NAD^+(aq)+2H^+(aq)+2e^- --> NADH(aq)+H^+(aq) E= -0.320V

Oaloacetate^2-(aq)+2H^+(aq)+2e^- --> malate^2-(aq) E= -0.166V

a. Calculate the standard potential for the following reaction: Oxaloacetate^2- (aq) +NADH(aq)+H^+(aq) --> malate-(aq)+NAD^+(aq)

b. Calculate the equilibrium constant for the reaction at 298K

The Na –glucose symport system of intestinal epithelial cells couples the \"downhill\" transport of two Na ions into the cell to the \"uphill\" transport of glucose, pumping glucose into the cell against its concentration gradient. If the Na concentration outside the cell ([Na ]out) is 163 mM and that inside the cell ([Na ]in) is 23.0 mM, and the cell potential is -51.0 mV (inside negative), calculate the maximum ratio of [glucose]in to [glucose]out that could theoretically be produced if the energy coupling were 100% efficient. Assume the temperature is 37 °C.

If the same volume of the buffer were 0.265 M in NH3 and 0.390 M in NH4Br, what mass of HCl could be handled before the pH fell below 9.00?

Two sig. figs.

m= ?

For a molecule of fluorous acid, the atoms are arranged as HOFO. (Note: In this oxyacid, the placement of fluorine is an exception to the rule of putting the more electronegative atom in a terminal position.) What is the formal charge on each of the atoms? Enter the formal charges in the same order as the atoms are listed. Express your answers as charges separated by comma. For example, a positive one charge would be written as +1.

Discuss the difference of the following sample preparation: (a) Liquid-liquid extraction (LLE) (b) Soxhlet extraction (c) Solid phase extraction (SPE) in terms of application, cost, extraction time, solvent usage.

1.) Determine the energy change (in Joules) associated with the transition from n=2 to n=4 in the Hydrogen atom.

2.) Calculate the wavelength (in nm) of the red line in the visible spectrum of excited H atoms using Bohr Theory.

3.) What is the energy (in Joules) of the X-ray radiation at 2.00x10^-10 m that are used for medical diagnosis?

4.) What is the binding energy of an electron in a photosensitive metal (in kj/mol) if the minimum frequency of light that can eject electrons from the metal is 6.3x10^14 Hz?

5.) How many photons are contained in a burst of yellow light (589nm) for a sodium lamp that contains 609 kJ of energy?

Which of the following hydrocarbons is expected to be the most reactive in ethanloic silver nitrate? Why? Write the organic product that you expect when your chosen substrate reacts.

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Draw the conjugate acid of compound A. Explain you choice.

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Provide a mechanism. Include all intermediates. Show all electron pushing.

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A sample contains a mixture of ²³⁹Pu and ²⁴⁰Pu in unknown proportions. The activity of the mixed sample was found to be 4.35 x 10⁷ dpm for a sample of 0.125 mg of Pu. Calculate the weight % of each Pu isotope present

53. Which of the following is an acid-base reaction? Select the best answer.

   (A). C(s) + O2(g)  CO2(g)

   (B). 2HClO4(aq) + Ca(OH)2(aq) 2H2O(l) + Ca(ClO4)2(aq)

   (C). Fe(s) + 2AgNO3(aq)  2Ag(s) + Fe(NO3)2(aq)

   (D). MgSO4(aq) + Ba(NO3)2(aq)  Mg(NO3)2(aq) + BaSO4(s)

   (E). All of the above are acid base reactions.

54. Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of K2S and Fe(NO3)2 are mixed.

   (A). Fe2+(aq) + S2-(aq)  FeS(s)

   (B). Fe2+(aq) + S2-(aq) + 2K+(aq) + 2NO3-(aq)  FeS(s) + 2K+(aq) + 2NO3-(aq)

   (C). K+(aq) + NO3-(aq)  KNO3(s)

   (D). Fe2+(aq) + S2-(aq) + 2K+(aq) + 2NO3-(aq)  Fe2+(aq) + S2-(aq) + 2KNO3(s)

55. According to the following reaction, what mass of PbCl2 can form from 422 mL of 0.110M KCl solution? Assume that there is excess Pb(NO3)2.

2KCl(aq) + Pb(NO3)2(aq)  PbCl2(s) + 2KNO3(aq) (balanced ?)

   (A). 7.19 g

   (B). 3.59 g

   (C). 6.45 g

   (D). 5.94 g

   (E). 1.30 g

56. When 10.00 moles of H2(g) react with 5.000 moles of O2(g) to form 10.00 moles of H2O(l) at 25°C and a constant pressure of 1.00 atm. If 683.0 kJ of heat are released during this reaction, and PΔV is equal to -37.00 kJ, then

   (A). ΔH° = -683.0 kJ and ΔE° = -646.0 kJ.

   (B). ΔH° = -683.0 kJ and ΔE° = -720.0 kJ.

   (C). ΔH° = +683.0 kJ and ΔE° = +720.0 kJ.

   (D). ΔH° = +683.0 kJ and ΔE° = +646.0 kJ.

57. Determine the molarity of a solution formed by dissolving 97.7 g LiBr in enough water to yield 750.0 mL of solution.

   (A). 0.130 M

   (B). 0.768 M

   (C). 2.30 M

   (D). 1.50 M

   (E). 1.18 M

59. Which one of the following compounds is(/are) soluble in water? Select all that apply.

   (A). Ca3(PO4)2

   (B). HgS

   (C). Ni(NO3)2

   (D). MgCO3

*** 8 Parts*** Write the equilibrium equation for the following reactions, and tell whether the reactants or products are favored in each case.

a) 2 CO(g) + O2(g) -------> 2 CO2(g) Keq = 2 x 10^11

b) Cl2O(g) + H2O(g) ------> 2 HOCl(g) Keq = 0.132

c) HF(aq) + H2O(l) ------> H3O+(aq) + F-(aq) Keq = 7.1 x 10^-4 

d) 3 O2(g) -----> 2 O3(g) Keq = 2.5 x 10^-29

e) S2(g) + 2 H2(g) -------> 2 H2S(g) Keq = 2.8 x 10^-21

f) CO(g) + 2 H2(g) -------> CH3OH(g) Keq = 10.5

g) Br2(g) + Cl2(g) ---------> 2 BrCl(g) Keq = 58.0

h) I2(g) -------> 2I(g) Keq = 6.8 x 10^-3

Determine the Reaction Order for HCl using calculations described in the Background section. Show your work. Note that your answer will probably not be an even whole number as it is in the examples, so round to the nearest whole number.

B.    Determine the Reaction Order for Na₂S₂O₃ using calculations described in the Background section. Show your work. Note that your answer will probably not be an even whole number as it is in the examples.

41. When 0.500 g of cyclohexane, C6H12, is combusted in a bomb calorimeter that has a water sheath containing 750.0 g of water, the temperature of the water increased by 5.5 °C. Assuming that the specific heat of water is 4.18 J/(g °C), and that the heat absorption by the calorimeter is negligible, calculate the enthalpy of combustion per mole of cyclohexane.

   (A). 2.90 x 106 J/mol

   (B). 4.20 x 106 J/mol

   (C). 1.19 x 104 J/mol

   (D). 2.97 x 105 J/mol

   (E). 8.21 x 106 J/mol

42. Choose the reaction that illustrates ΔH°f for Ca(NO3)2.

   (A). Ca(s) + N2(g) + 3O2(g)  Ca(NO3)2 (s)

   (B). Ca+(aq) + NO3-(aq)  Ca(NO3)2 (s)

   (C). Ca+(s) + NO3(aq)  Ca(NO3)2 (s)

   (D). Ca(s) + N2(g) + O2(g)  Ca(NO3)2 (s)

   (E). 2Ca(s) + 2N2(g) + 3O2(g)  Ca(NO3)2 (s)

45. Give the equation with the elements in Na2SO4 in their standard state as the reactants and Na2SO4 as the product.

   (A). 2 Na(s) + 1/8 S8 (s, rhombic) + 2 O2(g)  Na2SO4

   (B). Na(s) + S8 (s, rhombic) + 2 O2(g)  Na2SO4

   (C). Na(s) + S (s, rhombic) + ½ O2(g)  NaSO

   (D). Na(s) + 1/8 S8 (s, rhombic) + 2O2(g)  NaSO4

46. A gas cylinder contains 10.0 kg of C3H8 (propane) gas. Calculate the heat associated with the complete combustion of all of the propane in the cylinder. MW of C3H8 is 44.10 g/mol.

C3H8(g) + 5O2(g)  3CO2(g) + 4H2O(g) Δrxn = -2044 kJ

   (A). -5.68 x 105 kJ

   (B). -4.63 x 105 kJ

   (C). +5.68 x 105 kJ

   (D). +4.63 x 105 kJ

   (E). 2.31 x 105 kJ

48. Use the Δof information provided to calculate Δorxn for the following reaction:

SO2Cl2(g) + 2H2O(l)  2HCl(g) + H2SO4(l) Δorxn = ?

Δof (kJ/mol)

SO2Cl2(g) -364

H2O(l) -286

HCl(g) -92

H2SO4(l) -814

49. Calculate the change in internal energy (Δ) for a system that is giving off 26.0 kJ of heat and is changing from 12.00 L to 6.00 L in volume at 1.50 atm pressure. (101.3 J = 1 L∙tm)

50. Use bond energies to calculate the Δrxn for the following reaction:

N2(g) + 3H2(g)  2NH3(g) (balanced?)

51. Which of the following (with specific heat capacity provided) would show the smallest temperature change upon gaining 155 J of heat?

   (A) 25.0 g Au, CAu = 0.128 J/g.°C

   (B) 25.0 g Ag, CAg = 0.235 J/g.°C

   (C) 50.0 g Al, CAl = 0.903 J/g.°C

   (D) 50.0 g Cu, CCu = 0.385 J/g.°C

   (E) 25.0 g granite, Cgranite = 0.790 J/g°C

52. Use the standard reaction enthalpies given below to determine ΔHorxn for the following reaction:

2 NO(g) + O2(g)  2 NO2(g) Δorxn = ?

Given:

N2(g) + O2(g)  2 NO(g) Δorxn = +183 kJ

½ N2(g) + O2(g)  NO2(g) Δorxn = +33 kJ

   (A) -211 kJ

   (B) -117 kJ

   (C) -153 kJ

   (D) +165 kJ

   (E) +795 kJ

What is the [H3O + ] concentration of a solution formed by mixing 50.0 mL of 0.20 M HCl and 50.0 mL of 0.10 M NaOH?

Given 100.0 mL of a buffer that is 0.50 M in HOCl and 0.40 M in NaOCl, what is the pH after 10.0 mL of 1.0 M NaOH has been added? (Ka for HOCl = 3.5  108 ).

What is the pH of a solution prepared by mixing 50 mL of a 0.10 M solution of HF with 25 mL of a 0.20 M solution of NaF? (The pKa of HF is 3.14.)

The chief compound in marble is CaCO3. Marble has been widely used for statues and ornamental work on buildings, including such structures as the Taj Mahal. However, marble is readily attacked by acids via the following reaction.

CaCO₃(s)+H⁺(aq)⇌Ca²⁺(aq)+HCO₃⁻(aq)

Equilibrium constants at 25 ^∘C are listed in the table below.

What is the molar solubility of marble (i.e., [Ca²⁺] in a saturated solution) in normal rainwater, for which pH=4.20?

In the simulation, select the Table Salt tab, and set the volume and the total number of sodium (Na+) ions as mentioned below. Allow the solution to attain equilibrium. Observe the number of dissolved ions and bound ions from the table displayed on the right. Then, identify which of the following solutions are saturated solutions.

1.0×10−23 L of solution containing 23 Na+ ions.

2.0×10−23 L of solution containing 81 Na+ ions.

3.0×10−23 L of solution containing 115 Na+ ions.

4.0×10−23 L of solution containing 121 Na+ ions.

5.0×10−23 L of solution containing 202 Na+ ions.

6.0×10−23 L of solution containing 213 Na+ ions.