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Consider the folowing mechanism for the oxidation of bromide ions by hydrogen peroxide in aqueous acid solution.
The kinetics of decomposition of dinitrogen pentaoxide is studied at 50 degrees C and at 75 degrees C. Which of the following statements concerning the studies is correct
In tables of thermodynamic data provided in chemistry books, one finds delta Hf, delta Gf, and delta S listed. Briefly explain why the entropy data are supplied as S
Give the cell notation based on the following reaction: Fe(s) + Hg2 ++ (aqueous) = Fe++ (aqueous) + 2Hg (l) the solution concentrations are 0.01 M
For a copper zinc cell of sulfate concentration 1M the potential is see to be 1.10 volts. Calculate the potential of the cell at room temperature if the concentrate of zinc sulfate is 1.2 M and the
For the copper zinc cell the potential at 25 degrees C is 1.10 volts. The reaction is: Cu++ (aq) + Zn(s) = Zn ++ (aq) + Cu(s) Calculate the equilibrium constant for this reaction (a wire is connecte
Water molecules can undergo a self-ionization reaction to produce very small concentrations of hydronium and hydroxide ions
Copper metal is dipped into a 0.01M silver nitrate solution. Calculate the concentration of silver ions in the final equilibrium solution.
Given the three formation equations and their enthalpy values, calculate the enthalpy of the given reaction.
A sample containing 839g of water was cooled from 95°C to 27°C. How much heat was involved in this process? provide the answer in joules or kilojoules
The calorimeter contains exactly 281 g of water, and the temperature increases by 1.126°C. Calculate the heat given off by the burning Mg, in kJ/g and in kJ/mol.
A solution is colorless in phenolphthalein and blue in bromcresol green. Therefore we can conclude that the pH of the solution
A 25.00 mL sample of the weak acid, propionic acid, HPr, of unknown concentration was titrated with 0.104 M KOH. The equivalence point was reached when 35.31 mL of base had been added. The concentra
The calorimeter contains exactly 341 g of water, and the temperature increases by 1.126°C. Calculate the heat given off by the burning Mg, in kJ/g and in kJ/mol.
Write structural formulas for six, recognizing that the molecular formula may be twice the empirical formula in some of them.
a water soluble salt forms a precipitant during Group 3 analysis. An acidic solution of this precipitant and NaBiO3 yields a pinkish color. This same salt has no reaction to concentrated H2SO4 or Ag
Given the following equilibrium constant at 25 C, calculate the equilibrium constant for the unknown reaction below.
Assume that the following terpenoid is derived biosynthetically from isopentenyl diphosphate and dimethylallyl diphosphate, each of which was isotopically labeled at the diphosphate-bearing carbon a
Calculate the pH of the solution made by adding 0.50 mols of HOBR and 0.30mols of KOBR to 1.00L of water. The Ka value of forHOBR is 2.0x10 ^-9.
Use balanced equations to determine whether either Fe(OH)2 or CuS has a different solubility with a change in pH:CuS changes solubility with changing pH. Fe(OH)2 does not change solubility.
because the electronegative chlorine atom pulls electrons away from the O-H bond and thus weakens it. Calculate the hydronium-ion concentration and the pH of a 0.0022 M solution of chloroacetic acid
What is the hydronium-ion concentration of a 5.23 10-4 M solution of p-bromobenzoic acid, BrC6H4COOH, for which Ka = 1.00 10-4
What is the molar mass of 1.00-g sample of gas that occupies a volume of 750 mL at a pressure 725. mm Hg and a temperature of 27.0°C?
Find the molar mass of a gas using the combined gas law if 950. mL of the gas collected over water at 750.0 mm Hg and 21.oC has a mass of 0.905 g
Use balanced equations to determine whether either CuBr or Ca3(PO4)2 has a different solubility with a change in pH: