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A saturated solution of sucrose (C12H22O11) is made by dissolving excess table sugar in a flask of water. There are 50 g of undissolved sucrose crystals at the bottom of the flask, in contact with the saturated solution. The flask is stoppered and set aside. A year later a single large crystal of mass 50 g is at the bottom of the flask. Explain how this experiment provides evidence for a dynamic equilibrium between the saturated solution and the undissolved solute.
Hardness in groundwater is due to the presence of metal ions, primarily Mg2 and Ca2 . Hardness is generally reported as ppm CaCO3 or mmol/L Ca2 . To measure water hardness, a sample of groundwater is titrated with EDTA,
Calculate the electrode potential of the following half cell if it was at standard conditions. Then recalculate how this changes using.
Write as a superposition of 3 eigenstates, indicating the numerical value of each coefficient. Using the coefficients, demonstrate that is normalized.
The reaction is second order in and has a rate constant of 0.0123 at 25.0 . A reaction vessel initially contains 250.0 of 0.133 which is allowed to react to form the gaseous product.
RNA-based viruses such as poliovirus use RNA as their genetic storage material. An important anti-viral drug is ribavirin (see below). RNA polymerase can use ribavirin (the triphosphate version) as a substrate,
The partial pressure of O2 in air at sea level is 0.21 atm. Using Henry's law, calculate the molar concentration of O2 in the surface water of a mountain lake saturated with air at 20C and an atmosphere pressure of 650 torr.
A patient weighs 165 pounds and is to receive a drug at a dosage of 45.0 mg per kg of body weight. The drug is supplied as a solution that contains 25.0 mg of drug per mL of solution. How many mL of the drug should the patient receive?
sulfuric acid from an automobile battery requires 35.08 mL of 2.12 M sodium hydroxide solution for complete neutralization. What is the molarity of sulfuric acid ? the reeaction is H2SO4 + 2NaOH to 2H2O+ Na2SO4
how many kilojoules of energy are needed to convert 100 g ice at 10.0C to water at 20.0C? (the specific heat of ice at 10C is 2.01)
The gaseous product of a reaction is collected in a 25.0-L container at 27 degrees C. The pressure in the container is 300.0 kPa and the gas has a mass of 96.0 g. How many moles of the gas are in the container.
Compute the final temperature of the mixture (assuming no heat loss to the surroundings). The heat capacities of H2O(s) and H2O (l) are 2.08 and 4.18 J/g · °C, respectively, enthalpy of fusion for ice = 6.02 kJ/mol.
Its atomic number was believed to be 126. What is the most probable distance of the innermost electrons from the nucleus of an atom of this element?
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