Sketch two 3d-orbital energy-level diagrams for the transition metal ion in [MCl₆]^4- when elongation and compression along the z axis take place, respectively. In the diagrams, label the names of the d orbitals, e.g., d_xy, d_xz, d_yz, d_z2, and d_x2-y2.

1. What is the theoretical yield of aspirin when reacting 3.08 g of salicylic acid with an excess of acetic anhydride? Report your answer to 3 significant figures.

2. If you prepare 3.45 kg of aspirin from an industrial process with a theoretical yield of 4.38 kg of aspirin, what is the percent yield of the process? Report your answer to 3 significant figures.

3. What is the yield of aspirin when reacting excess salicylic acid with 1.11 mL of acetic anhydride? The density of acetic anhydride is 1.082 g/mL. Report your answer to 3 significant figures.

Under anaerobic conditions, glucose is broken down in muscle tissues to form lactic acid according to the reaction, C6H12O6(s) → 2CH3CHOCOOH(s). Thermodynamic data for glucose and lactic acid at 298 K are given below. ΔHfº (kJ/mol) Cp.m (J/mol∙K) Smº (J/mol∙K) Glucose −1273.1 219.3 209.2 Lactic Acid −673.6 127.6 192.1 (a) Calculate ΔS for the system, surrounding and universe at T = 325 K. Assume the heat capacities are constant between 298 K and 325 K. (b) Is this reaction spontaneous or reversible at 325 K? Explain. (c) At what temperature, will this reaction establish the equilibrium?.

In a hydrogenic atom, s- and p-type orbitals of the same shell are degenerate. Explain why the 2s and 2p
orbitals would not be degenerate in a carbon atom, and justify their relative energy ordering. (Hint: consider
the radial distribution functions for these orbitals).

Advance oil chemistry, answer in brief and correct otherwise leave!

What are the major solid effluents come from oil industries.

Summarize the different of type of indicator electrodes, their definition, characteristics and applications

________________ compounds are made up of non-metals only.

1- In the titration between potassium iodate and the sodium thiosulfate solution, if the titration is not performed immediately after the addition of the sulfuric acid, how would this likely affect the calculated concentration of your diluted sodium thiosulfate solution?

2- Why did the titrations performed need to be started immediately after adding the sulfuric acid?

3- A sample of bleach was analyzed as in this procedure. The only procedural difference is that the student weighed out the bleach solution used instead of pipetting a certain volume of bleach. The student weighed out 0.634 g of commercial bleach solution. It was found that it required 13.24 mL od 0.0732 M sodium thiosulfate solution to react with the iodine produced. What is the percentage of sodium hypochlorite in this bleach sample?

4- The active ingredient in many commercial liquid bleaches is sodium hypochlorite. The bottle lists the percentage of sodium hypochlorite as 6.0%. If the density of commercial bleach is 1.084 g/mL of 0.150 M sodium thiosulfate is required to reach the end point in a titration similar to the one performed in this experiment, if a student analyzed a 2.0 mL sample of bleach.

At what temperature will a molecule of UF6 have the same average speed as a molecule of hydrogen at 37 degrees celsius?

Consider a titration of 0.15M NaOH and 250 mL of 0.10M HBr.

1. What is the pH of the HBr solution before any base is added?
2. What is the pH after 50 mL NaOH is added?
3. What is the pH after 125 mL NaOH is added?
4. What is the pH after 150 mL NaOH is added?

Part A.) Phosgene (carbonyl chloride), COCl2, is an extremely toxic gas that is used in manufacturing certain dyes and plastics. Phosgene can be produced by reacting carbon monoxide and chlorine gas at high temperatures: CO(g)+Cl2(g)⇌COCl2(g) Carbon monoxide and chlorine gas are allowed to react in a sealed vessel at 475 ∘C . At equilibrium, the concentrations were measured and the following results obtained: Gas Partial Pressure (atm) CO 0.840 Cl2 1.28 COCl2 0.130. What is the equilibrium constant, Kp, of this reaction?

Part B.) The following reaction was performed in a sealed vessel at 797 ∘C :

H2(g)+I2(g)⇌2HI(g)

Initially, only H2 and I2 were present at concentrations of [H2]=3.00M and [I2]=2.35M. The equilibrium concentration of I2 is 0.0700 M . What is the equilibrium constant, Kc, for the reaction at this temperature?

FOR QUESTION 5-7):Solve the problems completely

5) 1.60 g of an unknown molecular substance is dissolved in 20.0 g of benzene. The freezing point of pure benzene is 5.5^oC, and the freezing point of the mixture is 2.8^oC. What is the gram formula mass of the unknown substance?

6) Complete the following two Bronsted-Lowrey reactions and indicate the acid (A), base (B), conjugate acid (CA), and conjugate base (CB). (20)

                   HSO₄^-_(aq) + H₂O_(l)   

Air is 21.0% by volume oxygen molecules and C3H8 produces CO2 and H2O on combustion. What volume of air at 1.00 bar and 20.0 °C would be required to burn 38.8 Kg of propane (C3H8)?

When a 22.0 mL sample of a 0.448 M aqueous hydrocyanic acid solution is titrated with a 0.387 M aqueous barium hydroxide solution, what is the pH after 19.1 mL of barium hydroxide have been added? pH =

Order these chemical species by increasing pH of an 0.1M aqueous solution of each. That is, imagine making an 0.1M solution of each species. Select 1 next to the species that makes the solution with the lowest pH. Select 2 next to the species that makes the solution with the next higher pH, and so on. Notice that some of the rankings have been filled in for you already. Also notice that water is on the list. For that particular case, just compare the pH of pure water to the pH of the other solutions. Note for advanced students: for all charged species, you may assume the necessary counterions act as neither acids nor bases. species relative pH of 0.1M aqueous solution HF ▼(Choose one) ClO2− ▼(Choose one) HClO2 1 (lowest) H2O 4 NO2− 7 OH− ▼(Choose one) F− 6 HNO2 ▼(Choose one)