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1. Give an example of a metabolic reaction of a drug or endogenous substance for each of the following reaction types and determine the electrophile and nucleophile
1. SN1 reaction
2. Radical reaction
3. E1 reaction
Mixture also contains He (helium gas). determine the partial pressure of the He gas?
dissolved in 200 mL of solution. What is the pH of the solution? pKa1 = 6.37 and pKa2 = 10.25.
Explain the differences in values of the ligand field splittings (Delta = DeltaO or DeltaT for the cobalt complexes below): [Co(NH3)6]3+ ----> Delta = 22,900 cm-1, [Co(H20)6]3+ -----> Delta = 18,200 cm-1, [Co(NH3)6]2+ -----> Delta = 10,200 cm-1 [C..
You have 32.4 g of O2 gas in a container with twice the volume as one with CO2 gas. The pressure and temperature of both containers are the same. Calculate the mass of carbon dioxide gas you have in the container.
Calculate the required quantity of the reagent and the volume of water that must be added for dilution.
Explain what is the longest wavelength of light that will give photons of sufficient energy to break the bond and cause the isomerization
A 1-L flask is filled with 1.30g of argon at 25C . A sample of ethane vapor is added to the same flask until the total pressure is 1.00 atm. What is the pressure of argon Par in the flask. What is the partial pressure of ethane, Pethane, in the fl..
a solution is prepared by dissolving 4.21 g of a non electrolyte in 50 g of water. if the boiling point increases by .203 degree celsius, what is the molar mass of the solute? the boiling point elevation constant for water is .502 degree celsius p..
If a solution of sea water was found to have a molarity of .26 m, what is the new freezing point of this water? (Kf = 1.86 degrees C/M)
B2H6 + 3O2= B2O3+3H2O ; delta H=-2035 KJ how much heat is released when a mixture of 7.35 g B2H6 and 2.60 g O2 is burned?
Calculate the concentration of all species in a 0.050 M tartaric acid solution. These species include [H3O+], [HC4H4O6^1-], H2C4H4O6] and [C4H4O6^2-]. For tartaric acid, Kal=1.0 x 10^-3 and Ka2=4.6 X 10^-5.
Calculate the apparent molecular weight of the unknown hydrocarbon on the basis of the freezing-point depression experiment.
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