For a particle of mass m in a two-dimensional potential well(i.e. particle confined in a 2D box) with sides L1 and L2:
a) Set up the Schrödinger equation for this system.
b) Using separation of variables, derive an expression for thewavefunction
Ψ and for the energy levels of the system. Be sure toshow all of your work for this derivation.
c) For the case of square potential well with side L (i.e.L₁=L₂=L), sketch an energy level diagram forthe nine lowest energy levels, showing degeneracy whereappropriate.

It requires substantial energy to reduce metal ore to pure metal. The reverse process, corrosion, happens spontaneously. The rusting of iron, the tarnishing of silver, and the formation of patina on copper and brass are some common examples of corrosion.

Rusting is the greatest corrosion problem because it occurs rapidly and because so many objects are made of iron and steel. A great deal of the annual production of iron goes simply to replace that lost by rusting. Iron will not rust in dry air or in water that is completely free of air. Oxygen gas and water must be present for iron to rust. Describe chemistry and electrochemistry of corrosion of iron and copper. In each redox reaction, specify the element that is being oxidized, the element that is being reduced, and identify the oxidizing and the reducing agent. Why cars rust more rapidly near the beach or in cold climate where salt is used to de-ice the roads?

Please show all work!

Balance the following reactions in an acidic solution:

Cr2O7^2-(aq)+HNO2(aq)--->Cr^3+(aq)+ NO3-(aq)

Pb^2(aq)+ IO3-(aq)--->PbO2(aq)+I2(aq)

Both AgCl and AgI are very sparingly soluble salts, but the solubility of AgI is much less than that of AgCl, as can be seen by their Ksp values. Suppose that a solution contains both Cl− and I− with [Cl−] = 0.046 M and [I−] = 0.047 M. If solid AgNO3 is added to 2.22 L of this mixture (so that no appreciable change in volume occurs), what is the value of [I−] when AgCl first begins to precipitate?

7. Choose the bond that is least polar (how would you do this without looking at an electronegativity chart)

a. P-F

b. C-F

c. C-Cl

d. C-Br

e. C-I

8. Using periodic trends, place the following in order of increasing ionic character.( Please explain)

Si-P, Si-Cl,Si-S

9. How do you calculate the bond order of resonance structures (Please explain.)

Using the following reduction potentials:

I₂(s) + 2e^- <---> 2I^-(aq) E⁰ = 0.535 V

I₂ (aq) +2e^- <---> 2I^-(aq) E⁰ = 0.620 V

I₃^-(aq) + 2e^- <---> 3I^-(aq) E⁰ = 0.535 V

a) Calculate the equilibrium constant for I₂(aq) + I^-(aq) <---> I₃^-(aq)

b) Calculate the equilibrium constant for I₂(s) + I^-(aq) <---> I₃^-(aq)

c) Calculate the solubility (g/L) of I₂(s) in water.

A 0.025 M solution of hydroxylamine has a pH of 9.11. What is the value of Kb for this weak base?

H2?NOH(aq)+H2O(?)?H3?NOH+(aq)+OH-(aq)

In the second row of the transition metals there are five elements that do not follow the normal orbital filling. Five - Nb, Mo, Ru, Rh, and Ag-result in a [Kr] 5s14dx configuration and Pd results in a [Kr] 4d10 configuration. Write the ground state electron configuration for the following species.

Ag

Ag+

Ru

Ru3+

Rh

Rh2+

Pd

Pd+

Pd2+

At 1 atm, how much energy is required to heat 89.0 g H 2 O ( s ) at − 24.0 ∘ C to H 2 O ( g ) at 115.0 ∘ C? Use the heat transfer constants found in this table.

q = kJ

Potassium dichromate is used in breathalyzers to measure alcohol content. The balanced chemical equation for the reaction between ethanol and potassium dichromate is given below.

3CH3CH2OH (aq) + 2K2Cr2O7 (aq) + 8H2SO4 (aq) --> 3CH3COOH (aq) + 2Cr2(SO4)3 (aq) + 2K2SO4 (aq) + 11H2O (l)

a. what is the oxidation state of Cr is Kr2Cr2O7?

b. what is the oxidation state of Cr in Cr2(SO4)3

c. Is Cr oxidized or reduced in the reaction? Explain.

Question 1.) Given the following data:

C2H2(g) + 5/2 O2(g) à2CO2(g) + H2O(l)      ΔH= -1300.kJ

C(s) + O2(g) àCO2(g)                                   ΔH= -394kJ

H2(g) + O2(g) à H2O(l)                                 ΔH= -286kJ

Use Hess’s Law to calculate ΔH for the reaction

2C(s) + H2(g) àC2H2(g)

Question 2.) Calculate ΔH° for each of the following reactions using the data for the enthalpy of

formation in the appendix.

2Na(s) + 2H2O(l)à2NaOH(aq) + H2(g

Thermophilic bacterium can convert glucose (C6H12O6) to ethanol and acetic acid .

1) Calculate the reaction enthalpy ΔrH when 1 mol of glucose is oxidized to ethanol at 80∘C.
C6H12O6(s)→2C2H5OH(l)+2CO2(g)

2) Calculate the reaction enthalpy ΔrH when 1 mol of glucose is oxidized to acetic acid at 80∘C.
2O2(g)+C6H12O6(s)→2CH3COOH(l)+2CO2(g)+2H2O(l)

For the reaction 2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g). E∘=0.483 V what is the cell potential at 25 ∘C if the concentrations are [Co3+]= 0.222 M , [Co2+]= 0.275 M , and [Cl−]= 0.309 M and the pressure of Cl2 is PCl2= 3.80 atm ?