Calculate the standard free-energy change for the following reaction at 25 C degrees. 2Au^3+(aq)+3Ni(s) 2Au(s)+3Ni^2+(aq) Ni2+(aq) + 2e- -> Ni(s) E=-0.26 Au3+(aq) + 3e- -> Au(s) E=+1.498 G= ? KJ Would it be G=1.758? •Chemistry - DrBob222, Sunday, March 31,

90,110 results
1. Chem

For the reaction, 3C2H2(g) ===> C6H6 at 25°C, the standard enthalpy change is -631 kJ and the standard entropy change is -430 J/K, Calculate the standard free energy change (in kJ) at 25°C. What is the formula that relates stand. entropy, enthalpy and

2. Chemistry

Calculate delta G of the reaction at 25 degrees C: 2Au^3+ (aq) + 3Ni(s) 2Au(s) + 3Ni^2+(aq) Au3+ + 3e- ==> Au Eo = +1.50V Ni2+ + 2e- ==> Ni Eo = -0.23 V 2Au3+ + 3Ni ==> 3Ni2+ + 2Au The answer is -1.00 x 10^3 kJ but i'm not getting that answer!!!!!!! please

3. Chemistry

A solution of AuCl- is mixed with a solution of Sn2+ under standard conditions. What is the equation? the answer is 2AuCl4- + 3Sn2+ -> 3Sn4+ + 2Au + 8Cl- how do i get this? ITS desperate... plz help me! THANK_YOU SO MUCH!

4. Chemistry

C2H2(g) + 2 H2(g)--> C2H6(g) Information about the substances involved in the reaction represented above is summarized in the following tables. Substance So (J/mol∙K) ∆Hºf (kJ/mol) C2H2(g) 200.9 226.7 H2(g) 130.7 0 C2H6(g) - - -84.7 Bond Bond Energy

5. Chemistry

Calculate the standard entropy, ΔS°rxn, of the following reaction at 25.0 °C using the data in this table. The standard enthalpy of the reaction, ΔH°rxn, is –44.2 kJ·mol–1. C2H4(G)+H20 ---> C5H5OH ΔS°rxn= ______ J*K^-1*mol^-1 Then, calculate

6. Chemistry

The standard internal energy change for a reaction can be symbolized as ΔU°rxn or ΔE°rxn. For the following reaction equations, calculate the energy change of the reaction at 25 °C and 1.00 bar. Sn(s) + 2Cl2(g) --> SnCl4(l) ΔH°rxn = -511.3 kJ/mol

7. chemistry

The standard internal energy change for a reaction can be symbolized as ΔU°rxn or ΔE°rxn. For the following reaction equations, calculate the energy change of the reaction at 25 °C and 1.00 bar. Sn(s) + 2Cl2(g) --> SnCl4(l) ΔH°rxn = -511.3 kJ/mol

8. Chemistry

Calculate the standard free-energy change for the following reaction at 25 C degrees. 2Au^3+(aq)+3Ni(s) 2Au(s)+3Ni^2+(aq) Ni2+(aq) + 2e- -> Ni(s) E=-0.26 Au3+(aq) + 3e- -> Au(s) E=+1.498 G= ? KJ Would it be G=1.758? •Chemistry - DrBob222, Sunday, March

9. Chemistry

For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction 2NO(g) + O2(g) --> 2NO2(g) the standard change in Gibbs free energy is ΔG° = -69.0 kJ/mol. What is ΔG for this reaction at 298 K when

10. chemistry

Calculate the standard free-energy change for the following reaction at 25 °C. 2Au^3+(aq) + 3Ni(s) -->2Au(s) + 3Ni^2+(aq)

11. Chemistry

For the reaction 2CO2(g) + 5H2(g)C2H2(g) + 4H2O(g) H° = 46.5 kJ and S° = -124.8 J/K The standard free energy change for the reaction of 1.75 moles of CO2(g) at 328 K, 1 atm would be ___ kJ This reaction is (reactant, product) ____ favored under standard

12. Chemistry

Predict the standard cell potential and calculate the standard reaction Gibbs free energy for galvanic cells having the following cell reactions: a.)3Zn + 2Bi3+ = 3Zn2+ + 2Bi b.)2H2 + O2 = 2H20 in acidic solution c.)2H2 + O2 = 2H20 in basic solution

13. chemistry

for the reaction 3C2H2=> C6H6 at 25 C, the standard enthalpy change is -631 KJ and the standard entropy change is -430 J/K. calculate the standard free energy change at 25 C. show all work!

14. Chemistry

C2H2(g) + 2 H2(g)--> C2H6(g) Information about the substances involved in the reaction represented above is summarized in the following tables. Substance/ So (J/mol∙K) /∆Hºf (kJ/mol) C2H2(g) / 200.9 / 226.7 H2(g)/ 130.7 / 0 C2H6(g)/ ?? / -84.7 Bond

15. Chemistry

The standard reduction potential for Cr3+(aq) is −0.74 V. The half-reaction for the reduction of Cr3+(aq) is the following. Cr3+(aq) + 3 e− → Cr(s) The standard reduction potential for Ni2+(aq) is −0.26 V. The half-reaction for the reduction of

16. General Chemistry

The problem is: Calculate the standard free-energy change for the following reaction at 25 degrees Celsius. 2Au^+3(aq) + 3Cr(s)-> 2Au(s) + 3Cr^+2(aq) I worked it out, getting half reaction: Au^3+ + 3e- -> Au; E = 1.498 Cr^3+ + 3e- -> Cr; E = -0.74 Ecell =

17. chemistry

QUESTION: Calculate the standard free-energy change (deltaG°) for the following reaction at 25 °C in kJ. 2Ag^3+(aq) + 3Zn(s) 2Au(s) + 3Zn^2+(aq) here's what i have so far: first i wrote out the half reactions: Au^3+(aq) + 3e^- --> Au(s) = +1.52*2 Zn(s)

18. Chemistry

The standard free energy change, delta f G, for the formation of NO (g) from its elements is +86.58 kJ/mol at 25 degrees C. Calculate Kp at this temperature for the equilibrium 1/2 N2(g) + 1/2 O2(g) = NO(g) Comment on the sign of delta G and the magnitude

19. Biochemistry

How do you calculate the free energy change for the acetyl phospahate hydrolysis in a solution of 2 mM acetate, 2 mM phosphate and 3 nM acetyl phosphate. The standard state free energy of hydolysis of acetyl phosphate is /\G = -42.3 kJ/mol.

20. Chemistry

Calculate the standard free-energy change for the following reaction at 25 °C. Standard reduction potentials can be found here. 2Au^3+(aq) + 3Cr(s) 2Au(s) + 3Cr^2-(aq)

21. Chemistry

Calculate the standard free-energy change for the following reaction at 25 °C. Standard reduction potentials can be found here. 2Au(3+) + 3Cr-->2Au+3Cr(2+)

22. Chemistry

The problem is: Calculate the standard free-energy change for the following reaction at 25 degrees Celsius. 2Au^+3(aq) + 3Cr(s)-> 2Au(s) + 3Cr^+2(aq) I worked it out, getting half reaction: Au^3+ + 3e- -> Au; E = 1.498 Cr^3+ + 3e- -> Cr; E = -0.74 Ecell =

23. Chemistry

A reaction has a standard free-energy change of –10.30 kJ mol–1 (–2.462 kcal mol–1). Calculate the equilibrium constant at 25ºC.? This is what I've done so far.. ∆Gº= -2.3 RT + log (K) -10.31 kJ = -2.3 (.0083145)(298) + log K -10.31 kJ = -2.3

24. chemistry 2

for the reaction 2C2H2(g)=>C6H6(l) at 25 C, the standard enthalpy change is -631 kJ and the standard entropy change is -430 J/K. calculate the standard free energy change at 25 C. show all work Help please!

25. Chemistry

Gold can be recovered from sea water by reacting the water with zinc, which is refined from zinc oxide. The zinc displaces the gold in the water. What mass of gold can be recovered if 2.00g of ZnO and an excess of sea water are available? 2ZnO + C -> 2Zn +

26. Chemistry

The standard free energy of activation of a reaction A is 73.4 kJ mol–1 (17.5 kcal mol–1) at 298 K. Reaction B is one million times faster than reaction A at the same temperature. The products of each reaction are 10.0 kJ mol–1 (2.39 kcal mol–1)

27. Chemistry

At 25 °C, the equilibrium partial pressures for the following reaction were found to be PA = 4.10 bar, PB = 5.60 bar, PC = 1.20 bar, and PD = 9.70 bar. 2A(g)+2B(g)-->C(g)+ 3D(g) What is the standard change in Gibbs free energy of this reaction at 25 °C.

28. AP Chemistry

(a) When 300.0 milliliters of a solution of 0.200 molar AgNO3 is mixed with 100.0 milliliters of a 0.0500 molar CaCl2 solution, what is the concentration of silver ion after the reaction has gone to completion? (b)Write the net cell reaction for a cell

29. chemistry

Calculate the temperature at which it is thermodynamically possible for C (s) to reduce iron(III) oxide by the reaction: 2Fe2O3 (s) + 3 C (s) ---> 4Fe (s) + 3CO2 I don't need a specific answer, but I'm not sure how to approach the problem. I'm assuming it

30. Chemistry

Calculate the standard reaction Gibbs free energy for the following cell reactions: a.)3Cr3+(aq) + Bi(s)= 3Cr2+(aq) + Bi3+(aq) with Ecell=-.61V b.)Mg(s) + 2H20(l)=Mg2+(aq)+H2(g)+2OH-(aq) with Ecell=2.36 V I know the formula. I just need help figuring out n

31. Chemistry

Calculate the cell potential for the following reaction as written at 25.00 °C, given that [Cr2 ] = 0.859 M and [Ni2 ] = 0.0190 M. Standard reduction potentials can be found here. Cr+Ni(2+) ->Cr(2+) + Ni

32. Chemistry

The standard electrode potential for Zn/Zn2+ and cu/cu2+ are -0.96volts and +0.3volts respectively at 293k.(a) calculate the free energy change when a zinc rod dips into 1M of zinc tetraoxosulphate(vi) solution and a copper rod dips into a 1M of copper

33. Chemistry

Calculate the standard free-energy change for the following reaction at 25 C degrees. 2Au^3+(aq)+3Ni(s) 2Au(s)+3Ni^2+(aq) Ni2+(aq) + 2e¨C ¡ú Ni(s) E=¨C0.26 Au3+(aq) + 3e¨C ¡ú Au(s) E=+1.498 G= ? KJ Would it be G=1.758?

34. Chemistry Question

Calculate the ∆G˚ for the oxidation of nickel in the following balanced reaction. 2[RhCl6]3-(aq)+ 3Ni a 2Rh(s) + 3NiCl2(aq) + 6Cl-(aq) E˚ for RhCl6 is 0.5V E˚ for Ni(s) is -0.25V

35. chemistry 2

for the reaction 2C2H2(g)=>C6H6(l) at 25 C, the standard enthalpy change is -631 kJ and the standard entropy change is -430 J/K. calculate the standard free energy change at 25 C. show all work Help please!

36. Chemistry

C2H2(g) + 2 H2(g)--> C2H6(g) Substance So (J/mol∙K) ∆Hºf (kJ/mol) C2H2(g 200.9 226.7 H2(g) 130.7 0 C2H6(g) -- -84.7 Bond Bond Energy (kJ/mol) C-C 347 C=C 611 C-H 414 H-H 436 If the value of the standard entropy change, ∆Sº for the reaction is

37. Chemistry

C2H2(g) + 2 H2(g)--> C2H6(g) Substance So (J/mol∙K) ∆Hºf (kJ/mol) C2H2(g 200.9 226.7 H2(g) 130.7 0 C2H6(g) -- -84.7 Bond Bond Energy (kJ/mol) C-C 347 C=C 611 C-H 414 H-H 436 If the value of the standard entropy change, ∆Sº for the reaction is

38. Chemistry

C2H2(g) + 2 H2(g)--> C2H6(g) Information about the substances involved in the reaction represented above is summarized in the following tables. Substance/ So (J/mol∙K) /∆Hºf (kJ/mol) C2H2(g) / 200.9 / 226.7 H2(g) / 130.7 / 0 C2H6(g)/ ?? / -84.7 Bond

39. Chemistry

(a) Calculate the standard free-energy change (ΔG°) for the following oxidation-reduction reaction. Cu(s) + Br2(aq) → Cu2+(aq) + 2 Br−(aq) (b) Calculate the equilibrium constant for this reaction at 298 K.

40. Chemistry

The standard free energy of activation of a reaction A is 88.6 kJ mol–1 (21.2 kcal mol–1) at 298 K. Reaction B is one hundred million times faster than reaction A at the same temperature. The products of each reaction are 10.0 kJ mol–1 (2.39 kcal

41. Chemistry

Free-energy change, ΔG∘, is related to cell potential, E∘, by the equation ΔG∘=−nFE∘ where n is the number of moles of electrons transferred and F=96,500C/(mol e−) is the Faraday constant. When E∘ is measured in volts, ΔG∘ must be in

42. Chemistry

A reaction A+B---> C has a standard free energy change of -5.13 kj/mol at 25 degrees celcius, What are the concentrations of A, B, and C at equilibrium if at the beginning of the reaction there concentrations are .3M, .4M, and 0M respectively?

43. Chemistry

Given the following half-reactions and their standard reduction potentials, Ni2+ + 2e− Ni E° = -0.25 V 2H+ + 2e− H2 E° = 0.00 V Ag+ + e− Ag E° = 0.80 V a spontaneous reaction will occur between: a. Ni2+ and H2 b. H+ and Ag c. Ag+ and Ni d. Ni2+

44. physics

1. The equilibrium constant for a certain system is 50 at 25 celsius. Calculate the free energy change 2. When the fee energy change: a) =0, the position of the equilibrium, temperature * change in entropy, free energy change at standard states

45. Chemistry

A reaction has a standard free-energy change of –12.40 kJ mol–1 (–2.964 kcal mol–1). Calculate the equilibrium constant for the reaction at 25 °C.

46. Chemistry

A reaction has a standard free-energy change of –12.40 kJ mol–1 (–2.964 kcal mol–1). Calculate the equilibrium constant for the reaction at 25 °C.

47. Science

A reaction has a standard free-energy change of –11.70 kJ mol–1 (–2.796 kcal mol–1). Calculate the equilibrium constant for the reaction at 25 °C. Im so lost please help

48. Chem2

The Ksp for Ag2SO4 is 1.1x10^-5. Calculate the standard free energy change for silver sulfate dissolution at 25 degrees.

49. CHEM

1.) What is the correct net cell reaction for the electrochemical cell diagramed below? Ni(s) ∣ Ni2+(aq) || Ag+(aq) ∣ Ag(s) a.) Ag+(aq) + Ni(s) ---> Ag(s) + Ni2+(aq) b.) Ag(s) + Ni2+(aq) ---> Ag+(aq) + Ni(s) c.) 2Ag+(aq) + Ni(s) ---> 2 Ag(s) + Ni2+(aq)

50. Chemistry

A reaction: A(aq)+B(aq)C(aq) has a standard free-energy change of –4.69 kJ/mol at 25 °C. What are the concentrations of A, B, and C at equilibrium if, at the beginning of the reaction, their concentrations are 0.30 M, 0.40 M, and 0 M, respectively? I

51. CHEMISTRY - BATTERIES

What is the voltage and the Gibbs Free Energy for the following reaction? (Assume standard conditions) 3Sn^2+ (aq) + 2Al (s) --> 2 Al^3+ (aq) + 3 Sn (s) Now calculate the Gibbs Free Energy for the above reaction if Sn^2+ (aq) is 0.15 and Al^3+ (aq) is 1.8

52. chemistry

Co2(aq)->Co2(g) calculate the free-energy change for this reaction at 25 degrees Celsius.

53. Chemistry

The Haber process is used to synthesize ammonia (NH3) from N2 and H2. The change in standard Gibbs free energy is ΔG°rxn = -16 kJ/mol A. Calculate the equilibrium constant for this reaction B. Calculate the ΔGrxn when you have 2 atm of NH3 (g), 2 atm of

54. Chemistry

Question asking about how enzymes affect the rate of a reaction. Check all that apply 1. They shift the reaction equilibrium towards the products. 2. They increase the concentration of the reactants. 3. They lower the activation energy of the reaction. 4.

55. Chemistry

Under standard conditions, the Gibbs free energy of the reactants G,std(reactants) in a redox reaction in aqueous solution is 360.65 kJ and the Gibbs free energy of the products G,std(products) is 158.14 kJ. The number of moles, n, of electrons transferred

56. chemistry

Under standard conditions, the Gibbs free energy of the reactants G,std(reactants) in a reaction in the gas phase is 232.94 kJ and the Gibbs free energy of the products G,std(products) is 211.56 kJ. Calculate the value of the equilibrium constant for this

57. chemistry

(AAAAA)The standard reduction potentials of lithium metal and chlorine gas are as follows: (for Li, reduction potential is -3.04, for Cl it is 1.36) In a galvanic cell, the two half-reactions combine to 2Li{+](s) + Cl{-}2(g) --> 2Li{+}Cl{-}(aq) Calculate

58. Biochemistry

Consider the malate dehydrogenase reaction from the citric acid cycle. Given the following concentrations, calculate the free energy change for this reaction at 37.0 °C (310 K). ΔG°\' for the reaction is 29.7 kJ/mol. Assume that the reaction occurs at

59. Biochem

Consider the malate dehydrogenase reaction from the citric acid cycle. Given the following concentrations, calculate the free energy change for this reaction at 37.0 °C (310 K). ΔG°\' for the reaction is 29.7 kJ/mol. Assume that the reaction occurs at

60. Chemistry

A reaction: A(aq) + B(aq) C(aq) has a standard free-energy change of –4.65 kJ/mol at 25 °C. What are the concentrations of A, B, and C at equilibrium if, at the beginning of the reaction, their concentrations are 0.30 M, 0.40 M, and 0 M, respectively?

61. Chemistry

A reaction : A(aq)+B(aq) --> C(aq) has a standard free-energy change of –4.01 kJ/mol at 25 °C. What are the concentrations of A, B, and C at equilibrium if, at the beginning of the reaction, their concentrations are 0.30 M, 0.40 M, and 0 M,

62. Chemistry

A reaction A(aq)+B(aq)C(aq) has a standard free-energy change of –3.35 kJ/mol at 25 °C. What are the concentrations of A, B, and C at equilibrium if, at the beginning of the reaction, their concentrations are 0.30 M, 0.40 M, and 0 M, respectively?

63. Chemistry

A reaction has a standard free-energy change of –4.60 kJ/mol at 25 °C. What are the concentrations of A, B, and C at equilibrium if, at the beginning of the reaction, their concentrations are 0.30 M, 0.40 M, and 0 M, respectively?

64. chemistry

the standard state free energy of hydrolysis of acetyl phosphat is G= -42.3 kJ/mol. Calculate the free energy change for the acetyl phosphate hydrolysis in a solution of 2mM acetate, 2 mM phospate and 3 nM acetyl phospahte.

65. Biochemistry

the standard state free energy of hydrolysis of acetyl phosphat is G= -42.3 kJ/mol. Calculate the free energy change for the acetyl phosphate hydrolysis in a solution of 2mM acetate, 2 mM phospate and 3 nM acetyl phospahte.

66. Science

For the dissociation of acetic acid, CH3COOH CH3COO- + H+, the free energy change, ΔG° = 27.26 kJ/mol. What is the free energy change, ΔG°', in the biochemical standard state? Given R = 8.315 J/mol · K. T = 25°C.

67. Chemistry

The change in entropy for a reaction is 3.0 J/(mol·K) at 25°C. Calculate the change in free energy for the reaction when ΔH = –394 kJ/mol and determine whether it will occur spontaneously at this temperature. Is the answer -395 kJ/mol? and second

68. Chemistry

At 298K, 2PCl3(g)+O2(g)---> 2POCl3(l) Delta H= -620.2kJ for the reaction and the standard molar entropies are ,PCl3(g)= 311.8J/K,O2(g)= 205.1J/K and POCl3(l)=222.4J/K. Determine the standard free energy change at 298K.

69. Chemistry

For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 bar for all species. For the reaction C2H6(g)+H2(g)---->2CH4 the standard change in Gibbs free energy is ΔG° = -32.8 kJ/mol. What is ΔG for this reaction at 298 K when the

70. Chemistry

Calculate the cell potential for the following reaction as written at 25.00 °C, given that [Cr2 ] = 0.859 M and [Ni2 ] = 0.0190 M. Standard reduction potentials can be found here.

71. Chemistry

Calculate the cell potential for the following reaction as written at 25.00 °C, given that [Cr2 ] = 0.859 M and [Ni2 ] = 0.0190 M. Standard reduction potentials can be found here.

72. chemistry

My teacher went over it really fast and now I'm just really confused about how to do my homework =( Calculate the cell potential for the following reaction as written at 25C, given that [Cr2+] = 0.821 M and [Ni2+] = 0.0190 M. Cr(s) + Ni2+ (aq) Cr2+ (aq) +

73. Chemistry 152

For a certain reaction, the enthalpy change is -148.5 kJ, the entropy change is 256 J/K, and the free energy change is -250.1 kJ. At what temperature is the reaction occurring, in C? Choose one answer. a. 85 b. 102 c. 124 d. 158 e. 210

74. Chemistry

calculate the standard free-energy change for the synthesis of hydrazine from nitrogen and hydrogen. N2(g) + H2(g) right arrow N2H4(l)

75. Chemsitry

Consider the equilibrium A(g)=2B(g)+3C(g) at 25 degrees Celsius. When A is loaded into a cylinder at 10 atm and the system is allowed to come to equilibrium, the final pressure is found to be 12.13 atm. What is the standard gibbs free energy of reaction

76. Chemistry

Calculate the cell potential for the following reaction as written at 25.00 °C, given that [Zn2 ] = 0.842 M and [Ni2 ] = 0.0100 M. Standard reduction potentials can be found here. reaction: Zn(s)+Ni^2+(aq)--->Zn^2+(aq)+Ni(s) standard reduction Zn: -.76

77. chemistry

Calculate the free energy change of the following reaction (in kJ). 3A^2+ +2B------->3A + 2B^3+ Ecell= 1.66 -(5 mol)*(9.65*10^4)*1.66= -8.0095*10^5 Did I do it right? or is the number of electrons wrong?

78. chemistry

My professor never teach us this kind of question before. I don't know why she put this question as a homework since she doesn't teach us this yet. I need help with one question. I don't know where to start. So don't you mind if you can help me please.

79. chemistry

I have to find delta G from a problem. Not the standard free energy, from the change in engery. So this delta G does not have the degree sign above. The equation i used was deltaG=standard G+RTlnQ If deltaG was a positve number, what does that tell me. I

80. Chemistry

Give the enthalpy change and entropy change values shown below calculate the free energy change for this reaction at 25 degrees C using Gibbs free energy equation. How does this value compare to the free energy change using the standard free energy of

81. chemistry

C2H2(g) + 2 H2(g)--> C2H6(g) Substance So (J/mol∙K) ∆Hºf (kJ/mol) C2H2(g 200.9 226.7 H2(g) 130.7 0 C2H6(g) -- -84.7 Bond Bond Energy (kJ/mol) C-C 347 C=C 611 C-H 414 H-H 436 If the value of the standard entropy change, ∆Sº for the reaction is

82. biochemistry

when a reaction AB starts, there is three times as much product as reactant. When it reaches equilibrium, there is twice as much product as reactant. Show how to calculate the standard change in gibbs free energy for this reaction. I did it but I'm not

83. Chemistry

A reaction has a standard free-energy change of -11.80 kJ/mol (-2.820 kcal/mol). Calculate the equilibrium constant for the reaction at 25 degrees C. Please help!

84. Chemistry

C2H2(g) + 2 H2(g)--> C2H6(g) Information about the substances involved in the reaction represented above is summarized in the following tables. Substance/ So (J/mol∙K) /∆Hºf (kJ/mol) C2H2(g) / 200.9 / 226.7 H2(g) / 130.7 / 0 C2H6(g)/ ?? / -84.7 Bond

85. Inorganic chemistry

The standard free energy change for a chemical reaction is -18.3kJ/mole. What is the equilibrium constant for the reaction at 87 degrees Celsius? (R=8.314J/K*mol) Delta G = -Rtlnk -18,300/8.314/360 = -6.114

86. Chemistry

I am still not understanding how to calculate n in Ecell=Enaughtcell-(.0592/n)logQ. Example: Au/Au^3+ and Cu/Cu^2+ If I am correct it should look like this Au->Au^3+ + 3e- (Enaughtcell = 1.50V) and Cu->Cu^2+ + 2e- (Enaughtcell = 0.34V). The Cu/Cu2+ is the

87. Chemistry

delta G reaction = delta G products - delta G reactants. Hydrogen peroxide is used as a bleachin agent, a disinfectant and medicinally as a topical antibacterial agent. Hydrogen peroxide decomposes according to the reacton 2H^2O^2(l)-->2H^2O(l)+o^2(g) A.

88. Chemistry

Hydrogen peroxide is used as a bleachin agent, a disinfectant and medicinally as a topical antibacterial agent. Hydrogen peroxide decomposes according to the reacton 2H^2O^2(l)-->2H^2O(l)+o^2(g) A. Given the standard free energy of formation values shown

89. Chemistry

"Energy is released when 100 kg of steam at 150 degrees Celsius and standard pressure changes to water at 60 degrees Celsius. Calculate the total energy change". I used q=mct to find the energy required to change to 100 degrees Celsius. But now what??

90. chemistry

In the fifth reaction of Glycolosis, G3P dehydrogenase converts glyceraldehydes-3-phosphate into glycerate-1,3-bisphosphate. In order to make the reaction spontaneous at biological conditions it must be coupled to the reduction of NAD+. a) DG° for the

91. physics

The classify the as synthesis, decomposition, Single replacement. Double replacement. 2 Al +3NiBr2. 2AlBr3+3Ni

92. AP Chemisty

N2(g)+3F2 yields 2Nf3(g) Delta H(degree)298=-264KJ mol-1;Delta S(degree)298=-278J K-1 mol-1 The following questions relate to the synthesis reaction represented by the chemical equation above. a.)CAlculate the value of the standard free energy change,

93. ~Chem

Check my work please The solubility product of nickel (II) hydroxide at 25°C is 1.6 x 10-16. Calculate the molar solubility of nickel (II) hydroxide in 0.100 M sodium hydroxide. Ni(OH)2 Ni2+ + 2OH– I = Ni2+ is 0 & 2OH– is 0.1 Change = Ni2+ is X and

94. chem

standard free energy change of -11.70 kJ mol-1. Calculate equilibrium constant for 25 degrees C. I got 7.772..and it's wrong I did -11700J/ (-2.303 x 8.314 x 298)= 2.0505277 and then e^(2.0505277)= 7.77 I don't know what I did wrong

95. Chemistry

the standard free energy change for a chemical reaction is +13.3 kj/ mol. What is the equilibrium constant for the reaction at 125 degree C ? (R= 8.314 j/mol )

96. Chemistry

Hydrogen peroxide is used as a bleachin agent, a disinfectant and medicinally as a topical antibacterial agent. Hydrogen peroxide decomposes according to the reacton 2H^2O^2(l)-->2H^2O(l)+o^2(g) A. Given the standard free energy of formation values shown

97. Chem

Change in enthalpy problem. Consider the reaction represented below. Referring to the data in the table below, calculate the standard enthalpy change for the reaction at 25 degrees C. O3(g)+NO(g)-->O2(g)+NO2(g) Standard enthalpy of formation in kJ/mol:

98. Chemistry

Can someone explain in easier terms the spontaneous process, entropy, and free energy. The textbook is hard to understand. Just a simple explanation. Thanks. Appreciate it! Free energy is the amount of energy that can be released in a chemical reaction. If

99. chemistry

Calculate the cell potential for the following reaction as written at 53 °C, given that [Zn2 ] = 0.862 M and [Ni2 ] = 0.0110 M. Standard reduction and oxidation potentials can be found here. Zn(s) + Ni^2+(aq) --> Zn^2+(aq) + Ni(s)

100. Chemistry

The standard free energy of activation of one reaction is 94.3 kj/mol^-1 (22.54 kcal/mol^-1). The standard free energy of activation for another reaction is 76.4 kJ/mol^-1 (18.26 kcal/mol^-1). Assume temp of 298K and 1 M conc. By what factor is one faster