You have a cold gas of gold atoms, and you observe that if you shine light consisting of photons with energy 10.2 eV through the gas, some free electrons are observed, implying that a photon of this energy is able to ionize an atom in the gas. You find that the emitted electrons have a kinetic energy of 1.0 eV. What is the ionization energy of the gold atom? What is its ground state energy K + U?

you shine light with continuous energy distribution, and you observe absorption lines at the following photon energies: 1.1 eV, 2.7 eV, 4.6 eV, 5.1eV, 6.7eV, and 7.2eV.

Q/ Using the information from the two experiments describes above, draw a diagram of the energy levelsof one of the atoms in this gas. Draw the diagram expermintly to scale. Label the energy levels with their Values and label the transitions observed from the absorption line Data.

Rewrite the net ionic reaction. If there is NO reaction, simply write NR.

1) (CuSO₄ + NaOH)

2) (AlCl₃ + NaOH)

3) (Zn(C₂H₃O₂)₂ + NaOH)

4) (Pb(NO₃)₂ + NaOH)

5) (Na₃PO₄ + NaOH)

6) (AlCl₃ + Na₃PO₄)

7) (CuSO₄ + Na₃PO₄)

8) (Zn(C₂H₃O₂)₂ + Na₃PO₄)

Which compound is likely to have an incomplete octet? H2S PH3 NO SF6

Rewrite the net ionic reaction. If there is NO reaction, simply write NR.

1) (Na₂CO₃ + Kl)

2) (AgNO₃ + Kl)

3) (CuSO₄ + AgNO₃)

4) (AlCl₃ + AgNO₃)

5) (Zn(C₂H₃O₂)₂ + AgNO₃)

6) (Pb(NO₃)₂ + AgNO₃)

7) (Na₃PO₄ + AgNO₃)

When 15.0 mL of a 7.02×10-4 M ammonium fluoride solution is combined with 22.0 mL of a 9.63×10-4 M magnesium sulfate solution does a precipitate form? (yes or no) For these conditions the Reaction Quotient, Q, is equal to

The literature value for the Ksp of Ca(OH)₂ at 25 °C is 4.68E−6. Imagine you ran the experiment and got a calculated value for Ksp which was too high. Select all of the possible circumstances which would cause this result.

A. The HCl was more concentrated than the labeled molarity (0.0500 M).

B. The Ca[OH]₂ solution may have been supersaturated.

C. The HCl was less concentrated than the labeled molarity (0.0500 M).

D. The Ca[OH]₂ solution may have been unsaturated.

E. The titration flask may have not been clean and had a residue of a basic solution.

F. The titration flask may have not been clean and had a residue of an acidic solution.

Please show all work

A.)Place the following in order of decreasing standard molar entropy.

NaCl(s) Na₃PO₄(aq) NaCl(aq)

B.)Calculate the ΔG°_rxn using the following information.

ΔG°_rxn = ?

C.)Calculate the ΔG∘rxn for the reaction using the following information.

4HNO3(g)+5N2H4(l)→7N2(g)+12H2O(l)

ΔG∘f(HNO3(g)) = -73.5 kJ/mol;
ΔG∘f(N2H4(l)) = 149.3 kJ/mol;
ΔG∘f(N2(g)) = 0 kJ/mol;
ΔG∘f(H2O(l)) = -273.1 kJ/mol.

1. Describe the meaning of the molecular equation between the NaOH and HCl solutions on the microscopic and macroscopic scales.
2. Provide a detailed description for titrating the calculated volume of HCl solution with the 0.3 M NaOH solution. Make sure to describe what equipment you would use, how it is used and which characteristics of the equipment make them suitable for this purpose.
3. Consider the properties of HCl solutions. Identify reasons why it needs to be titrated to determine its actual concentration.

A solution of an unknown acid is prepared by dissolving 0.250 g of the unknown in water to produce a total volume of 100.0 mL. Half of this solution is titrated to a phenolphthalein endpoint, requiring 12.2 mL of 0.0988 M KOH solution. The titrated solution is re-combined with the other half of the un-titrated acid and the pH of the resulting solution is measured to be 4.02. What is are the Ka value for the acid and the molar mass of the acid?

Which of the subshell designations are possible and which are impossible?

PossibleImpossible

4f

2d

4d

1p

3f

Answer Bank

A 0.4592 g sample of pewter, containing tin, lead, copper, and zinc, was dissolved in acid. Tin was precipitated as SnO 2 ⋅ 4 H 2 O and removed by filtration. The resulting filtrate and washings were diluted to a total volume of 200.0 mL. A 15.00 mL aliquot of this solution was buffered, and titration of the lead, copper, and zinc in solution required 34.07 mL of 0.001476 M EDTA . Thiosulfate was used to mask the copper in a second 20.00 mL aliquot. Titration of the lead and zinc in this aliquot required 33.13 mL of the 0.001476 M EDTA solution. Finally, cyanide was used to mask the copper and the zinc in a third 25.00 mL aliquot. Titration of the lead in this aliquot required 25.11 mL of the 0.001476 M EDTA solution. Determine the percent composition by mass of each metal in the pewter sample.

Cu = ____% Zn= ____% Pb= ____% Sn= ____%

Assume a titration with 0.100 M NaOH titrant and 25.00 mL of a 0.0800 M CH3COOH analyte. What will the pH of the analyte be if 10.00 mL of NaOH is added?

KClO₃ disproportionates on heating to give KCl and KClO₄ only. The number of moles of KClO₄ produced on complete disproportionation of 24.5 g KClO₃ is

• A. 0.156
• B. 0.106
• C. 0.126
• D. 0.206
• E. 0.056