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The empirical formula of a solid is AB2 and it dissolves to form the cation A2+ and the monoanion B-.Solid AB2 is added to water and allowed to reach equilibrium. At equilibrium, the concentration of A2+ is found to be 0.22 moles/L. What is the Ksp of this salt? Give your answer to three decimal places.
what number of grams of NaHCO3 in a .210 g piece of antacid would generate 38.0 moles of CO2, if the CO2 is measured at 20 degrees C and 1.00 atm.
A sample of gas with an initial volume of 32.5 L at a pressure of 760 mmHg and a temperature of 315 K is compressed to a volume of 16.3 L and warmed to a temperature of 435 K
The enthalpy of formation of compound X is -612 kJ/mol, and the sole product of its combustion has a enthalpy of formation of -671 kJ/mol. What is the enthalpy of combustion of compound X?
What amount of energy is required to completely ionize 6.2 grams of carbon atoms in the gas phase (C(g)) if the ionization energy of C(g) is 1086 kJ/mole?
Although the aluminum cylinder is a solid (and, therefore, is quite in-compressible), it actually contains quite a bit of empty space.
A gas is compressed in a cylinder from a volume of 20 L to 2.0 L by a constant pressure of 10 atm. Calculate the amount of work done on the system.
calculate the number of microstates, W, that have this energy. Make sketches of these microstates. Calculate the corresponding entropy for each state.
A sample of an unknown gas effuses in 12.4 min. An equal volume of H2 in the same apparatus at the same temperature and pressure effuses in 2.59 min.
A sample of H½O with a mass of 46.0 grams has a temperature of -58.0 C. How many joules of energy are necessary to melt 46.0 grams of ice? (Use 2.1 J/g.C for the specific heat of ice, and 334.4 J/g for the heat of fusion of water.)
A mixture of O2, CO2, and N2 has a total pressure of 762. torr. In this mixture the partial pressure of O2 is 112. torr and the partial pressure of CO2 is 185. torr. What is the partial pressure of the N2 (in torr)?
high boiling point are obtained now you need to identify the limiting reagent and compute the percent yield of nitrobenzene
A sample of pure NO2 is heated to 334 degree C at which temperature it partially dissociates according to the equation 2NO2(g)-->2NO(g)+O2(g)
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