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What is the pressure of the gas in this mercury manometer if h = 73 mm and atmospheric pressure is 773 mmHg?
Sodium carbonate Na_2CO_3) is used to neutralize the sulfuric acid spill. How many kilograms of sodium carbonate must be added to neutralize 4.03×103 kg of sulfuric acid solution?
Determine the mass of H 2 O in the flask and it's the true volume at 20° C?(at 20°C the Density g/mL=0.9982071,20°C the volume of 1g of water (mL) corrected for buoyancy is 1.0029 )
What is the minimum number of liters of air that must pass over a sample of the compound at 25oC to vaporize 1.0 mg of it? Hint: You know the Vapor Pressure from question "a" above and you are given the temperature and mass.
in an organic compound % of carbon is 75.2%,% of hydrogen is 10.75 and % of oxygen is 14.03..Find the empirical formula of compound?
If 157 of wet is collected over water at 24 and a barometric pressure of 739 , how many grams of have been consumed? (The vapor pressure of water is 22.38 .)
In an experiment, 2.50 g salicycylic acid was reacted with excess acetic anhydride to synthesize aspirin, as shown below.
2.00 L of H2 at a pressure of 398 torr and 1.00 L of N2 at an unknown pressure. If the total pressure in the flasks is 331 torr after the stopcock is opened,
The vapor pressure of pure methanol, CH3OH, at 30 C is 160. torr. How many grams of the nonvolatile solute glycerol, C3H5(OH)3, must be added to 131. g of methanol to obtain a solution with a vapor pressure of 133. torr.
Triethylene glycol, the solvent for your first reaction, and heavy mineral oil are both high boiling, high molecular weight solvents.
calculate the percentage of empty space in 1 mol of water at 25C. Obtain the density from the experiment " Some Measurements of Mass and Volume." The volume of a molecule of water can be taken as the sum of the volumes of the two hydrogen atoms.
The glass electrode used in commercial pH meters gives an electrical response proportional to the concentration of hydrogen ion. To convert these responses to a pH reading
Determine the concentration of the original Na 2 C 2 O 4 solution and disodium oxalate in the presence of excess acid.
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