# For a particular reaction, ΔH° is 20.1 kJ/mol and ΔS° is 45.9 J/(mol·K). Assuming these values change very little with temperature, over what temperature range is the reaction spontaneous in the forward direction? The reaction is spontaneous for temperatures is

35,327 results
1. ## Honors Chemistry

"How many grams of NH3 can be produced from the reaction of 28 g of N2 and 25 g of H2? N2 + 3H2 ---> 2NH3 ==> 28 g N2 x (1 mol N2/14.0 g N2) x (2 mol NH3/1 mol N2) x ( 17.0 g NH3/ 1 mol NH3) = 68 g NH3 25 g H2 x ( 1mol H2/2.0 g H2) x (2 mol NH3/3 mol H2) x

2. ## Chemistry

For the reaction described by the chemical equation: 3C2H2(g) -> C6H6(l) .. Delta H rxn = -633.1 kJ/mol a) Calculate the value of Delta S rxn at 25.0 C... b) Calculate Delta G rxn... c) In which direction is the reaction, as written, spontaneous at 25 C

3. ## Chemistry

Predict whether the following reactions will be exothermic or endothermic A) N2(g)+ 3H2(g) --> 2NH3(g) B) S(g) +O2(g) ---> SO2(g) C) 2H2O(g) ---->2H2(g) + O2(g) D) 2F(g) +F2(g) Bond H-H 432 kj/mol N-N(triple bond) 942 kj/mol O=O 494 KJ/Mol F-F 155 KJ/mol

4. ## ap chem

calculate the lattice enthalpy of potassium fluoride from the following data: enthalpy of formation of K(g): +89 kJ · mol−1 first ionization energy of K(g): +418 kJ · mol−1 enthalpy of formation of F(g): +79 kJ · mol−1 electron affinity of F(g):

5. ## Chemistry

Which of the following reactions are spontaneous (favorable)? A] 2Mg(s) + O2(g) -> 2MgO(s) Delta G = -1137 kJ/mol .. B] NH3(g) + HCl(g) -> NH4Cl(s) Delta G = -91.1 kJ/mol ... C] AgCl(s) -> Ag+(aq) + Cl-(aq) Delta G = 55.6 kJ/mol .. D] 2H2(g) + O2(g) ->

6. ## chem

Calculate the standard enthalpy change for the reaction 2A+B->2C+D Use the following data: Substance A=-257kj/mol B=-413kj/mol C=189kj/mol D=-475kj/mol For the reaction given , how much heat is absorbed when 3.00mol of A react?

7. ## chemistry

Tetraphosphorus trisulphide (P4S3) is used in the match heads of some matches. It is produced in the reaction 8P4+3S8 --> 8P4S3. Determine which of the following statements are incorrect, and rewrite the incorrect statements to make them correct. a. 4 mol

8. ## AP Chemistry

DrBob222 PLEASE HELP Hf of CO2 = -393.5 kJ/mol Hf of H2O = -285.8 kJ/mol The combustion reaction for benzoic acid C6H5CO2H(s) + 15/2 O2(g) → 7 CO2(g) + 3 H2O(ℓ) has ∆H0 = −3226.7 kJ/mole. Use Hess’s Law to calculate ∆H0f for benzoic acid. 1.

9. ## Chemistry

According to the reaction 2Al+3H2SO4→3H2+Al2(SO4)3, the total number of moles of H2SO4 needed to react completely with 5.0 mol of AL is 1. 2.5 mol 2. 5.0 mol 3. 7.5 mol 4. 9.0 mol

10. ## chemistry

If 15.0 grams of C3H6, 10.0 grams of oxygen, and 5.00 grams of NH3 are reacted, what mass of acrylonitrile can be produced assuming 100% yield, what mass of the excess reactants remain? 15g C3H6 (1 mol / 42.08 g) = .35 mol C3H6 .36 mol C3H6 ( 2 mol C3H3N /

11. ## Chemistry

For a particular reaction, ΔH° is 20.1 kJ/mol and ΔS° is 45.9 J/(mol·K). Assuming these values change very little with temperature, over what temperature range is the reaction spontaneous in the forward direction? The reaction is spontaneous for

12. ## chemistry:)

The bond enthalpy of the Br–Cl bond is equal to DH° for the reaction BrCl(g)-> Br(g) + Cl(g). Use the following data to find the bond enthalpy of the Br–Cl bond. Br2(l)--->Br2(g) ÄH=30.91 KJ/mol Br2(g)--->2Br2(g) ÄH=192.9 KJ/mol Cl2(g)---->2Cl(g)

13. ## Chemistry( HELP PLEASE, IM DESPERATE!!!)

For the reaction 2CH3OH + 3O2 → 2CO2+ 4H2O, what is the maximum amount of CO2 which could be formed from 13.97 g of CH3OH and 5.45 g of O2? Consider the reaction H3PO4 + 3NaOH → Na3PO4 + 3H2O. How much Na3PO4 can be prepared by the reaction of 3.43 g

14. ## chemistry

If 3 moles of a compound use 12 J of energy in a reaction, what is the Hreaction in kJ/mol? A. -4 kJ/mol B. -0.004 kJ/mol C. 0.004 kJ/mol D. 4 kJ/mol

15. ## CHEMISTRY PLEASE!!! ( I NEED HELP ASAP)

Consider the reaction H3PO4 + 3NaOH → Na3PO4 + 3H2O. How much Na3PO4 can be prepared by the reaction of 3.43 g of H3PO4 with an excess of NaOH? For the reaction ?Fe+?H2O → ?Fe3O4 +?H2, what is the maximum amount of Fe3O4(231.533 g/mol) which could be

16. ## Chemistry

For a particular reaction at 195.1 °C, ΔG = -1488.09 kJ/mol, and ΔS = 288.67 J/(mol·K).? Calculate ΔG for this reaction at -20.0 °C. delta G = delta H - (T*delta S) -1488.09 kJ/mol = (delta H) - ((461.8K)*(+288.67 J/(mol x K))*(1 kJ/1000 J)) -1488.09

17. ## Chemistry

Acetylene, C2H2, can be converted to ethane, C2H6, by a process known as hydrogenation. The reaction is: C2H2(g) + 2H2(g) === C2H6(g) Given the following, what is the Kp for the reaction? C2H2(g): 209.2 ΔG˚f (kJ/mol) H2(g): 0 ΔG˚f (kJ/mol) C2H6(g):

18. ## Chemistry

NH4Cl(s) → NH3(g) + HCl(g) ΔH°=176 kJ/mol At 25 °C, this reaction has a ΔG° of 91.1 kJ/mol. What is the ΔS° of this reaction? I came up with the solution of 0.896 kJ/mol. Is this correct?

19. ## Chemistry

The reaction of gaseous H2 and liquid Br2 to give gaseous HBr has ΔH = -17.4 kcal/mol (-72.8 kJ/mol) and ΔS = 27.2 (cal/mol⋅K) (114 J/(mol⋅K)). What is the value of ΔG (in kcal and kJ) for the reaction at 297 K ?

20. ## chemistry

When 3.2 g of ammonium chloride is dissolved in 75 g of water, the temperature of the solution decreases from 22.8°C to 20.1°C. What is the energy of dissolution of NH4Cl per mole? (The molecular mass of NH4Cl = 53.49 g/mol, and the specific heat of

21. ## chem 12

consider the following equilibrium 2NOCl(g)--- 2 NO(g) + Cl2(g) Initally 1.00 mol of NO and 1.00 mol of Cl2 are placed in a 5.00L container. Calculate the initial concentrations of NOCl, NO and Cl2 NO= 0.20 mol/L Cl2= 0.20 mol/l NOCl=0 At equilibrium it is

22. ## Chemistry

For a one step reaction, the activation energy for the forward reaction is 40.0 kJ mol-1, and the enthalpy of reaction is -20.0 kJ mol-1. Calculate the activation energy for the reverse reaction. Is my answer correct? (40 kJ mol-1)-(-20 kJ mol-1) = 20kJ

23. ## Chemistry

given the balanced equation representing a reaction: 4NH3+5O2-->4NO+6H2O what is the minimum number of moles of O2 that are needed to completely react with 16 moles of NH3? (1)16 mol (2)20.mol (3)64 mol (4)80. mol i think its 2 but im not sure.

24. ## Chemistry

If ammonia is manufactured at 356 K, is the reaction spontaneous, given that the enthalpy and entropy change for the reaction are -93 kJ/mol and -198 J/mol K, respectively? A. Yes, the ΔG is -92 kJ/mol. B. No, the ΔG is 92 kJ/mol. C. No, the ΔG is 22.5

25. ## Chemistry

Use a Born Haber cycle to calculate the lattice energy (in kJ/mol) of Potassium Chloride (KCl) from the following data: Ionization Energy of K(g) = 431kJ/mol Electron affinity of Cl(g) = -346kJ/mol Energy to sublime K(s) = 85kJ/mol Bond energy of Cl2(g) =

26. ## Chemistry - Science (Dr. Bob222)

Hydrazine is used as a rocket fuel because its reaction with oxygen is extremely exothermic: N2H4(liquid) + O2(g)  N2(g) + 2H2O(liquid) ΔH(reaction) = -615 kJ mol-1 What is the enthalpy of this reaction if water were produced in the gaseous rather than

27. ## Chemistry

1. The delta Hf of an element in its standard state is defined to be a) 0 kJ/mol b) 10 kJ/mol c) -10 kJ/mol d) greater than 0 kJ/mol e) a unique value for each element I am assuming its a? 2. Which of the following statements are true? I) The reaction

28. ## ap chemistry

The energy change H associated with the reaction NBr3(g) + 3H2O(g) ! 3HOBr(g) + NH3(g)is +81 kJ/mol rxn. These bond energy values might be useful:O-H 459 kJ/mol; N-H 386 kJ/mol;O-Br 201kJ/mol. The strength of the N Br bond is

29. ## Chemistry

Consider the reaction below. 2C6H14 + 19O2 mc032-1.jpg 12CO2 + 14H2O How many moles of hexane (C6H14) must burn to form 18.4 mol of carbon dioxide? 1.53 mol 3.07 mol 110. mol 175. mol

30. ## AP Chemistry

Carbon monoxide reacts with oxygen to form carbon dioxide by the following reaction: 2CO(g) + O2(g) --> 2CO2(g) change in H for this reaction is −135.28 kcal. If 811.7 kcal is released, how many moles of CO must have reacted? 1. 16.3 mol 2. 40.5 mol 3.

31. ## chemistry

The equilibrium constant (Kc) for the gas phase reaction 2 NH3 N2 + 3 H2 is 3.0 x 10-3 at some temperature. The reaction is started by placing a 0.040-mol sample of ammonia in an empty one-liter flask. When equilibrium is established how much N2 is

32. ## chemistry

Consider the following reaction at 298 K: C(graphite) +2Cl2 (g) -----> CCl4(l) Calculate the following quantities. Delta H: -139 kJ/mol deltaS(sys)=? J/mol*K deltaS(surr)=? J/mol*K deltaS(univ)=? J/mol*K My answer is: deltaS(sys)=654.9J/mol*K

33. ## Chemistry

The standard free energy of a reaction At 25 oC, ∆G°= 553 J/mol for the reaction A ⟶ B+C. Determine the concentration of the substance “B” at equilibrium if only a quarter of reactant remains at equilibrium. Group of answer choices 0.087 mol 0.349

34. ## chemistry

The standard molar entropy value of N2 (g) is 191.5 J/K-mol, of O2 (g) is 205.0 J/K-mol and of NO2 (g) is 240.0 J/K-mol. From these values we can calculate the Delta S for the reaction N2 (g) + 2 O2 (g) produces 2 NO2 (g) to be a. – 156.5 J/K b. 636.5

35. ## chemistry

Which of the following mixtures will be a buffer when dissolved in a liter of water? a. 0.1 mol Ca(OH)2 and 0.3 mol HI b. 0.3 mol NaCl and 0.3 mol HCl c. 0.4 mol NH3 and 0.4 mol HCl d. 0.2 mol HBr and 0.1 mol NaOH e. 0.2 mol H3PO4 and 0.1 mol NaOH i think

36. ## Chemistry

Delta H is 20.1 kJ/mol and Delta S is 45.9 J/(mol-k). Assuming these values change very little with temperature, over what temperature range is the reaction spontaneous in the forward direction? Is the reaction spontaneous for temperatures less than or

37. ## CHEM:

The bond enthalpy of the Br−Cl bond is equal to ƒ¢H‹ for the reaction BrCl(g) ¨ Br(g) + Cl(g). Use the following data to find the bond enthalpy of the Br−Cl bond. Br2(l)--->Br2(g) ƒ¢H=30.91 KJ/mol Br2(g)--->2Br2(g) ƒ¢H=192.9 KJ/mol

38. ## chemistry

Nitroglycerin is a powerful explosive, giving four different gases when detonated.2 C3H5(NO3)3 (l) → 3 N2 (g) + 1/2 O2 (g) + 6 CO2 (g) + 5 H2O (g)Given that the enthalpy of formation of nitroglycerin, ΔHf°, is −364 kJ/mol, calculate the energy (heat

39. ## chemistry

Given a percent yield of 45.0% for the reaction: H2 + Cl2 → 2 HCl(g) How many moles of HCl gas are produced if 15.5 L of Cl2 at STP and excess H2 are reacted? 1. 0.769 mol 2. 0.346 mol 3. 0.622 mol 4. 3.08 mol 5. 1.38 mol 6. 0.156 mol

40. ## Chemistry

Calculate the molar enthalpy of reaction per mole of carbon in the following reaction: 3 C(s) + 2 Fe2O3(s) + 466 kJ c12-u3_files/i0210000.jpg 4 Fe(s) + 3 CO2(g) a. +466 kJ/mol C b. +155 kJ/mol C c. +117 kJ/mol C d. –466 kJ/mol C e. –155 kJ/mol C

41. ## chemistry

The fermentation of sugar (C6H12O6) to form ethanol (C2H5OH) and carbon dioxide (CO2) occurs according to the following equation: C6H12O6(aq) ¡ú 2 C2H5OH(aq) + 2 CO2(g) kJ mol¨C1 ¦¤Hf (C6H12O6(s)) is ¨C1275 ¦¤Hf (C2H5OH(l)) is ¨C277 ¦¤Hbond

42. ## chemistry:)

The bond enthalpy of the Br–Cl bond is equal to DH° for the reaction BrCl(g)-> Br(g) + Cl(g). Use the following data to find the bond enthalpy of the Br–Cl bond. Br2(l)--->Br2(g) ÄH=30.91 KJ/mol Br2(g)--->2Br2(g) ÄH=192.9 KJ/mol Cl2(g)---->2Cl(g)

43. ## chemistry

Given the standard heats of reaction Reaction ∆H0 M(s) + 2 X2(g) → MX4(g) −123.7 kJ/mol X2(g) → 2 X(g) +297.3 kJ/mol M(g) → M(s) −25.1 kJ/mol calculate the average bond energy for a single M X bond. Answer in units of kJ/mol

44. ## Chemistry

Given the standard heats of reaction Reaction ∆H0 M(s) + 2 X2(g) → MX4(g) −123.7 kJ/mol X2(g) → 2 X(g) +297.3 kJ/mol M(g) → M(s) −25.1 kJ/mol calculate the average bond energy for a single M X bond. Answer in units of kJ/mol

45. ## chemistry

Nitric oxide reacts with bromine gas at elevated temperatures according to the equation, 2 NO(g) + Br2(g) = 2 NOBr(g) The experimental rate law is rate = k[NO][Br2]. In a certain reaction mixture the rate of formation of NOBr(g) was found to be 4.50 x 10-4

46. ## ap chem

Analysis of a reaction mixture showed that it had the composition 0.417 mol/L N2, 0.539 mol/L H2, and 0.127 mol/L NH3 at 800 K, at which temperature Kc = 0.278 for N2(g) + 3H2(g) *) 2NH3(g) . Calculate the reaction quotient Qc .

47. ## Chemistry

Combustion of natural gas (primarily methane) occurs in most household heaters. The heat given off in this reaction is used to raise the temperature of the air in the house. Assuming that all the energy given off in the reaction goes to heating up only the

48. ## ap chemistry

Carbon monoxide reacts with oxygen to form carbon dioxide by the following reaction: 2CO2 + O2 yields 2CO2 Delta H for this reaction is -566 kJ/mol run. What is the delta H for CO? 1). +270 kJ/mol 2). -110 kJ/mol 3). +65 kJ/mol 4). -405 kJ/mol 5). -65

49. ## chemistry

In a reaction vessel, the following reaction was carried out using 0.250 mol of NH3 and 0.100 mol of N2, 4NH3(l) + N2 (g) = 3N2H4 (l) what is the compositon in moles in the vessel when the reaction is completed? Is the answer: 0 mol NH3, 0.063 mol N2, and

50. ## Chemistry

Given the following information determine the reaction Gibbs energy for the formation of silicon dioxide at 298 K Si(s)+O2(g) →SiO2(s) ΔfH°(Si(s))=0 kJ mol-1, S°(Si(s))=18.8 J mol-1 K-1 ΔfH°(O2(g))=0 kJ mol-1, S°(O2(g))=205.0 J mol-1 K-1

51. ## Science

Which conversion factor should be used to solve the following problem? How many moles of water (H2O) would be produced from the reaction of 3.25 moles of hydrochloric acid (HCl) reacting with excess calcium hydroxide Ca(OH)2? Ca(OH)2 +2HCl --> CaCl2 + 2H2O

52. ## chemistry

The reversible reaction n2(g) + 3h2(g) produces ammonia, which is a fertilizer. At quilibrium, a 1-L flask contains 0.15 mol H2, 0.25 mol N2, and 0.10 mol NH3. Calculate K eq for a reverse reaction? Please HELPP!

53. ## Chemistry

The decomposition of ethane, C2H6, is a first-order reaction. It is found that it takes 212 seconds to decompose 0.00839 M C2H6 to 0.00768 M. What is the rate of decomposition (in mol/L-h) when [C2H6] = 0.00422 M? A. 6.43 x 10^-3 mol/L-h B. 6.34 x 10^-5

54. ## chemistry

Find the temperature at which the reaction below is spontaneous given this data: Hf^o of NH3(g) = - 46 kJ/mol, S^o of NH3(g) = 192.5 J/mol·K, S^o of N2(g) = 191.5 J/mol·K, S^o of H2(g) = 130.6 J/mol·K. N2(g) + 3H2(g) 2NH3(g)

55. ## Thermodynamics

Given the standard heats of reaction M(s) + 2 X2(g) → MX4(g) −113.7 kJ/mol X2(g) → 2 X(g) +317.3 kJ/mol M(g) → M(s) −23.1 kJ/mol calculate the average bond energy for a single M-X bond. Answer in units of kJ/mol. i have an idea of how but im not

56. ## AP Chem

The energy change H associated with the reaction NBr3(g) + 3H2O(g) -> 3HOBr(g) + NH3(g) is +81 kJ/mol rxn. These bond energy values might be useful: O-H 459 kJ/mol; N-H 386 kJ/mol; O-Br 201 kJ/mol. The strength of the N Br bond is 1. 4 kJ/mol 2. 465

57. ## ap chemistry

Carbon monoxide reacts with oxygen to form carbon dioxide by the following reaction: 2CO + O2 yields 2CO2 Delta H for this reaction is -135.28 kcal. If 811.7 kcal is released, how many moles of CO must have reacted? 1). 270.5 mol 2). 40.5 mol 3). 12.0 mol

58. ## Chemistry

Wood alcohol i.e. methanol CH3OH(l) might be a cheap source of methane CH4(g) (which is natural gas) where 1 mol of liquid methanol decomposes into 1 mol of methane gas and 1/2 mol of oxygen O2 (g). Write out the reaction (as described) and using the data

59. ## Chemistry- Dr.Bob!

Combustion of natural gas (primarily methane) occurs in most household heaters. The heat given off in this reaction is used to raise the temperature of the air in the house. Assuming that all the energy given off in the reaction goes to heating up only the

60. ## chemistry

Three solutions are mixed together to form a single solution. One contains 0.2 mol \rm mol Pb(CH 3 COO) 2 \rm Pb(CH_3COO)_2, the second contains 0.1 mol \rm mol Na 2 S \rm Na_2S, and the third contains 0.1 mol \rm mol CaCl 2 \rm CaCl_2. Write the

61. ## Chemistry

If at a certain instant during the course of the reaction 2 NO2(g) + F2(g) ¨ 2 NO2F(g), the rate of formation of the product were 0.16 mol/L∙s, how fast would the F2 be disappearing (also in mol/L∙s) at that same instant in time? A) 0.16 mol/L∙s

62. ## Chemistry

Two reactions that occur in the production of iron (Fe) are 2 C + O2 → 2 CO followed by Fe2O3 + 3 CO → 2 Fe + 3 CO2 . Note that the carbon monoxide (CO) formed in the first reaction is then used in the second reaction. According to these equations, how

63. ## Chemistry

Initially, 1.68 mol of PCl5(g) and 0.36 mol of PCl3(g) are in mixed in a 2.00 l container. It is later found that 1.44 mol of PCl5 are present when the system has reached equillibrium. Calculate the value of the equllibrium. This is what I did: Equation:

64. ## Chemistry

Consider the reaction: CO(g) + H2O (g) CO2(g)+H2(g) which of the following initial composition will NOT achieve equlibrium? a) 0.25 mol H2, 0.35 mol CO2, and 0.25 mol CO b) 0.25 mol CO, 0.75 mol H2O c) 1.0 mol of CO2 and 0.50 mol H2 d) 0.85 mol CO and 0.25

65. ## Chemistry Need help ASAP

A proposed mechanism for a reaction is: (i) A + B2 = AB2 Ea1 = 12 kJ/mol ƒ´H1 = 3 kJ/mol (ii) AB2 + C2 = ABC + BC Ea2 = 30 kJ/mol ƒ´H2 = 5.2 kJ/mol (iii) ABC + B2 = AB2 + BC Ea3 = 10 kJ/mol ƒ´H3 = -7.8 kJ/mol a) Which is the rate determining step?

66. ## Chem

Calculate ΔG at 25°C for the precipitation of lead(II) chloride from mixing 100. mL of 0.025 M lead(II) nitrate solution with 100. mL of 0.15 M sodium chloride solution. The ΔG° for the reaction at 25°C = −27.36 kJ/mol. (Hint: write out reaction

67. ## Science

Which conversion factor should be used to solve the following problem? How many moles of water (H2O) would be produced from the reaction of 3.25 moles of hydrochloric acid (HCl) reacting with excess calcium hydroxide Ca(OH)2? Ca(OH)2 +2HCl --> CaCl2 + 2H2O

68. ## Chemistry

Chemistry HELP - Rates of reaction, redox reactions? 10 points? An structural isomer of bromobutane (C4H9Br) can be hydrolysed using aqueous sodium hydroxide to produce butanol. This can be represented by the following equation: C4H9Br(l) + OH-(aq) >

69. ## chemistry

What mass of sodium hydroxide pellets must be poured into a waste drum containing 20.0 L o 3.0 mol/L sulphuric acid to completely neutralize the waste acid solution? Write a balanced chemical equation for this reaction. okay, so here is the work I already

70. ## CHEMISTRY!! NEED IMMEDIATE HELP PLEASE!!!

a. Calculate the delta H, delta G, and equilibrium constant for the reaction of methane with Cl2 to give CH3Cl and HCl. Use the following information for your calculations: Bond Dissociation Energies: CH3-H (104.8kcal/mol), Cl-Cl(59.0 kcal/mol),

71. ## chemistry

Find the temperature at which the reaction below is spontaneous given this data: Hfo of NH3(g) = - 46 kJ/mol, So of NH3(g) = 192.5 J/mol·K, So of N2(g) = 191.5 J/mol·K, So of H2(g) = 130.6 J/mol·K. N2(g) + 3H2(g) ßà 2NH3(g)

72. ## chemistry

When 0.100 L of 1.00 mol L−1 HCl(aq) is mixed with 0.100 L of 1.00 mol L−1 NaOH, the temperature of the solution rises by 8.5 oC. Assuming no heat loss to the container or the surroundings, what is the heat of reaction for the following reaction? (You

73. ## College Chemistry

In a reaction vessel, the following reaction was carried out using 0.250 mol of NH3(l) and 0.100 mol of N2(g). 4NH3(l) + N2(g) ¡ú 3N2H4(l) Which of the following represents the composition in moles in the vessel when the reaction reaches completion?

74. ## chemistry

A proposed mechanism for a reaction is: (i) A + B2 = AB2 Ea1 = 12 kJ/mol ƒ´H1 = 3 kJ/mol (ii) AB2 + C2 = ABC + BC Ea2 = 30 kJ/mol ƒ´H2 = 5.2 kJ/mol (iii) ABC + B2 = AB2 + BC Ea3 = 10 kJ/mol ƒ´H3 = -7.8 kJ/mol a) Which is the rate determining step?

75. ## Chemistry Need help ASAP

A proposed mechanism for a reaction is: (i) A + B2 = AB2 Ea1 = 12 kJ/mol ƒ´H1 = 3 kJ/mol (ii) AB2 + C2 = ABC + BC Ea2 = 30 kJ/mol ƒ´H2 = 5.2 kJ/mol (iii) ABC + B2 = AB2 + BC Ea3 = 10 kJ/mol ƒ´H3 = -7.8 kJ/mol a) Which is the rate determining step?

76. ## Chemistry

A proposed mechanism for a reaction is: (i) A + B2 = AB2 Ea1 = 12 kJ/mol ƒ´H1 = 3 kJ/mol (ii) AB2 + C2 = ABC + BC Ea2 = 30 kJ/mol ƒ´H2 = 5.2 kJ/mol (iii) ABC + B2 = AB2 + BC Ea3 = 10 kJ/mol ƒ´H3 = -7.8 kJ/mol a) Which is the rate determining step?

77. ## chemistry

The standard free energy of activation of a reaction A is 78.2 kJ mol–1 (18.7 kcal mol–1) at 298 K. Reaction B is ten 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)

78. ## chemistry

I have two questions that I really don't understand. The first one is: A reaction proceeds with delta H=-10kJ/mol. The energy of activation of the uncatalyzed reaction is 150kJ/mol, whereas it is 100kJ/mol for the uncatalyzed reaction. How many times

79. ## AP Chemistry

The equilibrium constant for thermal dissociation of F2 F2(g)2F(g) is 0.300. If initially 1.00 mol F2 is placed in a 1.00 L container, which of the following is the correct number of moles of F2 that have dissociated at equilibrium? 1. 0.130 mol 2. 0.418

80. ## Chemistry

K=1.6x10^-5 mol/L for the following reaction 2NOCl(g).... 2 NO(g) + Cl2(g) Calculate the concentrations of all species at equilibrium for each of the following original mixtures E) 2.4 mol of NOCl, 2.4 mol of NO, and 1.2 mol Cl2 in a 1.0 L flask F)1.9

81. ## chemistry

Consider the balanced equation 2A(g) + 3G(g) „\ 2X(g) + Z(g). To a 20.0 L container maintained at a temperature of 127 C were added 0.200 mol of A, 0.500 mol of G, 0.400 mol of X, and 0.600 mol of Z. After equilibrium was established, it was found that

82. ## Chemistry

Rates of reaction, redox reactions? 10 points? An structural isomer of bromobutane (C4H9Br) can be hydrolysed using aqueous sodium hydroxide to produce butanol. This can be represented by the following equation: C4H9Br(l) + OH-(aq) > C4H9OH(l) + Br-(aq)

83. ## chemistry

The power of the equation ΔG° = –RT ln(K) is that K can be determined from tabulated values of ΔG°f. Use the tabulated values of the Gibb's energy to determine K for the reaction, 2AB(l) ↔ 2A(g) + B2(g), at 298K. (R=8.314 J/K mol or R=0.008314 kJ/K

84. ## CHEM

Which of the following mixtures will result in the formation of a buffer solution when dissolved in 1.00 L of water? i) 0.50 mol NaOH and 0.50 mol HCl. ii) 0.50 mol NaCl and 0.25 mol HCl. iii) 0.50 mol NaF and 0.25 mol HF. iv) 0.50 mol NaOH and 0.25 mol

85. ## College Chemistry

The molar heat of reaction, H rxn, for the reaction of Ca(s) + 2H+(aq) Ca2+(aq) + H2(g) is -544.789 kJ/mol and Hrxn, for the reaction of CaO(s) + 2H+(aq) Ca2+(aq) + H2O(l) is -192.42 kJ/mol, the heat of formation of water is -286 kJ/mol, The H ffor CaO(s)

86. ## AP Chemistry

Analysis of a reaction mixture showed that it had the composition 0.43 mol/L N2, 0.541 mol/L H2, and 0.124 mol/L NH3 at 800 K, at which temperature Kc=0.278 for N2(g) + 3H2(g)2NH3(g). Calculate the reaction quotient Qc

87. ## Chem Question (thermo)

Calculate ΔG at 25 ºC for a reaction in which Ca2+(aq) combines with CO32–(aq) to form a precipitate of CaCO3(s) if the concentrations of Ca2+(aq) and CO32–(aq) are 0.023 M and 0.13 M, respectively. (ΔGº = –47.94 kJ) A. –62.3 kJ/mol B. –33.5

88. ## Chemistry

At 25 ∘ C 25∘C, 0.11 mol 0.11 mol of N 2 O 4 N2O4 reacts to form 0.10 mol 0.10 mol of N 2 O 4 N2O4 and 0.02 mol 0.02 mol of N O 2 NO2. At 90 ∘ C 90∘C, 0.11 mol 0.11 mol of N 2 O 4 N2O4 forms 0.050 mol 0.050 mol of N 2 O 4 N2O4 and 0.12 mol 0.12 mol

89. ## chemistry

Consider the reaction: N2(g) + 3 H2(g) --> 2 NH3(g). At a particular time, the nitrogen is being consumed at a rate of 0.60 moles/sec. At this same time, what is the rate at which ammonia is being formed? a. 3.0 mol/s b. 0.12 mol/s c. 0.30 mol/s d. 2.0

90. ## CHEMISTRY> HELP QUICK! pls

Calculate the reaction free energy of: H2(g) + I2(g) 2HI(g) when the concentrations are 0.026 mol L-1 (H2), 0.33 mol L-1 (I2), and 1.84 mol L-1 (HI), and the temperature is 700K. For this reaction Kc= 54 at 700 K. +11.6 kJ mol-1 0 kJ mol-1 -11.6 kJ mol-1

91. ## chem

Which rate constant would result in the fastest reaction? A. 1.3 × 10^3 L/mol · s B. 2.8 L/mol · s C. 9.5 × 10^-2 L/mol · s D. 4.2 × 10^-3 L/mol · s i think that it is answer c as it has the highest values plus a negative exponent

92. ## chemistry

A + B -> C + D (reversible reaction) a 2L container contains 1 mol of C, 1.6 mol of D, 0.8 mol of A snd 0.8 mol of B. Calculate the equillibrium composition of the reaction. Kc =0.065 I think C and D are forming A and B because there is higher

93. ## chemistry

A + B -> C + D (reversible reaction) a 2L container contains 1 mol of C, 1.6 mol of D, 0.8 mol of A snd 0.8 mol of B. Calculate the equillibrium composition of the reaction. Kc =0.065 I think C and D are forming A and B because there is higher

94. ## Chemistry

How much water would be formed if 3.00 mol NH3 reacted with excess oxygen gas in the following equation? Given the reaction 4NH3+ 5O2 --> 4NO + 6H2O A) 2.00 mol B) 3.00 mol C) 4.50 mol D) 6.00 mol E) None of these

95. ## chemistry

A proposed mechanism for a reaction is: (i) A + B2 AB2 Ea1 = 12 kJ/mol ƒ´H1 = 3 kJ/mol (ii) AB2 + C2 ABC + BC Ea2 = 30 kJ/mol ƒ´H2 = 5.2 kJ/mol (iii) ABC + B2 AB2 + BC Ea3 = 10 kJ/mol ƒ´H3 = -7.8 kJ/mol a) Which is the rate determining step? Explain

96. ## Chemistry

The reaction of 1 Mol of iron metal with 3 Mol aqueous HCI produces 1.5 mol H2 gas, 1 mol aqueous FeCI3, and 87.9 kj of heat. Write a thermochemical equation for this reaction

97. ## Enthalpy Change Calculations

Find the heat of reaction (ΔH) for each of the following chemical reactions and note whether each reaction is exothermic or endothermic. 1. H2O(l) -> H2O(g) This is what I have so far: H2(g) + ½ O2(g) -> H2O(l) ΔH = -286.0 kJ/mol H2(g) + ½ O2(g) ->

98. ## science

Which rate constant would result in the fastest reaction? A. 1.3 × 103 L/mol · s B. 2.8 L/mol · s C. 9.5 × 10-2 L/mol · s D. 4.2 × 10-3 L/mol · s is the answer for this one c?

99. ## Chemistry Need Help!

Okay, the reaction is this: Naphthalene + HNO3 ---> NitroNapthalene The limiting reagent is Naphthalene The excess is the nitric acid The equation is 1:1 balanced as far as I know 3 g of Nap used in the experiment x 1mol/128.17 g/mol = .023 mol Nap 12.69 g

100. ## Chemistry

So I have had several homework problem like this and managed to solve them easily, but these two problems I cannot get the correct answer for. Using a Table of thermodynamic data, calculate the change in Gibbs free energy for each of the following