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Compute the mass in g of precipitate formed when excess sodium hydroxide is added to 42.5mL of 15.5% magnesium nitrate solution whose density is 1.12 g/mL.
What is the change in energy for a constant pressure process where H = 23 J and 11 J of work are performed on the system? Hint: What is enthalpy equal to when pressure is constant
Halogenated compounds are particularly easy to identify by their mass spectra because chlorine and bromine occur naturally as mixtures of two abundant isotopes
Calculate the approximate volume of 0.02M KMnO4 (in the unit of mL) needed to titrate 0.17 g sodium oxalate.(Note: The KMnO4 solution will be added from a buret to a flask during titration.
Presume that all the carbon ends up in CO2 and all the hydrogen ends up in H2O. Also presume that all the nitrogen ends up in the NH3 in the second experiment.
The volume of a gas is 93 mL when the temperature is 91 C. if the temperature is reduced to 0 C without changing the pressure, what is the new volume of the gas
what is the energy uncertainty associated with a short pulse of laser light that lasts 4.8fs
How much heat energy is liberated when 11.0 grams of manganese is used in the formation of Mn2O3
An antacid tablet requires 25.82 mL of a .200 M HCl to titrate to its equivalence point. What Volume in mL of stomach acid can be neutralized by the antacid tablet? assume that stomach acid has a pH of 1.1.
a) The nitric oxide molecule, NO, readily loses one electron to form the NO+ ion. Why is this consistent with the electronic structure of NO. Predict the order of the N--O bond strengths in NO, NO+, and NO-, and describe the magnetic properties of e..
Bill's recipe for onion soup calls for 4.0 lb of thinly slicedonions. If an onion has an average massof 115 g, how many onions does Bill need
Volume of a certain mass of a gas is desired to be decreased by 25% of the initial volume of 10l at 1.5 bar and room temprature by what percentage the pressure should be incraesed
Presume that 25 g of each of the subsequent substances is initially at 27 degrees C. Define what is the final temperature of each upon absorbing 2.35 kJ of heat.
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