Predict whether each of the following reactions would be spontaneous or non spontaneous under standard conditions or if it is impossible to tell with the data given. a)2KClO3(s)+3C(s)-->3CO2(g)+2KCl(s) Exothermic b) 2NO(g) + O2(g) ---> 2NO2(g) Exothermic c)H2(g)+Zn(ClO3)2(s)-->2HClO3(l)+Zn(s) Endothermic Does information

18,966 results
  1. Chemistry

    Classify the possible combinations of signs for a reaction's ∆H and ∆S values by the resulting spontaneity. A) Spontaneous as written at all temperatures. B) Spontaneous in reverse at all temperatures. C) Spontaneous as written above a certain

  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

    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+

  4. 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) ->

  5. Chemistry

    Q: The value of ΔS° for this reaction is 177 J/K. At what temperatures is this reaction spontaneous at standard conditions? Assume that ΔH° and ΔS° do not depend on temperature. I got 300.768 K through dG = dH-TdS and T=dH/dS but it's still

  6. 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 foryour

  7. 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

  8. Chemistry

    CH3COO-(aq) + H3O+(aq) → CH3COOH + H2O is spontaneous or non spontaneous rxn?

  9. chemistry--please check

    1. In which of the following processes would the entropy of the system increase? a. A liquid forming from a gas. b. A solid forming from a gas. c. The number of gas molecules increasing during a chemical reaction.

  10. 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

  11. AP Chemistry

    Q - Aluminum metal reacts with zinc(II) ion in an aqueous solution by the following half-cell reactions: Al(s) → Al3+(aq) + 3e− Zn2+(aq) + 2e− → Zn(s) Predict the potential of the cell under standard conditions. Predict whether the reaction will

  12. 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

  13. Chemistry--please check

    1. Which is true about spontaneous reactions? a. For a reaction to be spontaneous, Keq = 1. b. Spontaneous reactions happen very rapidly. c. A chemical reaction is spontaneous in both directions. *** d. Spontaneous reactions do not require that anything be

  14. 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

  15. chem

    Q: Calculate ℰ° values for the following cells. Which reactions are spontaneous as written (under standard conditions)? Balance the equations. Standard reduction potentials are found in the Standard Reduction Potentials table. (Use the lowest possible

  16. 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.

  17. 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

  18. Chemistry

    2. Aluminum metal reacts with zinc(II) ion in an aqueous solution by the following half-cell reactions: Al(s) → Al3+(aq) + 3e− Zn2+(aq) + 2e− → Zn(s) a. Predict the potential of the cell under standard conditions. (4 points) b. Predict whether the

  19. Chemistry

    Identify the correct statement for the following reaction: Br2 (l) → Br2 (g) ΔH° = 30.9 kJ ΔS° = 93.2 J/K A) The reaction is always spontaneous. B) The reaction is never spontaneous. C) The reaction is at equilibrium; therefore, ΔG° = 0. D) The

  20. Inorganic chemistry

    Given the following two half-reactions, determine which overall reaction is spontaneous and calculate its standard cell potential. Cd^2+(aq) + 2e^- ==> Cd(s) E naught = -1.21V Sn^2+ + 2e^- ==Sn(s) E naught = -0.14V

  21. Chemistry

    Which of the following is NOT true for ΔGrxn? A.) If ΔG°rxn > 0, the reaction is spontaneous in the forward direction. B.) If Q = 1, then ΔGrxn = ΔG°rxn.If ΔG°rxn = 0, the reaction is spontaneous in the reverse direction. C.) If ΔG°rxn > 0, the

  22. HW Entropy Question

    Sodium carbonate can be made by heating sodium bicarbonate: 2NaHCO3(s) ¨ Na2CO3(s) + CO2(g) + H2O(g) Given that ƒ¢H‹ = 128.9 kJ/mol and ƒ¢G‹ = 33.1 kJ/mol at 25‹C, above what minimum temperature will the reaction become spontaneous under

  23. Chemistry

    . Using the following spontaneous reactions, classify the 3 metals involved (Cr, Sn, Al) according to increasing reductant properties. a) 2Cr + 3Sn2+ ---> 2Cr3+ + 3Sn b) Al + Cr3+ ---> Al3+ + Cr

  24. Chemistry

    Predict whether the following reactions would be spontaneous or not under standard conditions or if it's impossible to tell. 2 KClO3(s) + 3 C(s) --> 3CO2(g) + 2KCl(s) Exothermic 2 NO(g) + O2(g) --> 2NO2(g) Exothermic H2(g) + Zn(ClO3)2(s) --> 2HClO3(l) +

  25. Chemistry

    Predict whether each of the following reactions would be spontaneous or non spontaneous under standard conditions or if it is impossible to tell with the data given. a)2KClO3(s)+3C(s)-->3CO2(g)+2KCl(s) Exothermic b) 2NO(g) + O2(g) ---> 2NO2(g) Exothermic

  26. 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

  27. chemistry

    Do any of you think that spontaneous combustion is possible? If a reaction brings about an increase of entropy (increase in randomness) and also exodermic, then a reaction is spontaneous. Right? Yes, I think spontaneous combustion is possible. It happens.

  28. Chemistry

    ***all negative signs should be in superscript*** Consider the following reactions: R-+ Q —> Q- + R (non-spontaneous) S + Q- —> Q + S- (non-spontaneous) S + T- —> T + S- (spontaneous) R- + U —> U- + R (spontaneous) Which of the following reactions

  29. Chemistry

    Explain why each of the following is incorrect: (a) Entropy increases in all spontaneous reactions. Wouldn't (a) be actually correct? Because when there's a spontaneous reaction, you have less stable molecules and more disorder. It will be lower in some

  30. Chemistry

    How do you know which reactions are spontaneous? For example, the equation I2(s)+2NaF(aq)->F2(g)+2NaI(aq) is spontaneous. Why is this so?

  31. chemistry help!!! please!!! DrBob222 I need you!!

    The G value for formation of gaseous water at 298 K and 1 atm is -278 kJ/mol. What is the nature of the spontaneity of formation of gaseous water at these conditions? A. The reaction is sometimes spontaneous. B. The reaction is spontaneous. C. The reaction

  32. Chemistry

    Which of the following statements is true? All spontaneous processes are exothermic All non-spontaneous processes are exothermic All spontaneous processes release free energy*** Entropy always increases in a spontaneous process

  33. Chemistry

    Consider the following reaction: CaCO3(s)→CaO(s)+CO2(g). Estimate ΔG∘ for this reaction at each of the following temperatures. (Assume that ΔH∘ and ΔS∘ do not change too much within the given temperature range.) A) 310K and is it spontaneous B)

  34. chemistry

    Reactions in which a substance decomposes by losing CO are called decarbonylation reactions. The decarbonylation of acetic acid proceeds as follows: CH3COOH(l)= CH3OH(g)+ CO(g. By using data from Appendix C in the textbook, calculate the minimum

  35. chemistry

    Determine if the following reaction is spontaneous under standard conditions. Zn(s) + 4 CN¡V(aq) + Ag2CrO4(s) „³ Zn(CN)42¡V(aq) + 2 Ag(s) + CrO42¡V(aq)

  36. 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

  37. chem

    Express the second law of thermodynamics as a mathematical equation. (Select all that apply.) For a reversible process, ÄSuniverse = 0. For a spontaneous process, ÄSuniverse > 0. For a spontaneous process, ÄSuniverse = 0. For a reversible process,

  38. Chemistry

    Spontaneous reactions ________. always release free energy*** always result in increase disorder of the system always take place at a rapid rate are always exothermic

  39. chem

    Can someone check this for me? Predict which reactions are spontaneous: a) Zn(s) + 2H+(aq) --> Zn+2(aq) + H2(g) b) CaCO3(s) + 2H2O(l) --> Ca(OH)2(s) + H2CO3(aq) c) CH4(g) + O2(g) --> CO2(g) + 2H2O(g) d) Ag+(aq) + Cl-(aq) --> AgCl(s) I said a) and c) were

  40. chemistry

    Under standard conditions for all concentrations, the following reaction is spontaneous at 25 ¢XC with EO = 0.16 V. + - 02 (g) + 4 H (aq) + 4 Br (aq) -+ 2 H20 (I) + 2 Br2 (1) If [H+] is a?justed by adding a buffer of 0.10 M NaOCN and 0.10 M HOCN (Ka = 3.5

  41. chemistry

    The G value for formation of gaseous water at 298 K and 1 atm is -278 kJ/mol. What is the nature of the spontaneity of formation of gaseous water at these conditions? A. The reaction is never spontaneous. B. The reaction is sometimes spontaneous. C. The

  42. Chemistry Check!

    1. Gibb's Free Energy is a. the spontaneous energy of a reaction *** b. the chemical energy that can be used for performing work c. the non-spontaneous energy of a reaction d. the amount of activation energy needed for a reaction to start 2. Which reaction

  43. Chemistry- Please help!!

    Using standard reduction potentials, calculate the standard E¡Æcell, emf, for each of the following reactions. State if each reaction is spontaneous or nonspontaneous. (Use the below reactions AS WRITTEN, DO NOT REARRANGE ANY REACTIONS.) You must show

  44. Chemistry

    the corrosion of iron is similar to the reactions that occur in an electrochemical cell. Oxidation and reduction occur at separate places on the metal and the circuit is completed by an electrolyte in solution one possible corrosion is Fe(s)+O2(g) + H2O(l)

  45. 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

  46. 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.

  47. Chemistry

    True or False: A non-spontaneous reaction is converted into a spontaneous reaction in a voltaic cell by the expense of electrical energy. I believe it is true because in a non spontaneous reaction, energy must be induced in order for it to occur. Is this

  48. chemistry

    calculate the theoretical potential of each of the following cells.is the cell reaction spontaneous as written or spontaneous in the oppsite direction? Bi|BiO+(0.04M),H+(0.2M)||I-(0.1M),AgI(sat`d)|Ag help meeeee

  49. 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

  50. Chemistry

    . In a biochemical reaction, A + B-->C with äG = 30 kJ/mol. Which of the following reactions might be effectively coupled to this reaction so that it becomes more spontaneous? I. C + D are the reactants, and B + E are the products äG = -40 kJ/mol II. C +

  51. 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

  52. 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

  53. Chemistry

    Consider the following reaction: CaCO3(s)→CaO(s)+CO2(g). Estimate ΔG∘ for this reaction at each of the following temperatures. (Assume that ΔH∘ and ΔS∘ do not change too much within the given temperature range.) A) 310K B) 1070K C) 1470K And is

  54. chemistry

    Suppose you have a reaction that has a ΔH of +80 kJ and a ΔS of 215 J/K. At what temperature will this reaction change from being not spontaneous to spontaneous? 31 C 99 C -18 C 25 C 53 C

  55. Chemistry

    An exothermic reaction is spontaneous above 400K but non spontaneous below it. Of the deltaH for the reaction is -40.0 kcal, what are the values of deltaS and deltaG at 400K?

  56. asap Chemistry

    Which ones are true? 1. Redox reactions are reactions where oxidation and reduction occur simultaneously. 2. Oxidation accurse at the cathode in a voltaic cell. 3. A voltaic cell is a cell that does not need a battery to run due to spontaneous chemical

  57. chemistry

    3HgO→2Hg+O2 Which of the following can definitely be concluded from the equation and heat of reaction above? A. The reaction is spontaneous. B. The reaction is non-spontaneous. C. The reaction is endothermic. D. The reaction is exothermic. E. None of

  58. Chemistry asap

    Using the activity series, either from the textbook (page 80) or your data sheets, determine whether the reactions given below would be spontaneous or not. JUSTIFY your answer in each case. a. Cu2+ (aq) + Au (s) → Au+ (aq) + Cu (s) b. Fe2+ (aq) + Al (s)

  59. Chemistry

    From your experience, predict which of the following reactions are spontaneous. a) Zn(s) + 2H+(aq)--> Zn+2(aq) + H2 (g) b) CaCO3(s) + 2H2O(l) --> Ca(OH)2(s) + H2CO3(aq) c) CH4(g) + O2(g) --> CO2(g) + 2H2O(g) d) Ag+(aq) + Cl-(aq) --> AgCl (s) Our book

  60. Chemistry

    Consider the following reaction at constant P. Use the information here to determine the value of ΔSsurr at 398 K. Predict whether or not this reaction will be spontaneous at this temperature. 4 NH3(g) + 3 O2(g) → 2 N2(g) + 6 H2O(g); ΔH = -1267 kJ

  61. chemistry

    Answer the questions by looking at the following reaction between nitrogen oxides. N2O(g) + NO2(g) → 3NO(g) (a) Find the values ​​of ΔH°, ΔS°, ΔG° (b) Assuming that ΔH° and ΔS° do not change with temperature, calculate ΔG° at 800 K. 800

  62. chemistry

    which of these reactions if spontaneous? (a) Fe^0 + Mg +2 --> Mg^0 +Fe+2 (b) Fe+2 + Mg ^0 --> Fe^0 + Mg +2 write the half cell equations for the spontaneous reaction. which element is oxidized and which is reduced?

  63. Chemistry

    What is meant by the directionality of a spontaneous reaction? I haven't heard of the term but I assume it means the direction in which a spontaneous reactions occurs.

  64. chemistry

    which of these reactions (a) or (b) is spontaneous? Explain why. write the half cell equations for the spontaneous reaction. Identify which element is oxidized and which is reduced. (a) Fe^0+Mg^+2 --> Mg^0 + Fe^+2 (b) Fe^+2 + Mg^0 --> Fe^0 + Mg^+2

  65. Chemistry

    under standard conditions, the following reaction is spontaneous at 298K. O2 + 4H+ + 4Br- --> 2H2O + 2 Br2 Will the reaction be spontaneous if the PH value is adjusted using a buffer composed of 0.10 M benzoic acid and 0.12M sodium benzoate? Given:Given:

  66. Chemistry

    Using G (measure of free energy) to determine wether the reaction 4Fe(s)+3O2(g)-> 2Fe2O3(s) is spontaneous at 25C, given that H=.393kcal and S=-0.13 kcal/(mol*K). Is the reaction more or less spontaneous at 1000C assuming that H and S remain constant with

  67. Chemistry

    Using standard reduction potentials, calculate the standard E¡Æcell, emf, for each of the following reactions. State if each reaction is spontaneous or nonspontaneous. (Use the below reactions AS WRITTEN, DO NOT REARRANGE ANY REACTIONS.) You must show

  68. college chemistry

    a) Is the reaction shown below spontaneous under standard conditions at 25⁰C? CH3OH (g) ----> CO (g) + 2H2 (g) b) Will this reaction be spontaneous at 25⁰C given the following amounts of materials? CH3OH at 1.20 atm CO at 0.080 atm H2 at 0.020 atm

  69. 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

  70. 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.

  71. Chemistry-Plz see this DrBob

    I am sorry I do not know what happens the symbolism, so I just deleted the symbols. Is it works for you that deleted the symbols? Using standard reduction potentials, calculate the standard Ecell, emf, for each of the following reactions. State if each

  72. Chemistry

    What causes a reaction to be spontaneous? Answer by answering each part a) (1 point) What is definition of spontaneous reaction?b) (1 point) What is Gibbs free energy?c) (1 point) How is Gibbs free energy related to a spontaneous reaction?d) (1 point) What

  73. Chemistry

    Please help me with these problems, the book examples very different. I'm really confused. Any help with these will help me immensely. Thank you in advance! What I got were: 1.)c 2.)d 3.)a 4.)c 5.)b 1.) When is any endothermic reaction spontaneous? a.)When

  74. Chemistry

    I have 2 questions. Can someone confirm my answers? 1.) Which of the following would almost always indicate a spontaneous reaction? A.) when a reaction requires the input of energy B.) if delta G is positive C.) when enthalpy is positive and entropy is

  75. chemestry

    I need serious help on this....please help guys.. i've to turn it in in an hours... Balance th following equation in acid Solutiong and determind if it is spontaneous under standard conditions. NO3^-1 + Sn^+2 ---> NO + Sn^+4 Please do not post duplicates.

  76. chemistry

    Which of the following reactions will be spontaneous at standard state? Not all the reactions are balanced, so make sure they are balanced first. The ΔG of formation data can be found in an appendix in your text book. You may select multiple answers. Any

  77. 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

  78. Chemistry

    What is the difference between a spontaneous and a non spontaneous reaction?

  79. Chem

    How do you predict when a reaction goes non-spontaneous if you have delta h Stotal and deltaS

  80. 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

  81. chemistry

    Predict wheter or not the following reaction will be spontaneous, please explain Br2(l) + Cl2(l) + 29.3 kJ --> 2 BrCl(g)

  82. Chemistry 152

    How many of the following processes would you expect to be spontaneous at 298K and 1atm? dissolving sugar in water decomposing NaCl to the elements climbing a mountain H2O (l)------H2(g)+O2(g) Choose one answer. a. 0 b. 1 c. 2 d. 3 e. 4 I thought that it

  83. chemistry

    If delta G (Gibbs) is positive and you are trying to find at what temperature the reaction is spontaneous would the formula be: T< H/S ? G=H-TS H-TS>0 T< H/S then the temperature found would be the temp at which the reaction is spontaneous?

  84. Chemistry help

    Sulfur trioxide is formed by the catalytic oxidation of sulfur dioxide: 2SO2(g)+O2(g)→2SO3(g) If ΔH∘= -197.8kJ/mol and ΔS∘= -188.0J/K , what is ΔStotal for this reaction? Is the reaction spontaneous under standard-state conditions at 25 ∘C?

  85. Biochemistry

    Is the substrate level phosphorylation (of succinate) spontaneous under conditions that exist in the mitochondria?

  86. chemistry

    For the reaction H2(g) +S(s)->H2S(s), Triangle H= -20.2 kJ and triangle S= 43.1 J/K. WHen will the reaction be spontaneous? I know that it has to be negative to be spontaneous but i don't exactly know how to answer this question.

  87. Chemistry

    When it comes to something being spontaneous, what does it mean? I know its something that goes out without no outside force or something like that but what are example of something that is spontaneous ?

  88. chemistry

    Please help!! Predict whether N2(g) + 3H2(g) ⇌ 2NH3(g) is spontaneous at 773.15 K. Assume: ∆H = -92.22 kJ and ∆S = -198.75 J/mol·K. Describe all components. Show work please!!

  89. chemistry

    is this true or false? i think its false because isnt it spontaneous if its positive When (triangle i think its called delta) H for a reaction is large and positive, the reaction is not expected to be spontaneous.

  90. AP Chemistry

    I am honestly lost on this question and you can't proceed without solving the first on, so if anyone would be so inclines to help me out Aluminum metal reacts with zinc(II) ion in an aqueous solution by the following half-cell reactions: Al(s) → Al3+(aq)

  91. Thermodynamics

    Sodium carbonate can be made by heating sodium bicarbonate: 2NaHCO3(s) ¨ Na2CO3(s) + CO2(g) + H2O(g) Given that ƒ¢H‹ = 128.9 kJ/mol and ƒ¢G‹ = 33.1 kJ/mol at 25‹C, above what minimum temperature will the reaction become spontaneous under

  92. Chemistry

    Using the following spontaneous reactions, classify the 3 metals involved (Cr, Sn, Al) according to increasing reductant properties. a) 2Cr + 3Sn2+ 2Cr3+ + 3Sn b) Al + Cr3+ Al3+ + Cr

  93. HELP HARD CHEM. QUESTION!

    Using the following spontaneous reactions, classify the 3 metals involved (Cr, Sn, Al) according to increasing reductant properties. a)2Cr + 3Sn2+ ->2Cr3+ + 3Sn b)Al + Cr3+ -> Al3+ + Cr

  94. electrochemistry gr 12

    Using the following spontaneous reactions, classify the 3 metals involved (Cr, Sn, Al) according to increasing reductant properties. a) 2Cr + 3Sn2+ ----> 2Cr3+ + 3Sn b) Al + Cr3+ ----> Al3+ + Cr

  95. Chemistry

    SOMEONE PLSS HELP . Using the following spontaneous reactions, classify the 3 metals involved (Cr, Sn, Al) according to increasing reductant properties. a) 2Cr + 3Sn2+ ----> 2Cr3+ + 3Sn b) Al + Cr3+ ---> Al3+ + Cr

  96. 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

  97. 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.

  98. biology (check answers)

    1. How do endothermic and exothermic reactions differ? a. Endothermic reactions release energy and are spontaneous. b. Exothermic reactions release energy and are spontaneous. c. Endothermic reactions give off heat and light. d. Photosynthesis is

  99. biology (check answers)

    1. How do endothermic and exothermic reactions differ? a. Endothermic reactions release energy and are spontaneous. b. Exothermic reactions release energy and are spontaneous. c. Endothermic reactions give off heat and light. d. Photosynthesis is

  100. Chemistry

    Which of the following is NOT a spontaneous reaction? a. Ice melting at 25 °C under atmospheric pressure b. Water freezing at 25 °C under atmospheric pressure c. Two gases mixing in the same container d. A gas expanding into a larger volume container e.

Pages

  1. 1
  2. 2
  3. 3
  4. 4
  5. 5
  6. 6
  7. 7
  8. 8
  9. 9
  10. 10
  11. 11
  12. 12
  13. 13
  14. 14
  15. 15
  16. 16
  17. 17
  18. 18
  19. 19
  20. 20