Q: What is ΔG° at 25 ºC for a process that has ΔH° = −35.4 kJ/mol and ΔS° = −153 J/mol·K? 45.6 kJ/mol…

A: Given: ΔH° = −35.4 kJ/mol ΔS° = −153 J/mol·K Temperature T = 25 ºC = 273 + 25 = 298 K

Q: 12. Consider the oxidation of iron metal 4Fe +302g → 2Fe,O) . by determining the sign of Astotal,…

Q: Estimate the normal boiling point of titanium tetrachloride, TiCl4, at 1 atm pressure, using the…

A: Since the normal boiling point of any molecule is given by Tb = ΔHeva / ΔSeva where ΔHeva = change…

Q: Calculate AH for the process: Hg, Cl2 (s) → 2Hg(e) + Cl2(g) from the following information: Hg(t) +…

Q: Given the following data P(s) + 6Cl;(g) 4PC1,(g) AH = -1225.6 kJ %3D P,(s) + 50,(g) – AH = -2967.3…

Q: 73. Given the following data Ca(s) + 2C(graphite) → CaC2(s) Ca(s) + O,(g) –→ CaO(s) CaO(s) + H,O(1)…

Q: Given the AH° and AS°, calculate the AG° values for the following reactions and indicate whether the…

Q: Determine ∆G° for the phase change CO₂(g) → CO₂(aq) at 25°C.

Q: (7) Calculate A G° for the reaction given the following information: 2502(g) + 02(g)→ 2s0;(g) AG for…

Q: Calculate ΔS° (J/mol-K) for the reaction below, given the thermodynamic data in the table. Report…

Q: 1. CaHa() + 502(g) 3CO20) + 4H2O(g) ; AH° = -2045 kJ %3D a. Calculate AG° b. What is the spontaneous…

A: Answer

Q: The element oxygen was prepared by Joseph Priestley in 1774 by heating merc HgO(s) → Hg(I) +…

A: The question is based on spontaneity of the reaction. we have to determine the temperature at which…

Q: If the Delta*H = 135kJ / m * ol and AS 92 J/K mol, at what temperature does this reaction become…

Q: (a) Is an endothermic reaction more likely to be sponta-neous at higher temperatures or lower…

A: Since you have posted multiple questions, we will solve only one question for you. If you any…

Q: Using the thermodynamic information: 1/2 N2(g) + 1/2 02(g)--> N0(g) delta H degrees = 90.4 kJ/mol…

Q: When an instant hot pack is activated, aqueous sodium acetate crystallizes to form a solid and heat…

A: Given, At the point when a moment hot pack is enacted, aqueous sodium acetate derivation solidifies…

Q: What is the free energy change when silver chloride form at 2000.0 K? (Use the equation delta G =…

A: Ag+(aq) + Cl–(aq) ----> AgCl(s) Given temperature, T = 2000.0 K ∆Gorxn = ∆Horxn - T…

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: Calculate the value of the free energy change, ΔG, for the reaction below at 250.0ºC when the…

A: using the value given NH3 , N2, H2 all value is given atm so using this calculate the Kp. apply the…

Q: Item 1 I Review | Constants | Periodic Table Elemental carbon usually exists in one of two forms:…

Q: 4 Fe + 30, 2 Fe,O; AS°3ys = - 225 J /K AH® 0.0 0.0 -98.3 kJ/mol What is AS° univ if AS°ys = - 225 J/…

Q: Calculate the value of the free energy change, ΔG, for the reaction below at 100.0ºC when the…

Q: Given the reference thermodynamic data below taken at 25°C, calculate the value of the equilibrium…

A: The reaction for given process is : N2(g) + 3H2(g) ⇌ 2NH3(g) Given that : ΔGº = -32.96 kJΔHº =…

Q: Use the data given to calculate the value of AG°rxn for the reaction at 25°C AgCI(s) Ag (aq) + Cl-…

Q: For the reaction N20 (g) + NO2 (g) →3 NO (g), at 25°C AH° = +155.6 kJ/mol and AS° = +172.4 J/mol K.…

Q: Calculate ∆H°25° for the reaction: Fe3O4(s) + 2 C(s, graphite) → 3 Fe(s) + 2 CO2(g) from the…

A: The given reaction is, Fe3O4(s) + 2 C(s, graphite) → 3Fe(s) + 2CO2(g) The given reactions are, 1)…

Q: Consider an exothermic and non-spontaneous process. make a drawing that represent this process and…

Q: Classify each of the reactions according to one of the four reaction types summarized in the table…

A: a) The reaction and data given is,

Q: Consider the physical process at 1 atm pressure: Br2 (l) --> Br2 (g) where ΔHo = 31.0 kJ/mol and…

A: Br2 (l) --> Br2 (g) ΔHo = 31.0 kJ/mol = 31000 J/mol ΔS = 93.0 J mol-1 K-1

Q: Calculate AHxn for the reaction 2Ni(s) + 2S(s) + 30,(g) → 2Niso,(s) from the following information:…

Q: At what temperature, in K, does X (l)-->X(g) occurr spontaneously? Delta H°=+573 kj/mol Delta…

A: Given that: Delta H° for the reaction = 573 KJ/mol Delta S° for the…

Q: A silver cube with an edge length of 2.38 cm and a gold Substance Specific heat (J/g-°C) Density…

A: Given : Edge length of silver cube = 2.38 cm Edge length of gold cube = 2.66 cm Initial…

Q: Consider the reaction described by the chemical equation shown. 3C,H,(g) → C,H,(1) AHn = -633.1 kJ…

Q: The standard Gibbs free energy (∆G°rxn) for the formation of sulfur trioxide from sulfur dioxide and…

A: Given reaction: SO2 (g) + ½ O2 (g) → SO3 (g) The standard Gibbs free energy (∆G°rxn) for the…

Q: (b) What is the first law of thermodynamic? Define the Hess law. Given the following data; 2CIF(g) +…

Q: The normal freezing point of n-octane (C8H18) is -57 °C.(a) Is the freezing of n-octane an…

A: Given that the freezing point of n-octane is -57 oC.

Q: Calculate the enthalpy change for the reaction 2K+ S K28 using the following thermochemical…

A: Given 1)K + S -> KS Delta H = 32.5 KJ 2) KS + K -> K2S Delta H = 38.2 KJ To…

Q: In question #9 you calculated ΔGo at lower temperature, now let's calculate ΔGo at a higher…

A: Given Ksp = 2.2 x 10-8 Temperature T= 99.4 0C = 99.4 +273 = 372.4 K R = 8.314 J/mol K We know that…

Q: Consider the following two reactions for the production of ethanol. (1) C2H4(g) + H20(g) →…

A: The reactions given for production of ethanol are 1. C2H4 (g) + H2O (g) → CH3CH2OH (l) 2. C2H6 (g)…

Q: 9. For the following reaction at 298 K, AS = -308.2 J/K and AH = -192.7 kJ: 4NO(g) N₂O(g) + N₂O₂(g)…

A: Given reaction is 4NO(g) → NO(g) + N₂O3(g) For this reaction at 298 K , ΔS= -308.2 J/K and = -0.3082…

Q: Calculate the enthalpy change for the reaction 2K + S → K2S using the following thermo K+S KS AH…

A: Consider the given target equation for which we have to determine the enthalpy change is as follows;…

Q: For the reaction 4NH3(g) + 5O2(g) ⇄ 6H2O(g) + 4NO(g) ΔG* = −955.6 kJ What is the free energy…

A: The balanced reaction taking place is given as, => 4 NH3 (g) + 5 O2 (g) ⇄ 6 H2O (g) + 4 NO (g)…

Q: 4 Fe 3 0, 2 Fe,O3 AS° sys = - 225 J/K + AH° 0.0 0.0 -98.3 kJ/mol What is AS°uniy if AS° sys = - 225…

Q: 1. From the values of AH and AS, predict which of the following reactions would be spontaneous at…

Question

Calculate ΔG^0 (in kJ/mol) given ΔG= -833.7 kJ/mol and R= 0.008314 kJ/mol K and T= 261.5 K and Q=0.623

ΔG=ΔG^0+RTlnQ

A) -836

B) -833

C) -834

D) -833

E) -710

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 2 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

For a liquid, which would you expect to be larger, Sfusion or Sevaporation? Why?
Substance C₂Hg(g) O₂(g) CO₂(g) H₂O(g) The thermodynamic data calculated above for this reaction C3Hg(g) + 5 O₂(g) AH (kJ/mol) -104.70 0.0 -393.51 -241.8 A,G= AH-2043.0 kJ mol¹ and A,S 100.62 J K mol 3 CO₂(g) + 4H₂O(g) kJ mol-1 Calculate A,G in kJ mol¹ if the reaction mixture is at 146°C. (You have 2 attempts until the answer will be given; you have already tried 0 times) S (J/mol/K) 270.30 205.1 213.74 188.8
Consider the following equation:3C2H2(g) ↔ C6H6(g)ΔGof(C2H2, g) = +209.2 kJ/ mol; ΔGof(C6H6, g) = +129.7 kJ/ molCalculate ΔGo and K for this reaction at 298 K
Calcium ΔHof (kJ/mol) ΔGof (kJ/mol) So (J/mol K) Ca (s) 0 0 41.4 Ca (g) 178.2 144.3 158.9 Ca2+ (g) 1925.9 CaC2 (s) -59.8 -64.9 70.0 CaCO3 (s, calcite) -1206.9 -1128.8 92.9 CaCl2 (s) -795.8 -748.1 104.6 CaF2 (s) -1219.6 -1167.3 68.9 CaH2 (s) -186.2 -147.2 42.0 CaO (s) -635.1 -604.0 39.8 CaS (s) -482.4 -477.4 56.5 Ca(OH)2 (s) -986.1 -898.5 83.4 Ca(OH)2 (aq) -1002.8 -868.1 -74.5 Ca3(PO4)2 (s) -4126.0 -3890.0 241.0 CaSO4 (s) -1434.1 -1321.8 106.7 CaSiO3 (s) -1630.0 -1550.0 84.0 Carbon ΔHof (kJ/mol) ΔGof (kJ/mol) So (J/mol K) C (s, graphite) 0 0 5.7 C (s, diamond) 1.9 2.9 2.4 C (g) 716.7 671.3 158.1 CCl4 (l) -135.4 -65.2 216.4 CCl4 (g) -102.9 -60.6 309.9 CHCl3 (l) -134.5 -73.7 201.7 CHCl3 (g) -103.1 -70.3 295.7 CH4 (g) -74.8 -50.7 186.3 CH3OH (g)…
3) For the phase change Br2(1) → Br2 (g), AH°= +31.0 kJ/mol and AS°= +92.9 J/mol.K. Assuming that AH° and AS° are nearly temperature independent, calculate the approximate Celcius temperature at which Br2(1) will be in equilibrium with Br2(g) at 1 atm.
Consider the dissolution of NaBr and NaI. The values provided here will be helpful for answering the following questions. ΔH∘solnΔHsoln∘ (kJ/mol) ΔS∘solnΔSsoln∘ $$Jmol•K NaBr –0.860 57.0 NaI –7.50 74.0 Write a balanced equilibrium equation for the dissolution of NaI in water. Include phases. Calculate the change in free energy if 0.575 moles of NaI is dissolved in water at 25.0°C. What is the dissolution of 1.00 mol of NaBr at 298.15 K?
Use the data in appendix 4 and the information below to calculate the standard free energy of formation for C4H10(g) 2C4H10(g) + 13O2(g)  8CO2(g) + 10H2O(l) ΔG°= 25490 kJ.
Consider the reaction below and its corresponding thermodynamic data to answer the following question. NH3 (9) + HCI (s)- NH4Cl (s) AH = -175.9 kJ/mol and AS -284.6 J/mol K What is the standard molar Gibbs free energy change, AG", for this reaction at 30°C? -89.7 kJ/mol -84.0 kJ/mol 72.6 kJ/mol 78.3 kJ/mol 66.9 kJ/mol
Calculate ΔG^0cell in kJ/mol at 603 K givenE^0cell= -0.290 voltsn= 1F= 96500 C/mole electronsΔG^0cell=−nFE^0cell a) 28.0 b) 0.000290 c) 252 d) 93.2 e) 12.4
C (graphite) + 4HNO3() → CO2(g) + 4NO2(g) + 2H2O() AH, J/mol) -393.5 33.2 -285.8 -174.1 O -123.9 kJ O - 472.1 kJ O -201.9 kJ O - 404.8 kJ O -135.9 kJ
Using the following data to calculate the value of ΔvapH° (in units of kJ/mol) of water at 365 K: ΔvapH° = 40.7 kJ/mol at 373 K; CP (l) = 75.2 J/mol/K; CP (g) = 33.6 J/mol/K.
Use the following information to calculate the standard free energy change (AG°) and equilibrium constant (K) for the following system: CaCO3(s) = CaO(s) + CO2(g) T= 900.0 °C AH;° values (kJ/mol): CaO(s) = -634.9, CO2(g) = -393.51, CaCO3(s) =–1220.0 %3D S° values (J/mol K): CaO(s) = 110.0, CO2(g) = 213.8, CACO3(s) = 38.1 %3D %3D %3D

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

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

Publisher:

Cengage Learning

Chemistry: An Atoms First Approach

Chemistry

ISBN:

9781305079243

Author:

Steven S. Zumdahl, Susan A. Zumdahl

Publisher:

Cengage Learning

Chemistry

ISBN:

9781133611097

Author:

Steven S. Zumdahl

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

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

Publisher:

Cengage Learning

Chemistry: An Atoms First Approach

Chemistry

ISBN:

9781305079243

Author:

Steven S. Zumdahl, Susan A. Zumdahl

Publisher:

Cengage Learning

Chemistry

ISBN:

9781133611097

Author:

Steven S. Zumdahl

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS