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The equilibrium constant, Kc, for the following reaction is 1.29E-2 at 600 K:
COCl2(g) CO(g) + Cl2(g)
Calculate the equilibrium concentrations of reactant and products when 0.342 moles of COCl2(g) is introduced into a 1.00 L vessel at 600 K.
A chemist wanted to determine the concentration of a solution of lactic acid, HC3H5O3. She found that the pH of the solution was 2.59. What was the concentration of the solution.
Using a sample of gas has a mass of 38.7mg. Calculate the molar mass if its volume is 228mL at a temperature of 57°C and a pressure of 832torr?
Find the partial pressure and concentration of Nitrogen, Oxygen, and Carbon dioxide.
Determine hydroxyl and hydrogen ion concentration in this solution. (if Ka for ammonium ion = 5.0 x 10^-10.)
"The chains of several cell membrane - bound proteins are known to wind back and forth through the cell membrane, such that some parts of the protein structure are extracellular, some parts are intracellular, and some parts lie within the cell mem..
Determine the pressure inside a container of a gas connected to an open-end manometer filled with CCl4, has the density = 1.594 g/cm3,
10.00 mL of the final acid solution with excess barium chloride to produce a precipitate of barium sulfate (FW=2.33g/mol). The dry solid weighs 0.397 g.
A steel tank with a volume of 9.583 L contains N2 gas under a pressure of 4.972 atm at 31.8 °C. Calculate the number of moles of N2 in the tank.
A flask contains 0.180 of liquid bromine br2, . Determine the number of bromine molecules present in the flask.
What is the solubility in moles/liter for copper(II) iodate at 25 oC given a Ksp value of 1.4 x 10-7. Write using scientific notation and use 1 or 2 decimal places (even though this is strictly incorrect!).
Compute the atomic weight for this naturally occurring element A and A Naturally occurring element A exists in three forms of its isotopes
50.0 ml of 2.00M H2SO4 react with 75.O ml of 2.00M NaOH.Identify the limiting and excess reactants.
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