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A 0.2500 g sample of impure potassium chloride was treated with an excess of AgNO3. The precipitate was filtered, washed, and dried in a crucible with an empty mass of 34.9736 g. The mass of the crucible plus the chloride sample resulted in the formation of 35.2648 g. Calculate the percentage of KCl in the sample
1.00 mol Zn reacts with excess hydrochloric acid, 1.00 mol H2 gas is produced. At 25ºC and 1.00 atm= 101,325 Pa, this amount of H2 occupies 24.5 L (= 24.5 x10-3 m3). How much work is done by the chemical system.
calculate the volume of O2 the bottle could deliver to a climber at an altitude where the temp is -38 C and the atmospheric pressure is 0.40 atm.
Two syntheses using a grignard reagent, starting with an alkyl halide and later
What NaCl concentration results when 289 mL of a 0.680 M NaCl solution is mixed with 457 mL of a 0.330 M NaCl
What is the number of moles of atoms of oxygen contained in 49 grams of sulfuric acid, H2SO4?
another part says spectra of caffeine, benzoic acid, and a mountain dew sample in 0.10 M HCl. On a graph it has the points 8.74 mg/L for benzoic acid, 1.5 dilution for mountain dew soda,
what is the formula for the ion formed when each of the following elements loses its valence electrons.
You will start with 500 mg of one of isoamyl acloho to make isoamyl acetate. While the alcohols are liquids, we will measure them by mass directly on the balance, not by volume (i.e. the density of the alcohol will not be used; pretend the alcohol..
What is the molarity of a solution made by dissolving 68 g of Mg(NO3)2 in enough water to make 450 ml of solution?
Three pure compounds are formed when 1.00 g sample of elements X combine with, respectively, 0.472 g, 0.420 g, and 0.236 g of element Z. The first compound has the formula X2Z3.
During the purification and recrystallization of a solid why can't you just remove the solvent by evaporation after filtering and decolorizing
Determine the solubility of N2 in water exposed to air at 25 C if the atmospheric pressure is 1.2 atm. Assume that the mole fraction of nitrogen is 0.78 in air and the Henry's law constant for nitrogen in water at this temperature is 6.1 10-4 M/at..
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