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Use the following reaction to find out how many grams of H2O you need to react with 5.67*10^-2 moles of Li2O Li2O + H2O ---------> 2LiOH
the value of the molar absorptivity is 4.84*10^3 M^-1 cm^-1 for K2CrO4 at that wavelength. what is the concentration of the solution
A 2.30-g sample of a large biomolecule was dissolved in 22.0 g of carbon tetrachloride. The boiling point of this solution was determined to be 77.85°C. Calculate the molar mass of the biomolecule.
How many structures can be drawn from C4H10O and how can you differentiate the molecules in a labratory
The density of chloroform, a widely used organic solvent, is 1.4832 at 20 . How many milliliters would you use if you wanted 119.0 of chloroform.
The density of solid Fe is 7.87 g/cm3. How many atoms are present per cubic centimeter of Fe. As a solid, Fe adopts a body-centered cubic unit cell. How many unit cells are present per cubic centimeter of Fe
a sample of argon is at a pressure of 1.24*10^4 kPa of 24 degrees c in a rigid 25-L tank. How many moles of argon does this tank contain?
how much heat in kj would be required to vaporize 1.00 l of diethyl ether c4h10o density is 0.714gml at 298 k if the
Consider various salts of octahedral complexes of Pt(IV) which, per mole of Pt(IV), contain one mole each of the bidentate ligands en and oxalate ion (ox) in the "1st coordination sphere" and, as possible monodentate ligands, SO4 2- and/or NC- and..
To determine the freezing points of distilled water, 1m glucose, 1m NaCl, 1m CaCl2. Use the freezing point of the pure water as a baseline to determine deltaTf for each of the solutions
The vapor pressure of dichloromethane,CH_2Cl_2, at 0 degrees C is 134 mmHg. The normal boiling point of dichloromethane is 40. degrees C. Calculate its molar heat of vaporization.
ICE Problem: Calculate Final Concentrations, Phosgene, COCl2 (g), is an extremely toxic gas. It was used during World War I. Today it is used to manufacture pesticides, pharmaceuticals, dyes, and polymers. It is prepared by mixing carbon monoxide ..
For the decomposition of 10.9 Pa azomethane, CH3N2CH3, at 600 K the partial pressure is found
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