1. chem

    A certain constant-pressure reaction is nonspontaneous at 37°C. The entropy change for the reaction is 83 J/K. What can you conclude about the sign of ÄH? What can you conclude about the magnitude of ÄH?
  2. Please Help Me

    Use the equation for the synthesis of hydrogen to answer the following. C (s) + H2O (l) -> CO (g) + H2 (g) deltaH = + 31.3 kcal/mol carbon deltaS = +32 cal/(mol•K) Calculate the energy change (deltaH) when 5.00 g of carbon is consumed. Calculate the
  3. Chemistry

    Use the equation for the synthesis of hydrogen to answer the following. 10 points. C (s) + H2O (l) -> CO (g) + H2 (g) deltaH = + 31.3 kcal/mol carbon deltaS = +32 cal/(mol•K) Calculate the energy change (deltaH) when 5.00 g of carbon is consumed.
  4. chem

    Check the correct statements for the above reaction. Choose at least one answer. a. The reaction is exothermic. b. The reaction is endothermic. c. The change in entropy is positive. d. The change in entropy is negative. e. The reaction is at equilibrium.
  5. Chemistry

    A reaction has delta H_rxn= -125 kJ and delta S_rxn= 324 J/K. At what temperature is the change in entropy for the reaction equal to the change in entropy for the surroundings?
  6. 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
  7. chem please help drbob222

    What will be the result of a reaction if its enthalpy change is positive, its entropy change is negative and Gibbs free energy is positive? A. Spontaneous, if the temperature is high B. Nonspontaneous, if the temperature is low C. Always spontaneous D.
  8. chem

    What will be the result of a reaction if its enthalpy change is positive, its entropy change is negative and Gibbs free energy is positive? A. Never spontaneous B. Nonspontaneous, if the temperature is low C. Spontaneous, if the temperature is high D.
  9. Thermodynamics

    The initial state consists of a closed system containing one mole of water (liquid) at 85°C and 1 atmosphere pressure. The immediate surroundings are also at 85°C and 1 atmosphere pressure. The change in state is described as this one mole of liquid
  10. chemistry

    2C2H2(g) + 5O2(g)→4CO2(g) + 2H2O(g) a. Determine the enthalpy change for the reaction. ΔH = (4(-393.5)+ 2(-241.8)) – (2(227) + 5(0)) The enthalpy change is -2511.6. b. Determine the entropy change for the reaction. ΔS = (4(213.7)+
  11. chemistry

    What effect does raising the temperature of the reaction chamber at a constant pressure have on the following reaction at equilibrium? 2NO2(g) N2O4(g) + heat A. The equilibrium shifts toward the reactants because the reverse reaction is endothermic. B. The
  12. chemistry

    For which of the reactions listed below will Gibbs free energy always be negative? A. An exothermic reaction that increases in entropy B. An endothermic reaction that decreases in entropy C. An endothermic reaction that increases in entropy D. An
  13. Chemistry

    2 H2S (g) + SO2 (g) <===> ƒnƒn3 S (s) + 2 H2O (g) 1) At 298 K, the standard enthalpy change, H¢X, for the reaction represented below is -145 kilojoules. (a) Predict the sign of the standard entropy change, S¢X, for the reaction. Explain the basis
  14. Chemistry

    A gaseous reaction occurs at a constant pressure of 50.0 atm and releases 69.8 kJ of heat. Before the reaction, the volume of the system was 8.80 L . After the reaction, the volume of the system was 2.80 L . Calculate the total internal energy change,
  15. 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
  16. 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
  17. 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)/ ?? /
  18. 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)/ ?? /
  19. 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)/ ?? /
  20. 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
  21. CHEMISTRY

    The enthalpy change of an endothermic reaction is 8 kJ , and this reaction is spontaneous at 25 oC ,, what is the expected entropy change ? thank you a lot
  22. Chemistry

    the type of reaction in a voltaic cell is best described as 1.spontaneous oxidation reaction only 2.nonspontaneous oxidation reaction only 3.spontaneous oxidation-reduction reaction 4.nonspontaneous oxidation-reduction reaction i know its spontaneous, but
  23. 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
  24. 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
  25. 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
  26. college chemistry

    for the reaction at 298 K 2A+b ---->C enthalpy=100 K/cal entropy= 0.050 kcal/k assuming enthalpy and entropy to be constant over the temperature range, at what temperature will the reaction become spontaneous? answer: T>2000K
  27. Thermodynamics

    The initial state consists of a closed system containing one mole of super-heated liquid water at 115°C and 1 atmosphere pressure. The immediate surroundings are also at 115°C and 1 atmosphere pressure. The change in state is described as this one mole
  28. Chemistry

    All of the following apply to the reaction A(g)+B(g)<==>C(g) as it is carried out at constant temperature in a rigid container EXCEPT: A)The total pressure decreases B)The rate of reaction decreases C)The entropy of the system decreases D)The number
  29. chemistry

    Calculate the change in entropy (ΔS˚) of reaction (J/K) for the equation as written. BaCO3(s) → BaO(s) + CO2(g) Table: S° (J/(K mol)) BaCO3(s) = 112 BaO(s) = 70.3 CO2(g) = 213.7 So the answer is -41.7 I thought to find the entropy of
  30. Chem

    The entropy of combustion of benzoic acid is zero. This means that... a)combustion is not spontaneous here. b)combustion is spontaneous, however, since the reaction is exothermic. c)combustion is spontaneous, however, since the reaction is endothermic.
  31. chemistry

    A mole of reacts at a constant pressure of 43.0atm via the reaction Before the reaction, the volume of the gaseous mixture was 5.00L . After the reaction, the volume was 2.00L . Calculate the value of the total energy change, , in kilojoules.
  32. Chemistry

    A gaseous reaction occurs at a constant pressure of 50.0 atm and releases 55.6 kJ of heat. Before the reaction, the volume of the system was 7.60 L. After the reaction, the volume of the system was 2.00 L. Calculate the total internal energy change, Delta
  33. chemistry... HELPP

    A gaseous reaction occurs at a constant pressure of 45.0 atm and releases 62.5 Kj of heat. Before the reaction, the volume of the system was 8.60 L . After the reaction, the volume of the system was 3.00 L. Calculate the total internal energy change in
  34. chemistry

    Consider the following reaction. 2 CO (g) + O2 (g) −→ 2 CO2 (g) What is most likely true about the entropy change for this reaction? Why would the delta s of the rxn be less than zero? thanks.
  35. physical chemistry

    I tried working out this problem but am unsure of a few steps. Please help me if you can. Consider O3 --->1.5O2 At 210degrees Celsius and an initial gas pressure of 0.23atm, it is found that the rate of reaction is 1.8E-2 mol/(Lxs). a) What is the
  36. Chemistry

    Consider the following reaction: 2Na + Cl2  2NaCl ΔH = -821.8 kJ (a) Is the reaction exothermic or endothermic? (b) Calculate the amount of heat transferred when 5.6 g of Na reacts at constant pressure. (c) How many grams of NaCl are produced during an
  37. Science

    Consider the following reaction: 2Na + Cl2  2NaCl ΔH = -821.8 kJ (a) Is the reaction exothermic or endothermic? (b) Calculate the amount of heat transferred when 5.6 g of Na reacts at constant pressure. (c) How many grams of NaCl are produced
  38. Chemistry

    consider the following reaction: 2CH3OH(g) yields 2CH4(g) + O2(g) change in enthalpy= 252.8kJ Calculate the amount of heat transferred when 26.0 g of {\rm CH_3OH} (g) is decomposed by this reaction at constant pressure.
  39. chemistry

    LeChatelier's Principle !!!! ? plz help me with this problem the following reaction may be used to remove sulfur compounds from power plant smokestack emission. 2HS(g) + SO2 >>>> 3S + 2H2O ...... DELTA h = -145 KJ the value of the euilibrium
  40. Chemistry

    If a catalyst is added to a system at equilibrium and the temperature and pressure remain constant there will be no effect on the: (1) rate of the forward reaction (2) rate of the reverse reaction (3) activation energy of the reaction (4) heat of reaction
  41. Chemistry Lab

    What would happen to the reaction rate of a solution if 10 mL or more of water is added? Will the reaction rate increase or decrease? The following reaction occurs without a change in the color 2A (g) + B2(g) --- 2AB (g) a) How could you monitor the
  42. Chemistry Lab

    What would happen to the reaction rate of a solution if 10 mL or more of water is added? Will the reaction rate increase or decrease? The following reaction occurs without a change in the color 2A (g) + B2(g) --- 2AB (g) a) How could you monitor the
  43. Chemistry - Help!!!

    Which of the following criteria indicate that a reaction is SPONTANEOUS? Check all that apply. a) The change in free energy is positive. b) The entropy of the universe decreases. c) The change in free energy is negative. d) The entropy of the system
  44. chemistry ( little urgent pls)

    For oxidation of iron 4Fe+3O2=2Fe2O3 the entropy change is -549.45JK^-1mol^-1 at 298K. Though it has negative entropy change in the reaction is spotaneous.why? (Delta r H theta ∆rH°=-1648×10^3 J ml^-1. Is it because ∆G is negative????
  45. Chemistry<--------

    Sulfur dioxide in the effluent gases from coal-burning electric power plants is one of the principal causes of acid rain. One method for reducing SO2 emissions involves partial reduction ofSO2 to H2S followed by catalytic conversion of the H2S and the
  46. chemistry

    enthalpy change^H is +23kJ mol-1 of phosphine (PH3) for the reaction 2P(s)red+3H2(g)---->2PH3(g) a) Calc. entropy change for this reaction. Explain how this information allows you to determine the spontaneity or non-spontaneity of this reaction at any
  47. Chemistry

    Explain how the entropy and enthalpy values ( + or -) can be used to explain the spontaneous or nonspontaneous solvation of different salts. I know that the if the entropy value is higher the more spontaneous the process is but don't know why. And I don't
  48. chemistry- transferring energy

    For the following questions, use the reaction SO3(g) SO2(g) + O2(g), with ÄH = 98.4 kJ/mol and ÄS = 0.09564 kJ/(mol·K). (8 points) i. Draw a possible potential energy diagram of the reaction. Label the enthalpy of the reaction. (2 points) ii. Is the
  49. chem 100

    For the reaction CH3OH(g)←→CO(g) + 2H2(g), a. Determine ΔHo and ΔSo for the reaction at 298K b. Determine the entropy change for the surroundings assuming that they are at 298 K. What does this result tell you? c. Calculate ΔGo
  50. (11) Chemistry - Science (Dr. Bob222)

    In the following hypothetical reaction A + B → C + D, the equilibrium constant, Keq is less than 1.0 at 25°C and decreases by 35% on changing the temperature to 45°C. What must be true according to this information? A. The ΔH° for the
  51. Chemistry

    Which of the following is the best definition of Hess' Law? A. Since enthalpy is a state function, it will be different if a reaction takes place in one step or a series of steps. B. Heat is always released by the decomposition of 1 mole of a compound into
  52. Chemistry

    2 Al(s) + 3 Cl2(g) → 2 AlCl3(s) Into a cylinder with a moveable piston (pressure stays constant), a piece of aluminum is placed and chlorine gas is added. After they react, the temperature inside the piston is considerable higher than its initial
  53. chemistry

    Consider the following reaction in a closed reaction flask. If 0.600 atm of gas A is allowed to react with 1.20 atm of gas B and the reaction goes to completion at constant temperature and volume, what is the total pressure in the reaction flask at the end
  54. chemistry

    CH3OH(g) ----> CO(g) + 2H2 (g) (delta H =+90.7k) A) is heat absorbed or released in the course of this reaction? b) calculate the amount of heat transferred when 45.0g of CH3OH(g)is decomposed by this reaction at constant pressure. c) for a given sample
  55. 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 I keep using
  56. Chemistry

    I need to calculate the mass of CO2 produced in the reaction of NaHCO3 + HCl Data Mass of NaHCO3 = .05g Mass of system before reaction 117.9 g Mass of system after reaction 117l98 Maxium pressure 1.4094 initial pressure 1.0094 pressure change .4 temp
  57. Chemistry

    Assuming the dissolution of borax in water is a spontaneous reaction, do you expect the change in enthalpy to be positive or negative or are both signs possible? Explain your answer A. Neither, enthalpy does not change, the positive entropy for the
  58. chem

    For the gaseous equilibrium represented below, it is observed that greater amounts of PCl3 and Cl2 are produced as the temperature is increased. PCl5(g) <===> PCl3(g) + Cl2(g) a) What is the sign of S° for the reaction? Explain. b) What change, if
  59. Chemistry

    Which of the following is the best definition of Hess' Law? A. Heat is always released by the decomposition of 1 mole of a compound into its constitute elements. B. The enthalpy of a process is the difference between the enthalpy of the products and the
  60. chemistry

    What is the standard entropy of reaction, the standard entropy of reaction, in J/K, for the combustion reaction of ethylene described in the previous questions? The temperature is 298.15K. (Enter your answer as a signed number in scientific notation
  61. chemistry

    In a reaction A to products, ,4.40 min after the reaction is started concentration of A is 0.588M. The rate of reaction at this point is rate= -change in concentration of A/change in time=2.2x10^-2Mmin^-1. Assume that this rate remains constant for a short
  62. Chemistry

    The reaction b/t H2 and O2 yield water vapor and has a change of heat =-484kJ.Ho much PV work is done and what is the value of the change of E in kJ for the reaction of 0.50 mol of H2 with 0.25 mol of O2 amd atmospheric pressure of 1.00 , the volume change
  63. Chemistry

    Which of the following is the best definition of Hess' Law? A. Heat evolved in a given process can be expressed as the sum of the heats of several processes that, when added, yield the process of interest. B. The enthalpy of a process is the difference
  64. chemistry

    If a particular reaction absorbs 252 kJ of heat while doing 105 kJ of work at constant pressure. What are the ΔE and ΔH for values for the reaction? Is the reaction endothermic or exothermic?
  65. Chemistry

    For the reaction given, the value of the equilibrium of the constant at 400 K is 7.0. Br2(g)+ Cl2(g)=2BrCl(g) Does the: Reaction proceed to the left? Reaction proceed to the right? Partial pressure represent a system in an equation?
  66. 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.
  67. 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.
  68. 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.
  69. another A.P Chemistry Question

    A different rigid 5.00L cylinder contains 0.176mol of NO(g) at 298 k. A 0.176mol sample of 02(g) is added to the cylinder, where a reaction occurs to produce NO2(g) (d) write the balanced equation for the reaction. (e) calculate the total pressure, in atm,
  70. chemistry

    Choose all of the following statements about the equilibrium constant K that are true: (a) If the K value for a reaction is > 1 then Go must be negative for this reaction (b) A large value for K implies there is a strong driver for the reaction to
  71. chemistry please help

    The reaction between hydrogen and chlorine gases gives hydrogen chloride gas in the following reaction: H2(g) + Cl2(g) = 2HCl(g) It is found experimentally that 1 mole of H2 gas reacts with 1 mole of Cl2 gas at constant temperature and pressure, to release
  72. Chemistry- HWK CHECK

    1. A solution in which no more solid can be dissoved is referred to as ____. Answer: saturated 2.At constant pressure, heat can be referred to as (entropy, enthalpy, or free energy). Answer: enthalpy The measure of disorder or randomness of a system
  73. 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
  74. Hess' law

    Which of the following is the best definition of Hess' Law? A. Heat is always released by the decomposition of 1 mole of a compound into its constitute elements. B. Since enthalpy is a state function, it will be different if a reaction takes place in one
  75. Chemistry 3A

    An aqueous solution contains the ions B, C, and D that are in equilibrium with one another according to the reaction B (aq) + C (aq) ->/<- D (aq) A certain amount of water is added so as to double the volume of this solution, while keeping the
  76. Chemistry

    . For the gas reaction at low pressure 2NOBr ¡ê 2NO + Br2 ¥ÄH = +61.1 kJ which of the following statements are true? a) Adding more Br2 shifts reaction to the right b) Removing some NOBr shifts reaction to the left c) Increasing temperature shifts
  77. Science help

    Will someone please check my work for me? Molecules involved in a chemical reaction must meet to react. What is this concept called? entropy enthalpy collision theory<---- reaction rate 2. Which of the following equations is used to describe reaction
  78. Chemistry

    A student tested the effect of temperature on the decomposition of N2O5. He found that the rate of the reaction at a lower temperature was 4.2 x 10–3 s–1 and the rate at a higher temperature was 1.6 x 101 s–1. What is wrong with the student's data?
  79. chemistry kinetics

    The reaction SO2Cl2(g) → SO2(g) + Cl2(g) is a first order reaction carried out at constant volume at 600 K whose t1/2 is 4.1 hr. The initial pressure of SO2Cl2 is 1.25 atm. What will be the total pressure of the system after 1 hour?
  80. Chemistry -Thermodynamics

    1. Cl2(g) -> 2Cl(g) 2. H2(g) at 5.0 atm -> H2(g) at 1.0 atm 3. sublimation of solid CO2 4. 2H2(g) + O2(g) -> 2H20(g) 5. PCl5(g) <-> PCl3(g) + Cl2(g) A. The change in entropy will be positive. B. The change in entropy will be zero. C. The
  81. (1-16)Chemistry - Science

    Consider the reaction: SO2 (g) + NO2 (g) ==> SO3 (g) + NO (g) At T = 1000 K, where the reaction is exothermic with an equilibrium constant K = 9.00 The reaction vessel is charged initially with all four gases, each at a pressure of 0.5 atm. After
  82. chemistry

    . For the gas reaction at low pressure 2NOBr ↔ 2NO + Br2 ΔH = +61.1 kJ which of the following statements are true? a) Adding more Br2 shifts reaction to the right b) Removing some NOBr shifts reaction to the left c) Increasing temperature shifts
  83. 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
  84. Thermodynamics

    5 pounds of an ideal gas with R=38.7 and K=1.668 have 300Btu of heat added during a reversible constant pressure change of state, initial temperature=80°F. Determine: a.)the final temperature b.)change of internal energy change of enthalpy change of
  85. ap chemistry :(

    consider the reaction C6H14 + 9.5O2 yields 6CO2 + 7H2O at constant pressure. which response is true? 1. work may be done on or by the system as the reaction occurs, depending upon the temperature. 2. work is done on the system as the reaction occurs. 3. no
  86. chem

    If a reaction rate increases with temperature, how will the rate constant of the reaction change with temperature? A. The rate constant only changes upon addition of a catalyst to the reaction. B. The rate constant will decrease with temperature. C. The
  87. science

    If a reaction rate increases with temperature, how will the rate constant of the reaction change with temperature? A. The rate constant only changes upon addition of a catalyst to the reaction. B. The rate constant will decrease with temperature. C. The
  88. AP Chemistry

    Q - An electrochemical reaction occurs between an unknown element and zinc. The half-cell reaction for the zinc is: Zn(s) → Zn2+(aq) + 2e− The cell potential for the reaction is Eºcell = 1.83 V. Is the reaction spontaneous or nonspontaneous?
  89. Chemistry

    The equilibrium constant Kc for the following reaction is equal to 0.20 at 250°C. Calculate the equilibrium constant Kp for the reverse reaction at the same temperature. COCl2 (g) = CO (g) + Cl2 (g) My Answer: To find the reverse reaction of Kc, it should
  90. Chemistry

    I would really like to understand how to do these problems, because my exam is coming up in a few weeks. I still cannot comprehend how you can tell if a system is is positive or negative according to reaction. For #1, I presume it is E if it is spontaneous
  91. Chemistry

    I would really like to understand how to do these problems, because my exam is coming up in a few weeks. I still cannot comprehend how you can tell if a system is is positive or negative according to reaction. For #1, I presume it is E if it is spontaneous
  92. ap chemistry :(

    consider the reaction C6H14 + 9.5O2 yields 6CO2 + &H2) at constant pressure. which response is true? 1. work may be done on or by the system as the reaction occurs, depending upon the temperature. 2. work is done on the system as the reaction occurs. 3. no
  93. Chemistry

    The lab we are doing is: Determining the ENTHALPY of a Chemical Reaction. There are three reactions. Reaction 1: NaOH + HCl, Reaction 2: NaOH + NH4Cl, and Reaction 3: HCl + NH3. I found the max temp, initial temp, and temp change of each reaction. Can you
  94. CHE1

    Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reaction: 2H2O2(l) → 2H2O(l) + O2(g) ΔH = -196 kJ Calculate the value of q (kJ) in this exothermic reaction when 4.60 g of hydrogen peroxide decomposes at constant
  95. Chemistry

    My question is ..can anyone explain how to do problem #2? I feel lost. :( And could you also explain why? Problem#1, is that a regular dG = dH - TdS problem? Then using Go = -RTlnK to find K? Im just afraid if there are other seps to it.. 1. The combustion
  96. chemistry

    Which of the following can we predict from an equilibrium constant for a reaction? 1 The extent of a reaction 2 Whether the reaction is fast or slow 3 Whether a reaction is exothermic or endothermic a. 1 only b. 2 only c. 3 only d. 1 and 2 only e. 1 and 3
  97. Chemistry

    If delta H°rxn and delta S°rxn are both positive values, what drives the spontaneous reaction and in what direction at standard conditions? The spontaneous reaction is a)enthalpy driven to the left. b)entropy driven to the right. c)entropy driven to the
  98. chem help!

    Which statement is true about a reaction at equilibrium? A. The reaction is not reversible. B. The reaction concentrations of the reactants and products are always equal. C. The reaction rates of the forward and reverse reaction are always equal. D. The
  99. AP CHEM-- check work?

    How many moles of ATP must be converted to ADP by the reaction ATP(aq) + H2O ---> ADP(aq) + HPO4-2(aq) + 2H+(aq) delta-G*= -31 kJ to bring about a nonspontaneous biochemical reaction in which delta-G*= +372 kJ? I did my work out like this..: 372 kJ x 1
  100. Pchem

    2 NO2(g) N2(g) + 2 O2(g) The ¥ÄH¡Æ for the reaction above is -66.4 kJ. The system is initially at equilibrium. What happens if NO2 is added to the reaction mixture at constant temperature and volume? (Select all that apply.) And here's the options. The