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What is the pH of 0.549 M piperidinium iodide, C5H11NHI? The Kb of piperidine, C5H11N, is 1.3 x 10-3.
How many quartz of ethylene glycol, C2H6O2 (density = 1.116 g/mL). Will have to be added to 5 gal of water (density = 1 g/mL) to protect an automobile radiator down to a temperature of-10 oF?
A doctor prescribes 3 g of a drug, daily, for a patient. The pharmacist has only 750-mg tablets available. How many tablets will the patient take daily
An exothermic reaction liberates 7.58 kJ of heat in a coffee cup calorimeter containing 157 grams of solution. The temperature of the solution in the calorimeter increases by 11.2°C. How much heat was absorbed by the calorimeter? Assume the specif..
A 25.0g sample of nitrogen (N2) has a volume of 50.0L and a pressure of 630.0 mmHg. What is the temperature of the gas.
Calculate the amount of n2 gas released(in liters) when the diver returns to the surface of the water where the partial pressure of N2 is 0.80 atm
A sample of indium sulfate, In2(SO4)3, contains 0.0446 moles of oxygen. What mass of indium is present?
Using a single reagent and only reaction chemistry that was part of this experiemnt, how could you distinguish between the following pair of substances contained in seperate test tubes?
A tank contains a mixture of 3.0 mol N2, 2.0 mol O2, and 1.0 mol CO2 at 25 degree Celcius and a total pressure at 10.0 atm. Calculate the partial pressure(in torr) of each gas in the mixture.
Trees in cold climates may be subjected to temperatures as low as -60 C. Estimate the concentration of an aqueous solution in the body of the tree that would remain
determine the temperature at which the reaction will become spontaneous. See the section on Free Energy and spontaneity in our book. You will also find Appendix C very helpful as well. The delta H for the reaction is 90.84 kiloJoules/mol
A buffer (pH 3.70) was prepared by mixing 1.00 mole of formic acid and 1.00 mole of sodium formate to form an aqueous solution with a total volume of 1.00 L.
When the reaction that occurs finally ceases, what will be the mass of unreacted copper in the bar? What will be the mass of silver metal that "plates out" of solution (that is, what mass of silver metal is produced by the reaction)
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