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At 450 K the equilibrium concentrations for the following reaction was measured and used to calculate the kc value of 0.0431. What is the value of Kp for the Reverse reaction under the same conditions?SO2Cl2 (g) <--> SO2 (g) + Cl2 (g)
A 0.2527-g sample of a mixture of Mg(OH)2 and Al(OH)3 was treated with 50.00 mL of 0.225 mol L 1 HCl(aq). The resulting solution required 13.73 mL of 0.176 mol L 1 NaOH(aq) to neutralize the excess, unreacted HCl.
The atmospheric oxidation of nitrogen monoxide was studied at 183C with initial partial pressure of 1.000 atm of NO and 1.000 atm of O2. At equilibrium, Po2= .50-6 atm. Calculate Kp. 2 NO(g) +02 ->
Imagine two solutions with the same concentration and the same boiling point, but one has benzene as the solvent and the other has carbon tetrachloride as the solvent. Determine that concentration and boiling point.
NH3 is a weak base (Kb = 1.8 × 10-5) and so the salt NH4Cl acts as a weak acid. What is the pH of a solution that is 0.049 M in NH4Cl
2Na + 2H2O → + H2 How many moles of hydrogen gas are produced when 0.066 mole of sodium is completely reacted?
What is the partial pressure of argon, in torr, in a container that also contains neon at 147 torr and is at a total pressure of 536 torr?
The enthalpy of vaporization of water at 373 K and 1 bar is 40.7 kJ/mol and the molar heat capacities are 75.3 J/(mol K) for liquid and 33.6 J/(mol K) for gaseous water. Find the enthalpy of vaporization of water at 273 K and 1 bar.
Indicate the hybridization for each carbon and nitrogen atom in this molecule, then draw an orbital overlap picture for the molecule.
A mixture of ammonium chloride and sand is placed in an evaporating dish and massed at 56.246g. The mixture is heated, driving off the ammonium chloride and massed again
To a second 25.00 mL part, 10.00 mg of lead was added and extracted into a second 10.00 mL portion of the same organic solvent. This solution gave A = 0.525. What was the concentration of lead, in mg/mL, in the original sample?
Write an equation of the dissolution reaction for each of the precipitates that was soluble in CH3COOH. Al2(SO4)3+NaOH
to reach equilibrium (at pH 7.00) through titration by adding 14.25 mL of 0.2030 M NaOH to 20 mL of this solution. What is the Molarity of the acid?
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