Consider the following equilibrium: Fe(OH)₃(s) D Fe³⁺(aq) + 3OH^–(aq) with K_sp = 1.6 x 10^-39. The activity coefficients for Fe³⁺(aq) and 3OH^–(aq) are 0.445 and 0.900 in a solution with an ionic strength of 0.01M. The pH of the solution was 11.

a. Calculate [OH^–] in the solution.

b. Use the activity coefficients in order to calculate [Fe³⁺] in the solution.

Hydrogen gas can be produced by the reaction of iron metal with steam, as shown in the equation below:

3 Fe (s) + 4 H2O (g) à Fe3O4 (s) + 4 H2 (g)

If 40.00 g of iron are combined with 40.00 g of steam and reacted, calculate (i) how many grams of hydrogen gas will be formed and (ii) how many grams of the excess reagent will remain after the end of the reaction.

Mix the watery environment of Elodea with a pH indicator called phenol red. In the presence of an acid, phenol red will appear yellow. In the presence of a strong base, phenol red will appear purple. Intermediate colors correspond with intermediate pH values. Recall that plants use CO₂ for photosynthesis; the concentration of CO₂ will determine the pH of a solution. Plants also produce CO₂ as a byproduct of cellular respiration.

1. Will a solution with a high concentration of CO₂ be acidic or basic? Why? (search on the internet)
2. As Elodea uses CO₂ during photosynthesis, will the solution become more acidic or basic? If the solution is also mixed with phenol red, what color should it become over time?
3. Will the concentration of CO₂ increase or decrease for Elodea in darkness? What color will the phenol red indicator show over time?
4. Which colors of visible light are used by chlorophyll for photosynthesis? Which are not?
5. Write a hypothesis for how the intensity of light would affect the photosynthetic rate in Elodea.

Isolation of Nicotine from Tobacco

1. Why did you add 5 mL of 3 M NaOH to the mixture prior to the steam distillation?

2. How can you tell when steam distillation is complete when a large quantity of an organic compound is steam distilled?

3. Is the nicotine you isolated pure? Provide experimental evidence to support your answer.

calculate the mean ionic activity of a 0.0350 m Na3PO4 solution for which the mean activity coeffiecient is 0.685.

Answer should be: 0.0547

Please show me how to get there. Thank you

• The rate of reaction is defined as

  Rate = −1∆[A] = −1∆[B] = + 1∆[C] = +1∆[D] ?? ∆?? ?? ∆?? ?? ∆?? ?? ∆??

• Average rate: the change in measured concentrations in any particular time period

• Instantaneous rate: the change in concentration at any one particular time

• Generally, the greater the concentration of reactant molecules, the faster the reaction

• Increasing temperature increases the reaction rate for most reactions

  Questions 1: Table I displays some data relating to an experiment 2NO (g) + O2(g) ? 2NO2(g)

  Table 1: Experimental data

  1. 1.1 Why is there a negative sign in equation (1)? Give a corresponding equation for the rate of production of a product.

  2. 1.2 Based on the data provided in Table 1, what is the average rate of consumption (M/s) for the NO(g) and O2(g) over the first 100 seconds? What is the rate of production (M/s) for the product, NO2(g)? (report three rates respectively)

  3. 1.3 Are the three rates you obtained in #2 the same? What is the potential problem you see if you use rate of consumption/production to characterize how fast the reaction proceed?

  4. 1.4 How shall we define rate of reaction that will give us unique value, independent of which

  species we are monitoring? Determine the rate of reaction accordingly for this problem.

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.