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What is the minimum quantity of atmospheric oxygen required to completely convert 0.30 moles of propan-1-ol into carbon dioxide and water?
What is the maximum wavelength of light capable of removing an electron from a hydrogen atom in the energy states characterized
A liquid that has a density of 0.80 0.01g/ml and 0.80-0.01 g/ml is insoluble in cyclohexane. what is the liquid? what is the boiling point of cyclohexane at 600 mm hg?
Two objects at different temperatures are placed in a perfectly insulated calorimeter. When the system reaches equilibrium, which of the following statements is true?
What is the total vapor pressure 4 at 20° C of a liquid solution containing 0.30 mole fraction benzene, C6H6, and 0.70 mole fraction toluene, C6H5CH3? Assume that Raoult's law holds for each component of the solution.
Consider the chemical reaction 2NH3(g) N2(g) + 3H2(g). The equilibrium is to be established in a 1.0 L container at 1,000 K, where Kc = 4.0 ? 10-2. Initially, 1,220 moles of NH3(g) are present. Estimate the equilibrium concentration of N2(g).
What are the coeffiecients of potassuim iodide + lead (II) acetate - lead (II) iodide + potasium acetate when properly balanced
The Ka of butyric acid, C3H7COOH is 1.5 x 10-5. What is [C3H7COO-] in a 0.397 M solution of C3H7COOH
Weak base NH3 has Kb = 1.75 * 10^-5. Calculate the concentration of hydronium and pH of 0.252 M NH3 aqueous solution.
Calculate the maximum bond extension in Angstroms past equilibrium in HCl35 in its first excited vibrational state. The fundamental absorption frequency of this molecule is 2885 cm-1.
A 28.0-g sample of nitrogen gas combines completely with 6.0 of hydrogen gas to form ammonia. What is the mass of ammonia formed.
Elevation Pressure 0 ft 760 mmHg 1000ft 740.2 mmHg 2000ft 720.4 mmHg What is the boiling point of water at an elevation of 6.00×10^3 ft
A sample of copper sulfate pentahydrate, CuSO4 . 5H2O, contains 3.782 g of Cu. How many grams of oxygen are in this same sample
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