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

Predict the sign of the entropy change for each of the following processes and give your reasoning why:

1. Solid sugar is added to water to form a solution.

2. Iodine vapor condenses on a cold surface to form crystals.

3. N₂(g) + 3H₂ (g) 2 NH₃(g)

4. H₂O(l) H₂O(g)

5. CaCO₃(s) CaO(s) + CO₂(g)

6. NH₄NO₃(s) + H₂O(l) NH₄⁺ (aq) + NO₃^- (aq)

7. freezing of water   

8. boiling of water

9. crystallization of salt from a supersaturated solution

10. the reaction 2 NO(g) → N2O2(g)

11. the reaction 2 H2(g) + O2(g) → 2 H2O(g)

12. Fe(s) → Fe(l)   

13. 2 Fe(s) + 3/2 O2(g) → Fe2O3(s)   

14. HF(l) → HF(g)

15. 2 H2O2(l) → 2 H2O(l) + O2(g)

16. H2O(l) -> 2 H2(g) + O2(g)

17. CO_(g) + 3 H_2(g)-> CH_4(g) + H₂O_(g)

18. 2 NaHCO_3(s) ---> Na₂CO_3(s) + H₂O_(g) + CO_2(g)

19. CO(g) + H₂O(g) ----> CO₂(g) + H₂(g)

20. CaCO₃(s) ----> CaO(s) + CO₂(g)

21. 2NH₃(g) + CO₂(g) ----> NH₂CONH₂(aq) + H₂O(l)

22. 2Na₂O₂(s) + 2H₂O(l) ---> 4NaOH(aq) + O₂(g)

23. C₂H₅OH(l) + 3O₂(g) ---> 2CO₂(g) + 3H₂O(g)

Plz let me know how you did it.

Simple description is the best

Thanks

Calculate E?cell for each of the following balanced redox reactions.

A. O2(g)+2H2O(l)+4Ag(s)?4OH?(aq)+4Ag+(aq)

B. Br2(l)+2I?(aq)?2Br?(aq)+I2(s)

C. PbO2(s)+4H+(aq)+Sn(s)?Pb2+(aq)+2H2O(l)+Sn2+(aq)

D. Determine whether the reaction in part A is spontaneous as written.

E. Determine whether the reaction in part B is spontaneous as written.

F. Determine whether the reaction in part C is spontaneous as written.

Using standard Gibbs energy of formation values given in the table, calculate the equilibrium constant K of the reaction

Cl2_(g)+2NO_(g)⇌2NOCl_(g)

The standard Gibbs energy change of the reaction represents the drive the reaction has under standard conditions to move toward equilibrium from point A to point X in the diagram.

Nitrogen gas is compressed isothermally at 250K from 1.0 bar to 150 bars. Determine the change in enthalpy and entropy using:
a. Redlich-Kwong equation of state
b. Using tabular superheat data

nstant cold packs sometimes used to treat athletic injuries contain solid ammonium nitrate and liquid water separatedbya thin divider. When the divider is broken, the ammonium nitrate dissolves endothermically:

NH4NO3(s) NH4+(aq) + NO3–(aq)

To measure the enthalpy of this reaction, you dissolve 1.25 g of ammonium nitrate in enough water to make 25.0 mL of solution. The initial temperature is 25.8 °C, and the final temperature is 21.9 °C. (Assume that the density of the solution is 1.00 g /mL and that the heat capacity of the solution is 4.184 J/g∙°C