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Determine the mass of lithium hydroxide produced when 0.38 g of lithium nitride reacts with water to make Ammonia (NH3) and Lithium hydroxide.
Thirteen grams of titanium react with 60.0 g of bromine. How many grams of titanium(IV) bromide are produced, assuming 100% yield.
The vapor pressure of pure CH2Cl2 (with molecular weight 85 g/mol) is 133 torr at 0?C and the vapor pressure of pure CH2Br2 (with molecular weight 174 g/mol) is 11 torr at the same temperature.
If 5.28 x 10^3 kg each of NH3, O2, and CH4 are reacted, what mass of HCN and of H2O will be produced, assuming 100% yield?
A 1.43-L flask is filled with propane gas (C3H8), at 1.00 atm and -23.0°C. What is the mass of the propane in the flask?
A 7.0 liter balloon at room temperature (22 degrees celsius) contains hydrogen gas. If the balloon is carried outside to where the temperature is -3.0 degrees Celsius.
What volume of .250 M calcium chloride would be required to precipitate silver chloride if it is mixed with 600.0 ml of 0.650 M Silver nitrate.
When heated, lithium reacts with nitrogen to form lithium nitride: 6Li(s) +N2(g) → 2Li3N(s)
Determine the partial pressure and the total pressure using Dalton's law of partial pressures - Determine the total pressure of the mixture.
Calculate the mass of oxygen dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air. Assume the mole fraction of oxygen in air
The vapor pressure of pure acetone (propanone) is 266 torr. When a non-volatile solute is added, the vapor pressure of acetone above the solution falls to 232 torr. What is the mole fraction of acetone in the solution?
What might you conclude about the structures of these 3 (X,Y,Z)compounds?
What is the solubility product constant? Given Ksp = 1.1 x 10^-3 for BaF2(s), calculate the molarity of Ba+2 in a saturate solution of BaF2 (at equilibrium).
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