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1.5 mol of oxygen are mixed with an unknown amount of nitrogen in a 2.0 L container at a temperature of 26.0C. If the final pressure of the mixture is 20.3 atm, what is the number of moles of nitrogen in the container?
An aqueous CaCl2 solution has a vapor pressure of 83.7mmHg at 50 C . The vapor pressure of pure water at this temperature is 92.6mmHg.
A cube of metal has a mass of 0.321 kg and measures 3.05 cm on a side. Calculate the density and identify the metal.
.134 mol of KCl and .257 mol of CaCl2 were dissolved in water. calculate the total number of moles of Cl- ions in the solution
Give TWO possible reactions you could use in each case and write an equation for each reaction.
How much A would have been extracted into ether if the orginal aqueous solution had been extracted once with a 500-mL portion of ether? What percentage of A would have been extracted by the ether?
Calculate the number of grams of alcohol present in 1.00 L of 87 proof gin. The density of ethanol is 0.798 g/mL.
A gas of unknown molar mass was allowed to effuse through a small opening under constant pressure conditions. It required 184 s for 1.00 L of this gas to effuse.
Determine the charge on each ion in the following compounds, and name the compound. Li2O and CaS
The molar mass for NaCl and water are 58.443 g/mol and 18.015 g/mol, respectively. Calculate the partial molar volumes for NaCl and water in a 0.35m solution.
A 44.2 L sample of a gaseous hydrocarbon, measured at 1.00 atm pressure and 25 C is burned in excess oxygen, liberating 2.55x10^3 kj of heat at constant pressure.
Assuming 100% dissociation, calculate the freezing point and boiling point of 3.27 m AgNO3(aq). Constants may be found here.
Calculate the final temperature of the metal and water mixture, assuming no heat loss to the surroundings.
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