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A sample containing only carbon, hydrogen, phosphorus, and oxygen is subjected to elemental analysis. After complete combustion, a 0.4946-g sample of the compound yields 0.7092 g of CO2, 0.4355 g of H2O, and 0.3812 g of P4O10. What is the empirical formula of the compound?
what can we conclude about the energy required to excite an electron from n=5 to n=6 versus the energy required to excite an electron from n=4 to 5.
Calculate the mole fraction of benzene in a solution of benzene and toluene that has a total vapor pressure of 266mmHg at 60 degrees C. Note that both components contribute to the vapor pressure over the solution.
A solution is prepared by dissolving 14.4 g ammonium sulfate in enough water to make 100.0 mL of stock solution. A 11.50 mL sample of this stock solution is added to 55.00 mL of water.
determine the initial concentration - Constant rate is 3.20×10-4 M/s for a zero-order reaction. concentration has dropped to 9.00×10-2 M after 60.0 seconds
How many grams of sodium lactate should be added to 1.00 L of 0.150 M lactic acid to form a buffer solution with pH= 4.00? Assume that no volume change occurs when the sodium lactate is added.
How much heat is gained (in Joules) by the water where a chemical reaction takes place in 100 mL aqueous solution and has a temperature increase of 14 C?
What affect would an increased concentration of 2,3-BPG have on the oxygen-binding curve for hemoglobin. Why would this adaptation be beneficial for functioning well at high altitude?
element is the central atom of sodium chloride, megnesium sulfate, calcium carbonate, ammonia, and hydrogen cyanide?
when ammonia is burned in oxygen, free nitrogen gas and water are produced. What volume of ammonia will react completely with 25.0 L of oxygen? what volume of nitrogen gas is formed.
Calculate the change in pH when 6.00 mL of 0.100 M NaOH(aq) is added to the original buffer solution.
A 49 gram sample of impure potassium nitrate (KNO3) was heated to complete decomposition according to the equation 2 KNO3(s) → 2 KNO2(s) + O2(g) After the reaction was complete.
Bauxite, the principle ore used in the production of aluminum cans, has a molecular formula of Al2O3•2H2O. (a) Determine the molar mass of bauxite. (b) How many grams of Al are in 0.58 moles of bauxite?
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