Physical Chemistry Homework Help

8 calculate the ionization energy of the li 2 ion 9 show that the wavefunctions 100 and 200 for the hydrogen atom are

8 calculate the ionization energy of the li 2 ion 9 show that the wavefunctions 100 and 200 for the hydroge 10 calculate

Problems 1. The following electrode potentials were observed after a 1-year immersion period in natural seawater of pH 8.0 [20]:

5. In the interpretation of Pourbaix diagrams, corrosion is considered to occur when the concentration of dissolved metal ions attains a minimum concentration of 1.0 x 10-6 M. Suppose that a 0.50-cm² sample of aluminum immersed in 1.0 L of an aqueous solution corrodes at a constant current density of 100 μA/cm². How long will it take to produce a concentration of 1.0 x 10-6 MAI³+?

6.1 The problem has the potentials vs SCE whil pourbaix diagram has potential vs SHE, so you to convert via table 3.2.

which of the following displays geometrical isomerism ) square-plunar ERH (U)a clz square planar [P+ Len)272 Octunedral. Octahedral rWINHa)CI]2t

B.NumePOllowing metals 1, Ch torinepen ta aqua ehh liro Ch ruminiun nchiorpenta a qu a Ch rumi um (Ll!) 1on Chlonde 3. Penta aq -vh ch lor1) ch luride

Problem A: Below is shown a plot of the natural logarithm of the diffusion coefficient versus reciprocal of the absolute temperature, for the diffusion of iron in chromium. Determine values for the activation energy(in J/mol) and pre exponential (in m?/s).

Need Overall cell reaction for sodium sulfate electrolysis. Anode and cathode are given. Here are the half reactions for anode and cathode: \text { Anode: } \operatorname{Cu}(\mathrm{s}) \longrightarrow \mathrm{Cu} \wedge 2+(\mathrm{aq})+2^{\wedge} \mathrm{e}-\text { and cathode: } 2 \mathrm{H} 2 \mathrm{O}(1)+2 \mathrm{e}^{\wedge} \rightarrow \mathrm{H} 2(\mathrm{~g})-2 \mathrm{OH}-(\mathrm{aq})

Problem 5.19: Using the data in Table 5.2, compute the value of D for the diffusion of zinc in copper a t650°C. Show your work as you would on an exam: equations in symbols, values of the parameters with units, any unit conversions, final answer with units.

1. Which test tube (1 or 2) initially had the most solid precipitate? Why was there moreppt. in this test tube? (Hint: Which solution initially contains more free floating \left.\mathrm{C}_{2} \mathrm{O}_{4}{ }^{2-} \text { ions? } \ldots . \mathrm{K}_{2} \mathrm{C}_{2} \mathrm{O}_{4} \mathrm{Or} \mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4} ?\right) Test tube 2 had the more solid precipitate because the dissociation of K2C2O4 is more feasible than H2C2O4 Thus in case of potassium oxalate there are more oxalate ions present than that of oxalic acid . Hence by addition of CaCl2 test tube2 would produce more precipitate.

4) Calculate the mass of oxygen produced from 12.3 g of nitric oxide.

Problem 2. For the combustion of 1 mol of butanoic acid (C4H8O₂) with O₂ to form CO₂ and H₂O, figure out the stoichiometry of the balanced chemical reaction.

Problem 8. When it is found in well water, fluoride is sometimes due to the dissolution of the mineral fluoriteCaFz(s) which dissolves according to \mathrm{CaF}_{2 / \mathrm{s}]}=\mathrm{Ca}^{2+}+2 \mathrm{~F}- For this mineral at 25 °C, Ksp = 10-0. In the U.S., any level higher than 4 ppm fluoride exceeds the federal drinking water standard. In Kenya, levels as high as 35 ppm fluoride can be found. If the water is in equilibrium with fluorite at 25 °C, plot the concentration of Ca²* in molarity vs. concentration of fluoride in ppm from 1 to 35 ppm. Don't forget to convert the fluoride concentration to molarity for the calculation.

One of the most important industrial applications of redox titrations is evaluating the chlorination of public water supplies. One approach for determining the total residual chlorine in treated water uses the oxidizing power of chlorine to oxidize I- to iodine. If this reaction is carried out in the presence of excess iodide the soluble triiodide ion, I3-, is formed. The amount of I3- is determined by back titration with thiosulfate, S₂O3²-, which is oxidised to the tetrathionate anion, S406²-. (i)Write a balanced net ionic equation for the reaction between Chlorine and iodide in an excess of iodide. (ii)Write a balanced equation for the reaction between thiosulfate and triiodide. The world Health Organisation taste guideline for chlorinated water is 5 mg.L-¹. A sample of Canberra tap water was tested for its residual chlorine content using the redox titration process described above. A 500 mL sample of water was treated with 5 g of sodium iodide to convert the residual chlorine to chloride. The triiodide was then determined by taking 25 mL a liquots of the water and titrating it with 0.1409 M sodium thiosulfate. The results of the titrations were as follows: (iii) Determine the average titre. (iv)What is the triiodide concentration? (v)What was the concentration of the chlorine in the initial water sample? (vi)Does the water sample meet the WHO guideline?

Back Introduction docx.المستند (7) تا The pH is a measure of how acidic or basic a substance or solution is. pH is measured on a scale of 0 to 14. but, the buffer Solution is a water solvent based solution which consists of a mixture containing a weak acid and the conjugate base of the weak acid, or a weak base and the conjugate acid of the weak base. In this experiment, we will measure the pH of solutions and know the pH level. We will also measure the pH of the buffer and the . pH of HCL and NaOH

3. Examine the reaction mechanism found below: Step 1: P₂+Q₂ → 2PQ (slow) Step 2: 2PQ→→ P₂Q₂ (fast) Step 3: P₂Q₂ →→ P₂ + Z (very fast) a. Draw a circle around any reaction intermediates. b. Draw a box around any species that can be considered a catalyst. c. In the box above, provide the overall equation for this process. d. In the box below, provide the rate law based on this mechanism.

6. A student performs the reaction below in three experiments studying initial concentrations and initial rates. The data is summarized in the table below. a. What is the order of this reaction with respect to NO? b. What is the order of this reaction with respect to Br₂ ? c. What is the overall order of this reaction? d. What is the rate law constant, k, for this reaction? (Be sure to include the value and the units.) SHOW ALL YOUR WORK.