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The density of acetic acid vapor at the normal boiling point, 118.5 degrees C, is given by 3.15 g/L (normal boiling point is the boiling temperature at P = 1 atm).
a) calculate the fraction of the vapor that is monomer and the fraction that is dimer.
b) what is the partial pressure of the monomer, P sub m, and of the dimer, P sub d?
c) what is the equilibrium constant, Kp, at this temperature for the reaction:
2 CH3COOH (g) <----> (CH3COOH)2 (g), Kp = (P sub d)/ (P sub m)^2
What was the concentration of the unknown HClO4 solution? The neutralization reaction is: HClO4(aq)+NaOH(aq)==>H2O(l)+NaClO4(aq)
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An equilibrium mixture at 225 degrees C contains 0.10 M NH3 and 0.20 M H2 for the reaction 3H2 (g) + N2 (g) --- 2NH3(g) If the Kc at this temperature is 1.7 X 10 2.
Determine the mass of sodium phosphate that yields 1.00 g of calcium phosphate precipitate.
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which hydroxide precipitates first as NaOh is slowly added to the solution? b) what is the molar concentration of the first cation precipitated when the other cation just starts to precipitate out of solution?
Derive the rate law expression for the chlorination of vinyl chloride based on this mechanism.
while a person with inherited MCAD deficiency will experience life-threatening symptoms (lack of energy and coma) after about a day of fasting
Choosing CO^2+, write a series of two balanced chemical equations representing the reaction that occurs when HCl and NH3 are added to an aqueous solution of the transition metal cation.
How much water must be added to 488 mL of 0.223 M HCl to produce a 0.134 M solution?
You start with 100.0 mL of a 0.2500 M solution of NaCl sitting in a beaker. After several days you test the solution and find that it is now 0.3125 M. How much water must have evaporated?
Compute the final temperature of the solution assuming no heat lost to the surroundings .the solution has a specific heat capacity =4.18 J/°C·?
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