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Calculating concentration in equilibriumAt pH 6.00 and pE 2.60, what is the concentration of Fe2+ (mol/L) in equilibrium with Fe(OH)3?
Hint: Use the Nernst equation and the Ksp for the solubility of solid iron (III) hydroxide.
how to set up the Nernst equation and where it is appropriate to plug in the value and how it correlates with the concentration.
step by step directions and the constants (such as the ksp) used
When pure carbon burns in air, 10.0 kg of carbon react with the oxygen in the air to form 36.7 kg of carbon dioxide. Calculate the percentage of oxygen contained in carbon dioxide.
What is the molar mass of this substance, express your answer in g/mol and determine the moloar concentraitions Cr 2 O 7 ^2 and of K + ?
The mass of an Argon atom is more than that of a Helium atom. Does that mean that because of Argon has larger mass, it exerts a higher pressure on the walls of container than Helium at the same volume, molar density and temperature? Give explanati..
The density of liquid oxygen at its boiling point is 1.14kg/L , and its heat of vaporization is 213kJ/kg. How much energy in joules would be absorbed by 4.0 L of liquid oxygen as it vaporized.
A 2.42-L flask is filled with propane gas (C3H8), at 1.00 atm and -13.0°C. What is the mass of the propane in the flask.
If 100.0J of energy are added to 25.0g of water at 50 degrees celcius,what will the final temperature of the water be?
An impure sample of sodium carbonate, (Na2CO3) is allowed to react by dissolving it in an aqueous solution of 0.134 M HCl, according to the following reaction:
The feed to reactor contains only C 2 H 4 and HBr. if the molar flow rate = 165mol/s, compute the fractional conversion of the limiting reactant?
The solubility product of PbBr2 is 8.9x10^-6. Determine the molar solubility in the following. (a) pure water (b) 0.20 M KBr solution (c) 0.15 M Pb(NO3)2 solution
Calculate the fraction of Fluorine atoms at 1000 K in each of the first three electronic levels based upon the following data
The enthalpy of formation of ethanol, C2H5OH, is 277.o kJ/mol at 298.15K. Calculate the enthalpy of combustion of one mole of ethanol, assuming that the products are CO2 and H2O.
Determine the molar mass of the compound if boiling point constant for CCl 4 =4.95 K · kg/mol.?
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