Sketch potential energy curves for the ground and excited states showing events leading to phosphoresce. Use arrows to label all necessary transitions and answer the following:

A) Based on your picture does phosphoresce occur at lower or higher wavelength relative to the absorption wavelength?

B) Would you expect 0-0 transition for absorption and phosphorescence to be coincident?

Can someone please explain the acid cleavage reaction in detail? I know it's SN2 if its a primary or secondary, and the less hindered carbon is attacked. I know SN1 occurs if a carbon is tertiary, but I don't know how these reactions look. Please help!

When 24.0 mL of 0.600 M H2SO4 is added to 24.0 mL of 1.20 M KOH in a coffee-cup calorimeter at 23.50°C, the temperature rises to 30.17°C. Calculate H of this reaction per mole of H2SO4 and KOH reacted. (Assume that the total volume is the sum of the individual volumes and that the density and specific heat capacity of the solution are the same as for pure water: d = 1.00 g/mL and c = 4.184 J/g×K.) H per mole of H2SO4 reacted:

___ kJ/mol

H per mole of KOH reacted:

___kJ/mol

Calculate the percentage composition, by weight, in terms of the constituent oxides of the following minerals. Constituent oxides are SiO2, Al2O3, TiO2, FeO, MgO, Na2O, K2O, CaO, H2O, etc. Also, write a balanced chemical equation for each mineral.

a. Ilmenite {FeTiO3}

b. Muscovite {KAl2(AlSi3O10)(OH)2}

c. Plagioclase feldspar (albite) {NaAlSi3O8}

d. Magnetite {Fe3O4}

e. Olivine {(Mg,Fe)2SiO4 - assume equal proportions of Mg and Fe}

Calculate the pH in the titration of 20 mL of 0.125 M HCL with 0.250 M NaOH solution after adding 9.60 mL and 10.40 mL of NaOH

Using Silica or Alumina in packing the column results in “Normal” chromatography. What is reversed-phase chromatography and why is it useful?

When grape juice is fermented, glucose (C6H12O6) is converted to ethanol (C2H6O) and carbon dioxide. Please show work.

a.) Write a balanced chemical equation for the reaction. (There are not any other reactants or products.)

   C6H12O6 -> C2H6O + CO2     is this correct?

b.) How many grams of glucose are needed to form 150 g of ethanol?

c.) If a grape juice sample dontains 4.50 kg of glucose, how manu grams of ethanol can be produced?

d.) How many milligrams of carbon dioxide can be produced from 0.778 g of glucose?

An enzymatic reaction takes place in a 10 ml solution that has a total citrate (plus citric acid) concentration of 120 mM and an initial pH of 7.00. During the reaction 0.2 millimoles of H+ are produced. The relevant pKa of citric acid is 6.40. A) Calculate the final pH of the solution. B) What would the final pH of the solution be if the citrate were absent from the solution and no other buffering agents were present (assuming a starting pH of 7.00 again, basically, what would be the pH is you added the same amount of acid to that amount of water)?

In a titration of a 250mL solution of 0.05M ammonia (NH3) (Kb=1.8 * 10^-5) with a concentrated (0.2M) solution of HCL, calculate the following:

1. What is the initial pH before adding HCL?

2. What is the pH of the system after adding 20mL of the 0.2 M HCL?

3. What is the pH at equivalence?

*I have the answers, I really need to know how to do the work to get to the answers.*

The diffusion coefficients for species A in metal B are given at two temperatures: T (°C) D (m2/s) 1040 6.22 × 10-17 1280 6.11× 10-16 (a) Determine the value of the activation energy Qd (in J/mol). Entry field with incorrect answer 1.04e5 J/mol (b) Determine the value of D0. Entry field with incorrect answer 3.71e-22 m2/s (Use scientific notation.) (c) What is the magnitude of D at 1160°C? Entry field with incorrect answer 3.69e-18 m2/s (Use scientific notation.)

12.      Predict the direction of the equilibrium shift when temperature is decreased in the following reactions:

a.         C₂H₂ (g) + H₂O (g) ? CH₃CHO (g)      [?H = -151 kJ/mol]

b.         CH₃CH₂OH (l) + O₂ (g) ? CH₃CH₂O (g) + H₂O (g)      [?H = exothermic]

c.         2 CH₃CHO (g) ? 2 C₂H₄ (g) + O₂ (g)      [?H = endothermic]

13.            Consider the following endothermic reaction for the production of hydrogen gas in a rigid container:

CH₄(g) + H₂O(g) ? CO(g) + 3 H₂(g)

How will the yield of hydrogen change if the equilibrium is disturbed by:

a.         Adding a catalyst.

b.         Increasing the pressure.

c.         Decreasing the temperature.

d.         Adding inert argon gas.

e.         Increasing the temperature.

Electrochemistry - Standart Potential

1. For the voltaic cell shown, calculate the E^o_cell.

Hg(l), Hg₂Cl₂(s) l Cl^-(aq) ll Cu²⁺(aq), Cu⁺(aq) l Pt(s)

2. Calculate the standard emf for a voltaic cell whose cell reaction is represented by the balanced equation.

Pb(s) + Zn²⁺(aq) → Pb²⁺(aq) + Zn(s)

3. For the galvanic cell shown, calculate the E^o.

Au(s) l AuCl₄^-(aq), Cl^-(aq) ll F₂(g) l F^-(aq) l Pt(s)

Vitamin B12 was used in a column chromatography experiment as a marker to show when all of the protein had eluted off the column. Will vitamin B12 show up on the SDS-PAGE? Explain.

A 29.6 mL sample of 0.260 M diethylamine, (C₂H₅)₂NH, is titrated with 0.338 M hydrochloric acid.

After adding 33.7 mL of hydrochloric acid, the pH is

.

Use the Tables link in the References for any equilibrium constants that are required.