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A solution is prepared by mixing 0.0300 mol CH2Cl2 and 0.0500 mol of CH2Br2 at 25°C. Assuming the solution is ideal, calculate the composition of the vapor (in terms of mole fractions) at 25°C. At 25°C, the vapor pressures of pure CH2Cl2 and pure CH2Br2 are 133 and 11.4 torr, respectively. XVCH2Cl2: XVCH2Br2:
A patient weighs 146 pounds and is to receive a drug at a dosage of 45.0 mg per kg of body weight. The drug is supplied as a solution that contains 25.0 mg of drug per mL of solution.
calculate the number of moles of AgCrO4(Ksp=9.0x10^12) that will dissolve in 1.00L of 0.010 M K2CrO4 solution. what will be the ion concentrations at equilibrium?
Cesium(Cs) is used extensively in television cameras and in photocells because it has lowest ionization energy of all the stable elements.Determine the maximum kinetic energy of a photo electron ejected from cesium.
Zinc metal can be obtained from zinc oxide (ZnO) by reacting the oxide with the element carbon. The products of the reaction are Zn and CO2.
2SO2(g) + O2(g) 2SO3(g) Suppose the volume of this system is compressed to one-half its initial volume and then equilibrium is reestablished.
66.0 mL of a 1.60 M solution is diluted to a volume of 288 mL. A 144-mL portion of that solution is diluted using 163 mL of water. What is the final concentration.
A gas occupying a volume of 263 mL at a pressure of 0.970 atm is allowed to expand at constant temperature until its pressure reaches 0.541 atm. What is its final volume?
How much heat is evolved when 9.07 x 105 g of ammonia is produced according to the following equation:
A sample of calcium carbonate absorbs 45.5 J of heat upon which the temperature of the sample increases from 21.1 degrees celcius to 28.5 degrees celcius.
The standard molar enthalpy of formation of ClF3 is -405 kJ. 1/2 Cl2(g) + 3/2 F2(g) → ClF3(g)
Find out how many total moles of gas are produced If a sample has 2.10 mL of nitroglycerine (density = 1.592 g/mL) is detonated?
Silver chloride, often used in silver plating, contains 75.27% Ag. Calculate the mass of silver chloride required to plate 225 mg of pure silver.
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