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Chemistry - Analytical Chemistry - Molar MassAn aqueous solution is made by dissolving 33.2g of the compound in 250mL of water. The solution has an Osmotic Pressure of 1.2 atm at 250*C. What is the molar mass of the compound?
2 NO(g) + O2(g) 2 NO2(g) In one experiment 0.633 mole of NO is mixed with 0.354 mole of O2. Calculate also the number of moles of NO2 produced.
A solution of ethanol (C2H6O) in water is sometimes used as s disinfectant. 1.00 L of this solution contains 553 g or ethanol and 335 g of water. What is the mole fraction of ethanol in this solution.
A 4.20 g nugget of pure gold absorbed 299 J of heat. The initial temperature was 22.0°C. What was the final temperature.
Determine at what temperature must a balloon be heated to have six Litres volume consider that the balloon was at the temperature of 25 degree Celsius and volume of two litres initially?
If the reaction N2(g) + 3H2(g) ! 2NH3(g) is carried out at constant temperature and pressure, how much H2 is required to react with 6.4 L liters of N2.
What is the molality of CrCl3 in a solution prepared by dissolving 75.2 g chromium(III) chloride hexahydrate in 250.0 g of water.
Why is toxicity diminished in other congeners where chlorines are removed from the 2,3,7,8 positions, or when chlorines are added to remaining positions on the rings?
A solution of 100 mL of 0.2 M NH3 is titrated with 50 mL of 0.5 M HNO3. What is the pH of the resulting solution? Kb for NH3 is 1.8 × 10-5.
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.
If the titrant has a molarity of 0.2750 M and there are 25.00 mL of analyte present, what is the molarity of the analyte?
How many grams of Ca(OH)2 are needed to neutralize 3.6 moles of HCl in 655 mL of solution? The molar mass of HCl is 36.46 g/mol. The molar mass of Ca(OH)2 is 74.1 g/mol.
A 14.0-g sample of ice at -18.0°C is mixed with 122.0 g of water at 87.0°C. Calculate the final temperature of the mixture assuming no heat loss to the surroundings.
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