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At a certain temperature, the equilibrium constant for the following chemical equation is 3.80. At this temperature, calculate the number of moles of NO2(g) that must be added to 3.12 mol of SO2(g) in order to form 1.30 mol of SO3(g) at equilibrium.
If all connections in the apparatus are not airtight and some hydrogen gas escapes during the reaction
what is the balanced net ionic equation? AND what is the molarity of the tartaric acid solution?
What component of air will bring about this reaction and what is its approximate concentration in air? If you had a stoppered flask with basic luminol and then opened it to the air
Make an energy level diagram, showing ALL suborbitals, large enough to accomodate the 1st 36 elements
Acetylenic fatty acids are found in many tropical plants. Compound C, C18H30O2, is one such compound; it absorbs 3 equivalents of H2 when treated with H2 over a Pd/C catalyst. Ozonolysis of compound C produces the following products:
A red laser pointer emits light with a wavelength of 650 nm. What is the energy (in J) of a photon of light of this wavelength?
A 0.100 M solution of a weak acid, HX, has a pH of 2.110. What is the value of Ka for HX?
As the liquid vaporizes the plunger is pushed out. At equilibrium, the plunger reads 5.46 mL of gas. Atmospheric pressure is 740. mmHg. What is the approximate molar mass of the compound (in g/mol)?
Zinc chloride (ZnCl2) is 52.02% chlorine by mass. What mass of chlorine is contained in 66.0 g of ZnCl2?
The combustion of magnesium metal is described by the following equation. What mass of magnesium must be burned to produce 1.00 kJ of heat
A buffer solutions contains .120 M acetic acid and 0.150 M sodium acetate. How many moles of acetic acid and of sodium acetate are present in 50.0 ml of solution ? = 0.0075 moles.
calculate the mass of hydrogen gas that could have been produced. What would the gas volume be at room temperature and one atmosphere of pressure.
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