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What is the expected freezing point of a 0.50 m solution of Li2SO4 in water? Kf for water is 1.86°C/m.
Evaluate the energy of an electron excited from a hydrogen atom using Bohr's model. Determine the maximum wavelength of energy needed to observe a photoelectric effect for potassium.
what are the structural formulas for the following compound : 6-bromo-2-methyl-3-heptyne
The heat of solution of ammonium chloride is 15.2 kJ/mol. If a 6.253 g sample of NH4Cl is added to 65.0 mL of water in a calorimeter at 26.9°C.
when 15.0g of steam drops in temperture from 275.0C to 250.0C how much heat is released csteam=2.01j/gC
Rb has two naturally occurring isotopes 85Rb and 87Rb, with masses 84.9118 amu and 86.9092 amu, respectively. The average atomic mass is 85.468 amu.
Determine the molar concentration of chloride ions after adding 225 ml of 0.625 MKCL with 615 ml of 0.385M MgCl2 if final volume of the solution is 840ml.
Calculate the concentrations of all species in a 1.66 M Na2SO3 (sodium sulfite) solution. The ionization constants for sulfurous acid are Ka1=1.4x10^-2 and Ka2=6.3x10^-8.
Calculate the standard free energy change for the process N2O5(s)-->N2O5(g) at 25 0C if Vapor pressure of N2O5 at 7.5 degrees C is 100mmHg, and the solid sublimes at a pressure of 1.00 atm at 32.4 0C.
What mass of Aluminum is produced when 0.5 mole of Al2S3 is completely reduced with excess H2?
Which of the following isotopes is more likely to decay via positron emission rather than electron emission.
Write the overall reaction, showing how much ATP (Adenosine tri phosphate) can be produced per pentose used also write an equation for the generation of NADPH using ribose as a sole source of carbon?
how do you find the specific heat of platinum if 23.6 grams is heated from 10.0c to 20.0c using 30.68 J of heat.
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