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You have isolated compound X from panda pancreas. You started with a whole pancreas, and finished up with 5 ml of a pure solution of X. You take 200 µl of this solution, and add it to 1.8 ml of buffer. The absorbance of this dilute solution at 340nm was 0.732. The molar extinction coefficient at 340nm for compound X is 12,400 l/mol cm. The formula weight of compound X is 14,200 g/mol How many total mg of X are there in the panda pancreas?
An Ideal gas is in a 375mL Container. Pressure inside is 1012 mmHg. Temp is 31.3 deg Celsius. How manly moles of Ideal Gas are there?
A 0.75-L bottle is cleaned, dried, and closed in a room where the air is 24°C and 50.% relative humidity (that is, the water vapor in the air is 0.5 of the equilibrium vapor
what is the maximum mass of CO2 that can be produced from the combustion of .377g C2H5OH
Discuss the importance of economics as it relates to pollution prevention. Supple at least two seperate examples to augment your discussion.
Radioactive nitrogen-13 has a half-life of 10 minutes. After 40 minutes, how much of this isotope would remain in a sample that originally contained 96 mg?
What is the pH of a solution that is 6.5×10-2M in potassium propionate and 8.5×10-2M in propionic acid?
A chemist dissolves 128 mg of pure hydrobromic acid in enough water to make up of 110 mL solution. Calculate the pH of the solution.
Metals such as magnesium and zinc react with dilute sulfuric acid to give hydrogen, according to the equation: M (s) + H2SO4 (aq) -------> MSO4 (aq) + H2 (g) When 5.00 g of a mixture of powdered magnesium and zinc were dissolved in diluted sulfuri..
H2 and Cl2 combine to form HCl. In a gas phase equilibrium mixture of H2, Cl2, and HCl at 300 K, [HCl] = 0.0036 mol/L and [Cl2] = 0.00485 mol/L.
Grignard reagent and carbonyl-containing compound. Suppose scheme one involves the reaction of the Grignard reagent containing more carbon atoms with the carbonyl compound containing less carbon atoms and scheme two involves the reaction of the Gr..
Consider the reaction CaCN2 + 3 H2 O → CaCO3 + 2 NH3 . How much CaCO3 is produced if 47.5 moles NH3 are produced?
In which conversion is an oxidizing agent required? a. CH3CH2CH2CH3
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