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+ +

53,203 results
  1. AP Chemistry

    Calculate the delta H rxn for the following reaction: CH4(g)+4Cl2(g)-->CCl4(g)+4HCl Use the following reactions and given delta H's: 1) C(s)+2H2(g)-->CH4(g) delta H= -74.6 kJ 2) C(s)+2Cl2(g)-->CCl4(g) delta H= -95.7 kJ 3) H2(g)+Cl2(g)-->2HCl(g) delta H=

  2. 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) ->

  3. 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

  4. 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 =

  5. Chemistry

    Calculate the enthalpy change for the reaction: 2S(s) + 3O2(g) --> 2SO3(g) Use the following thermochemical equations: Reaction S(s) + O2(g) --> SO2(g) Delta H(in kJ) -296.8 2SO2(g) + O2(g) --> 2SO3(g) Delta H(in kJ) -197.0

  6. AP Chem

    Reaction 1: NaOH + HCL --> H20 + NaCl delta H of -100.332 kj/mol Reaction 2: NaOH + NH4Cl --> NH3 + H20 : delta H of 358.639 kj/mol Reaction 3: HCl + NH3 --> NH4Cl : delta H of -51.701 kj/mol Use your answers from question 2 above and Hess's law to

  7. Chemistry

    for the reaction of hydrogen with iodine H2(g) + I2(g) --> 2HI(g) relate the rate of disappearance of hydrogen gas to the rate of formation of hydrogen iodide. and my answer is: rate formation of HI= delta [HI]/delta t and the rate of reaction of I2 =

  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

    Given the thermodynamic data in the table below, calculate the equilibrium constant for the reaction: 2SO2(g)+O2--> 2SO3 Substance (DeltaH^o) (Delat S^o) SO2 -297 249 O2 0 205 SO3 -395 256 Answer (it was given) 2.32x10^24 Even though the answer is given

  10. thermodynamics

    A reaction has deltaHrxn=-127 kJ and delta S rxn=314 J/K. At what temperature is the change in entropy for the reaction equal to the change in entropy for the surroundings? so I made delta H-T delta S=0 plugged in values for S and H and solved for T. I got

  11. Chemistry

    delta T = ikfm delta T is the amount f.p. is lowered. i is the number of particles; i.e., Na3PO4 will have i = 4 (3 for Na and 1 for PO4). m is molality. k is a constant and need not enter into the calculations. Arrange the following solutions in order of

  12. 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

  13. Chemistry

    Calculate the delta H and delta S for the reaction. From there, calculate the delta G at 25 degrees Celsius. Predict whether it the reaction is spontaneous or non-spontaneous under standard conditions. CH3OH(l)+ O2(g)--> HCO2H(l)+ H2O(l) *i could not find

  14. Chemistry

    Enthalpy changes: H2O2(l) ----> H2O(l) + 1/2P2(g) delta H= -94.6kJ H2(g) + 1/2O2(g)----> H2O2 delta H= -286.0kJ Calculate the value on delta H for the reaction: H2(g) + H2O2(l)----> 2H2O(l)

  15. AP Chemistry

    1) Calculate the volume of air at 30 degrees C and 1.00 atm that is needed to burn completely 10.0 grams of propane. Assume that air is 21.0 percent O2 by volume. 2) Assuming all of the heat evolved in burning 30.0 g of propane is transferred to 8.00 kg of

  16. chemistry

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

  17. 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

  18. Chemistry

    Calculate the DELTA H(rxn), DELTA S(rxn), DELTA S(universe), DELTA G(rxn). For each system below indicate whether DELTA S and DELTA H are positive or negative. Then indicate if the reaction is entropy driven, enthalpy driven or neither. C3H8(g) + 2O2(g) =>

  19. Chemistry

    Please help me N2O5(g) + H2O(l) --> 2HNO3(l) delta H° = -76.2 kJ H2O(l) --> H2(g) + 1/2O2(g) delta H° = 286.0 kJ 1/2N2(g) + 3/2O2(g) + 1/2H2(g) --> HNO3(l) delta H° = -174.0 kJ Calculate delta H° for the reaction 2N2O5(g) --> 2N2(g) + 5O2(g)

  20. Chemistry

    How would you calculate delta H for the following reaction: 2P + 5Cl2 -> 2PCl5 Given: PCl3 + Cl2 -> PCl5 Delta H=-87.9 kJ 2P + 3Cl2 -> 2PCl3 Delta H=-574 kJ I have no clue how to do this since I was absent. Can someone help?

  21. Chemistry

    Calculate the delta G of the reaction using the following information. 4HNO3+ 5N2H4 --> 7N2+ 12H2O Delta H(Kj/mol) -133.9 50.6 0 -285.8 Delta S(J/mol x K) 266.9 121.2 191.6 70.0

  22. chemistry

    Given overall reaction: P4 + 10Cl2 ---> 4PCl5 Delta H for the reaction = ? PCl5 -----> PCl3 + Cl2 Delta H = +157 kJ P4 + 6Cl2 ----> 4PCl3 Delta H = -1207 kJ Calculate the Delta H for the overall reaction.

  23. Chemistry

    Calculate the molar enthalpy for the following reaction. HCl(aq) + NH3 (aq) --> NH4Cl (aq). HCl = 50 ml (2.00M) NH3 = 50 ml (2.05 M) Delta T = 9.28 degrees Celsius. Ccal = 28.9J/g degrees celcius.

  24. chemistry

    At 25 C the following heats of reaction are known: 2CIf (g)+ O2(g) -> CL2O (g) + f2O Delta H rxn= 167.4 kj/mol 2CIf3(g) + 2O2 (g)-> Cl2O(g) + 3F2O(g) Delta H rxn= 341.4 2F2(g) + O2(g) -> 2F2O(g) Delta H rxn= -43.4kj/mol at the temperature, use Hess's Law

  25. 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!

  26. science, chemistry

    2Al(s)+ 3Cl2(g)=2AlCl3(s) For the above reaction calculate: A) delta H, then state whether the reaction is endothermic or exothermic B) delta s, then whether the reaction becomes more or less disorder. C) delta G, the state whether the reaction is

  27. Chemistry

    Given the Data: N2(g) + O2g) = 2NO(g) delta H = 180.7kj, 2NO(g) + O2(g) = 2NO2(g) delta H = 0113.1kj, 2N2O(g) = 1N2(g) + O2(g) delta H = -163.2kj. Using Hess’s Law calculate delta H for the reaction: N2O(g) + NO2(g) = 3NO(g)

  28. Chemistry

    1) A reactions has a delta H of -76 Kj and a delta S of -117 J/K. Is the reaction spontaneous at 298 K? Work: Delta G= -76kJ/mol - 298K(-117J/K/1000) Delta G= -41.134 Spontaneous 2) A reaction has a delta H of 11 kJ and a delta S of 49 J/K. Calculate the

  29. 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 =

  30. Chemistry

    Given the thermodynamic data in the table below, calculate the equilibrium constant for the reaction: 2SO2(g)+O2--> 2SO3 Substance (DeltaH^o) (Delat S^o) SO2 -297 249 O2 0 205 SO3 -395 256 Answer (it was given) 2.32x10^24 Even though the answer is given

  31. Chemistry

    Calculate delta G of a reaction with equilibrium constant, K= 9.5 x 10^5 at 25 degrees C

  32. 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)

  33. 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 +

  34. Chem

    For the reaction I2(s)+Cl2(g) ==> 2ICl(g) delta H= 36kJ, delta S= 158.8J/K at 25° C. Calculate the temperature at which Keq is 4.0*10^3. delta G= (delta H)- T(delta S) = 36 - (298)(0.1588) = -11.32 delta G= -RTlnK -11.32= -8.31Tln(4*10^3) -11.32= -6892.35

  35. Chemistry

    Hydrogen and methanol (CH3OH) have both been proposed as alternatives to hydrocarbon fuels. a) Write balanced chemical equations for the complete combustion of hydrogen and the complete combustion of gaseous methanol. Combustion reaction for hydrogen:

  36. Chemistry 2

    For the gaseous reaction of carbon monoxide and chlorine to form phosgene, (COCl2), calculate each of the following. (a) Calculate S° at 298 K I got -136.76 J/K using delta S = sum of delta S of products minus sum of delta S of reactants which is the

  37. Chemistry

    Calculate the enthalpy of the reaction 2B2H6 + 6O2=2B2O3 +6H2O given the following pertinent information: A. B2O3(s) + 2H2) )g) = 3O2 (g) + B2H6 (g), delta H= +2035kJ B. 2B (s) + 3H2 (g) =B2H6 (g), delta H= +36 kJ C. H2 (g) + 1/2)2 (g) =H2O (l), delta

  38. Chemistry

    The following reaction has the following standard thermodynamic parameters: Reaction: C(g) + D(g)----> E(g) Delta H rxn=-26.1kJ/mol and Delta S rxn=-69.8J/(mol*K). Calculate the temperature at which the reaction becomes nonspontaneous.

  39. chemistry

    Consider the reaction HCl + NaOH ->NaCl + H2O Given: HCl Solution: 22 degrees celsius NaOH Solution: 22 degrees celsius Final Temperature: 26.1 degrees celsius A. Calculate the amount of heat evolved when 15 mL of 1.0 M HCl was mixed with 35 mL of 1.0 M

  40. 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)

  41. 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,

  42. Chemistry

    Given the Data: N2(g) + O2g) = 2NO(g) delta H = 180.7kj, 2NO(g) + O2(g) = 2NO2(g) delta H = 0113.1kj, 2N2O(g) = 1N2(g) + O2(g) delta H = -163.2kj. Using Hess’s Law calculate delta H for the reaction: N2O(g) + NO2(g) = 3NO(g)

  43. Chemistry

    The following reaction has the following standard thermodynamic parameters: Reaction: C(g) + D(g)----> E(g) Delta H rxn=-26.1kJ/mol and Delta S rxn=-69.8J/(mol*K). Calculate the temperature at which the reaction becomes nonspontaneous.

  44. CHEMISTRY

    Please explain. The enthalpy changes for two different hydrogenation reactions of C2H2 are: C2H2+H2---->C2H4 Delta H 1 C2H2+2H2---->C2H6 Delta H 2 Which expression represents the enthalpy change for the reaction below? C2H4+H2---->C2H6 Delta H = ? A. Delta

  45. Chemistry DRBOB HELP ME PLEASE

    Please help me N2O5(g) + H2O(l) --> 2HNO3(l) delta H° = -76.2 kJ H2O(l) --> H2(g) + 1/2O2(g) delta H° = 286.0 kJ 1/2N2(g) + 3/2O2(g) + 1/2H2(g) --> HNO3(l) delta H° = -174.0 kJ Calculate delta H° for the reaction 2N2O5(g) --> 2N2(g) + 5O2(g)

  46. 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+)

  47. Chemistry(Please check answers)

    1) For a reaction delta Go is more negative than delta Ho. What does this mean? a. delta So is zero. b. delta So is negative c. delta So is positive d. delta So is negative if delta Ho is positive. e. delta So is negative if delta Ho is negative. I think

  48. Chem 141

    Write the three thermochemical equations needed to calculate the delta H for the below reaction.? 2Mg(s) + O2(g) --------> 2 MgO(s) delta H rxn = ? (Include delta H values in kJ for each reaction)

  49. Chemistry

    Is the following reaction spontaneous at 25*C? delta s reaction = -217 J/K*mol delta H rxn = -1202 KJ 2Mg (s) + O2 (g) -> 2MgO (s) delta suniverse = delta s system - delta H system / T i got positive (+) 3.81 x 10 ^ 3 J/K and my notes says it is

  50. CHEMISTRY

    calculate the delta h for the reaction 2C+2H--> C2H4 C+O2--> Co2 delta h= -393.5 C2H4+ 3O2--> 2CO2+ 2H2O delta h= 1410.9 H2+ 1/2 O2--> H2O delta h= -285.8 2CO+ O2--> 2CO2 delta h= -566.0 do you flip the first two equations and times the first and third one

  51. AP CHEMISTRY

    Could you please look over my work and see if I did this correctly? Thanks When 3.200 g of liquid ethyl alcohol (C2H5OH) is burned in a bomb calorimeter containing 3.500 kg of water, the temp rises from 22.84 degrees C to 28.36 degrees C. The calorimeter

  52. Biology

    Okay so if i have two enzyme catalyzed reactions: 1) delta g of the ES = -22kJ/mol 2) delta g od the ES = 42 kJ/mol Is this first reaction going to have a higher reaction rate because the of the negative delta g, because doesnt a negative delta g give you

  53. Chemistry 143

    Write three thermochemical equation needed to calculate delta H for the following reaction: 2Mg(s) + O2(g) = 2MgO Include delta h values in kJ for each reaction. Please help!! I don't even know were to start!!

  54. 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

  55. 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

  56. Chemistry

    2M +6HCl–>2MCl+3H2 Delta H= -638.0 Kj HClg—>HCl aq= Delta H -74.8 Kj H2+Cl2–>2HCl Delta H -1845.0 Kj MCl3s–> MCl3 aq Delta H -249.0 Kj Use the information above to determine the enthalpy of the following reaction. 2M +3Cl2–>2MCl3 Delta H =???

  57. Chemistry(Please check answers)

    1) 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 So for the reaction N2 (g) + 2 O2 (g)-> 2 NO2 (g) to be? I did products - reactants

  58. 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?

  59. 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.

  60. Chemistry

    Why these answers are so? 1- For this reaction 2H2 + O2 = 2H2O a- dela H=delta Hf b-delta Hc= delta Hf c- delta H= delta Hc d- delta S= delta H and the answer is b , but how and why? 2- For this reaction 2S + 3O2 = 2SO3 + 792 kJ which of the following

  61. 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

  62. chem!

    Calculate the heat of reaction for the incomplete combustion of 67.0g propane producing carbon monoxide gas and water vapour. how would I go about and do this question? What are you studying? Do you know how to use the thermodynamic tables (delta Ho, etc).

  63. chemistry

    Q1) For the reaction, A to B, Delta H= +11.00 kJ mol-1 and Keq is 12.50 Calculate i) delta G and ii) delta S at 25 C (degrees celcius) 0 C degrees celcius = 273.15 K; R = 8.314 J K-1 mol-1] PLease help dr bob222

  64. Chemistry

    Please help, I am having trouble solving these problems at nonstandard temperatures. Methanol burns in oxygen to form carbon dioxide and water. Using the balanced reaction, 2CH3OH(l) + 3OH2(g) --> 2CO2(g) + 4H2O(g) 1) Calculate delta H(rxn) in kJ at 24

  65. Physical Chemistry

    When the reaction glucose-1-phosphate (aq) --> glucose-6-phosphate (aq) is at equilibrium at 25.0 degrees celcius, the amount of glucose-6-phosphate present is 95% of the total. A.) Calculate the Standard Delta G at 25.0 degrees celcius. B.) Calculate

  66. chemistry

    Q1) For the reaction, A to B, Delta H= +11.00 kJ mol-1 and Keq is 12.50 Calculate i) delta G and ii) delta S at 25 C (degrees celcius) 0 C degrees celcius = 273.15 K; R = 8.314 J K-1 mol-1]

  67. equibrium - help!

    Consider the reaction CO(g) + H2O(g) CO2(g) + H2(g) Use the appropriate tables to calculate a) delta-G*f at 552*C b) K at 552*C I'm pretty sure I have a good idea of how to do this: I believe I can use Gibbs-Helmholtz equation to account for the

  68. CHEMISTRY

    I put down all the info that I found but I cant figure out the questions 1 & 2 at the bottom!! Empty Calorimeter- 11.6 g Room temp - 21 degrees celcius Three different experiments of 50mL 1(M) HCl reacts with 0.15 g Mg, 0.25g Mg, and 0.35g Mg respectively.

  69. Chemistry, PPPLLEASE Help!

    Hello, I'm confused on what these problems are telling me. Is questions a) and b) the same? I don't know, please help me I don't know what to do... The inteconversion of DHAP and G3P is a part of both the glycotic pathway and the Calvin cycle for

  70. P-Chem

    The equilibrium constant K for the hydrolysis of adenosine triphosphate (ATP) to adenosine diphosphate (ADP) and phosphate is 1.66X10^5 at 37 degrees celcius, and Standard Delta H is -20.1 kJ/mol. Calculate Standard Delta S for the hydrolysis at 37 degrees

  71. chemistry

    Styrene is produced by catalytic dehydrogenation of ethyl- benzene at high temperature in the presence of superheated steam. (a) Find ÄH°rxn, ÄG °rxn, and ÄS °rxn, given these data at 298 K: (b) At what temperature is the reaction spontaneous? What

  72. CHEM

    Could you please look over my work and see if I did this correctly? Thanks When 3.200 g of liquid ethyl alcohol (C2H5OH) is burned in a bomb calorimeter containing 3.500 kg of water, the temp rises from 22.84 degrees C to 28.36 degrees C. The calorimeter

  73. chemistry

    Styrene is produced by catalytic dehydrogenation of ethyl- benzene at high temperature in the presence of superheated steam. (a) Find ÄH°rxn, ÄG °rxn, and ÄS °rxn, given these data at 298 K: (b) At what temperature is the reaction spontaneous? What

  74. chemistry

    Styrene is produced by catalytic dehydrogenation of ethyl- benzene at high temperature in the presence of superheated steam. (a) Find ÄH°rxn, ÄG °rxn, and ÄS °rxn, given these data at 298 K: (b) At what temperature is the reaction spontaneous? What

  75. Chemistry

    Calculate the equilibrium constant, k a reaction with delta G= -32.5 kj/mol at 25 degrees C

  76. Chemistry

    In a constant-pressure calorimeter, 50.0 mL of 0.300 M Ba(OH)2 was added to 50.0 mL of 0.600 M HCl. The reaction caused the temperature of the solution to rise from 24.50 degrees C to 28.59 degrees C. If the solution has the same density and specific heat

  77. Chemistry

    In a constant-pressure calorimeter, 50.0 mL of 0.300 M Ba(OH)2 was added to 50.0 mL of 0.600 M HCl. The reaction caused the temperature of the solution to rise from 24.50 degrees C to 28.59 degrees C. If the solution has the same density and specific heat

  78. chemistry

    Styrene is produced by catalytic dehydrogenation of ethyl- benzene at high temperature in the presence of superheated steam. (a) Find ÄH°rxn, ÄG °rxn, and ÄS °rxn, given these data at 298 K: (b) At what temperature is the reaction spontaneous? What

  79. Chemistry(Please help)

    1) Nitrosyl chloride (NOCl) decomposes at high temperature. The equation is 2 NOCl (g) -> 2 NO (g) + Cl2 (g) at 227oC Using delta Ho = 81.2 kJ and delta So = 128 J/K, calculate the value of the equilibrium constant for this reaction. I do not know how to

  80. CHEMISTRY

    A 2.75 g sample of the hydrocarbon acetone, CH3COCH3, is burned in a bomb calorimeter with 975 mL of water, initially at 23.50 degrees celsius. The bomb is constructed of 285.0 g of nickel metal having a specific heat capacity of Cp = 0.826 J/ g degrees C.

  81. AP Chemistry

    A 2.75 g sample of the hydrocarbon acetone, CH3COCH3, is burned in a bomb calorimeter with 975 mL of water, initially at 23.50 degrees celsius. The bomb is constructed of 285.0 g of nickel metal having a specific heat capacity of Cp = 0.826 J/ g degrees C.

  82. AP CHEMISTRY

    A 2.75 g sample of the hydrocarbon acetone, CH3COCH3, is burned in a bomb calorimeter with 975 mL of water, initially at 23.50 degrees celsius. The bomb is constructed of 285.0 g of nickel metal having a specific heat capacity of Cp = 0.826 J/ g degrees C.

  83. Chemistry

    A 2.75 g sample of the hydrocarbon acetone, CH3COCH3, is burned in a bomb calorimeter with 975 mL of water, initially at 23.50 degrees celsius. The bomb is constructed of 285.0 g of nickel metal having a specific heat capacity of Cp = 0.826 J/ g degrees C.

  84. Chemistry

    A 2.75 g sample of the hydrocarbon acetone, CH3COCH3, is burned in a bomb calorimeter with 975 mL of water, initially at 23.50 degrees celsius. The bomb is constructed of 285.0 g of nickel metal having a specific heat capacity of Cp = 0.826 J/ g degrees C.

  85. Chemistry

    The net reaction in a voltaic cell with Eºcell= +.726V 2Fe^3+(aq) + 3Zn(s) --> 2Fe(s) + 3Zn^2+(aq) What is the delta Gº for this reaction at 25ºC I tries using this equation: delta G = -nFEºcell = -n(90485)(.726) However, I don't know how to calculate

  86. Chemistry

    I need to calculate the value of Kp at 25 degrees celsius using the delta Go value. Delta Go = -29.10kJ I know that Delta Go = -RT lnK and that R=8.314e-3kJ/K mol -delta Go / RT I did -29.10 / 8.314e-3 X 298K and -11.74 but this was wrong. I am stuck. What

  87. 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),

  88. 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

  89. chemistry

    For a certain reaction, Delta H(not) = -76.8 kj and delta S(not) = -217 j/k. If n =3, calculate E for the reaction at 25degrees celcius.

  90. chemistry

    For a certain reaction, Delta H(not) = -76.8 kj and delta S(not) = -217 j/k. If n =3, calculate E for the reaction at 25degrees celcius.

  91. 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

  92. Chemistry

    The molar solubility of lead iodide is 1.45*10^-3M at 20 degrees C and 6.5*10^-3M at 80 degrees C . What are the values of delta H not and delta S not for dissolution of PbI2 ? PbI2(s) ---> Pb2+(aq) + 2I- (aq) You may assume that delta H and delta S are

  93. Chemistry

    Calculate the work involved if a reaction with an enthalpy change of -2418 kJ is carried out in a vessel with a mobile, frictionless piston. Other details: the reaction is H2(g) + 1/2Oxygen2(g) yields H2O(g) with enthalpy change of -241.8 kJ/mol. The

  94. Chemistry

    Na reacts violently with H2O to produce NaOH and H2. The resulting solution has a higher T than it did before the Na was added. What are the expected changes? deltaH ? deltaS >0 deltaG 0 I know the last three for a fact. Is deltaG "

  95. Chemistry

    The following reaction has the following standard thermodynamic parameters: Reaction: C(g) + D(g)----> E(g) Delta H rxn=-26.1kJ/mol and Delta S rxn=-69.8J/(mol*K). Calculate the temperature at which the reaction becomes nonspontaneous.

  96. Chemistry

    Consider the reaction 2 SO2(g) + O2(g) in equilibrium with 2 SO3(g) . At 25°C delta H° = -197.78 kJ and delta S° = -187.95 J/K. Using this information, calculate the equilibrium constant for the reaction at -32°C. (R = 8.314 J/K) Enter your answer

  97. Chemistry

    Please explain. The enthalpy changes for two different hydrogenation reactions of C2H2 are: C2H2+H2---->C2H4 Delta H 1 C2H2+2H2---->C2H6 Delta H 2 Which expression represents the enthalpy change for the reaction below? C2H4+H2---->C2H6 Delta H = ? A. Delta

  98. Chemistry DRBOB HELP ME PLEASE

    Please help me N2O5(g) + H2O(l) --> 2HNO3(l) delta H° = -76.2 kJ H2O(l) --> H2(g) + 1/2O2(g) delta H° = 286.0 kJ 1/2N2(g) + 3/2O2(g) + 1/2H2(g) --> HNO3(l) delta H° = -174.0 kJ Calculate delta H° for the reaction 2N2O5(g) --> 2N2(g) + 5O2(g)

  99. chemistry

    a 2.00g sample of zinc metal is added to a calorimeter containing 150g of nitric acid solution initially at 20.0 degrees celsius . The temperature of the solution increased to 28.0 degrees celsius . Calculate the delta H of the reaction assuming that the

  100. Chemistry!

    Calculate the work involved if a reaction with an enthalpy change of -2418 kJ is carried out in a vessel with a mobile, frictionless piston. Other details: the reaction is H2(g) + 1/2Oxygen2(g) yields H2O(g) with enthalpy change of -241.8 kJ/mol. The

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