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Use the ideal gas law to calculate the concentrations of nitrogen and oxygen present in air at a pressure of 1.0 and a temperature of 298 . Assume that nitrogen composes 78% of air by volume and that oxygen composes 21% of air.
A 5.00 g sample of KBr at 25.0°C dissolves in 25.0 mL of water also at 25.0°C. The final equilibrium temperature of the resulting solution is 18.1°C.
moist air exerts lower pressure and dry air exerts high pressure. how would the volume of the hydrogen gas that was ollectes been different if this eperiment was done on a very rainy day/ on a very dry day?
An overly efficient student simultaneously prepared two titration mixtures, consisting of diluted bleaching solution, KI solution, and HCI solution.
why is the h-f bond so much stronger than the h-I bond? how might you tell whether or not your toother paste conatied calcium carbonate caco3, or perhaps baking soda with out looking at the label?
Determine what is element Y if you have a compound consists of element "Y" and H, only and know that it is 79.89% element Y by mass. Each molecule has 3.00 times as many H atoms as Y atoms?
If Kp = 1.80 for this reaction, what is the total pressure inside the vessel at equilibrium?
a main component of photochemical smog. Classify this reaction as a synthesis, decomposition, single-displacement, or double-displacement reaction.
A .483 mol sample of graphite was heated with 2.14 mol oxygen gas to form carbon dioxide. Graphite is the limiting reagent in this reaction. Calculate the total moles of gas present after the reaction?
suppose the pressure inside a pressure cooker reaches 1.3 atm. By using the vapor-pressure table, estimate the temperature at which water will boil in this cooker
Determine the theoretical volume of NaOH it should take to neutralize the sulfuric acid in the equilibrium reaction mixture.
A student prepared a stock solution of the assigned compound by weighing 2.345 grams of Cu(NO3)2. 6H20 and diluting it with water to a final volume of 25.00mL.
A buffer solution is prepared by dissolving 1.51 g NH3 and 3.85 g (NH4)2SO4 in enough water to make 0.500 L of solution.
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