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At a certain temperature, the equilibrium constant for the following chemical equation is 3.50. At this temperature, calculate the number of moles of NO2(g) that must be added to 2.88 mol of SO2(g) in order to form 1.20 mol of SO3(g) at equilibrium.
The rate of disappearance of HBr in the gas phase reaction is 0.103 Ms-1 at 150 deg Celsius. what is the rate of reaction.
What is the percent ionization of a solution made by adding 6.00 grams of CH3COOH to 100 g of water (Kb = 0.512 ?C/m) if the boiling point of the solution is 100.712 ?C? Answer in units of %.
What are the subscripts in the empirical formula of this compound?
What can you say about the realtive magnitudes of the latice energy of lithium iodide and its heat of hydration?
unknown concentration of sodium hydroxide for complete neutralization. What is the molarity of the sodium hydroxide solution?
Iron is extracted from its ore using carbon. This can be represented using the following equation. Calculate the percent atom economy for pure iron.
Assuming the earth is a perfect sphere with a radius of 6371 km and an atmosphere that extends from the surface to an altitude of 20 km determine the number of metric tons of the elements/compounds+
Please explain the following technical terms used in mass spectrometry: a) Molecular ion,
At a temperature T, a previously empty 5.00L flask is prepared by adding 1.20 mol SO2 and 1.5 mol of O2. Determine the concentrations of SO2, O2 and SO3 once equilibrium is established. KC=963
The solubility of a certain compound in ice-cold water is .19g in 100mL. its solubility in hot water is 3.35g in 100mL.
Benzoic acid has a Ka value of 6.3x10^-5. A 35 ml sample of .13 M benzoic acid is titrated with a .15M solution of NaOH.Find the pH.
The mineral rhodochrosite [manganese (II) carbonate, MnCO2] is a commercially important source of manganese. Write a half reaction for the oxidation of the manganese in MnCO3 to MnO2 in neutral groundwater
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