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Question- Determine the freezing point of a solution that contains 62.8 g of urea (CH4N2O) dissolved in 275 g of water (Kf = 1.85 degree C/m)
Please provide the balanced reaction.
A particular first-order reaction has a rate constant of 1.35 x10^2 s^-1 at 25 degrees Celsius. What is the magnitude of k at 75.0 degress Celsius if Ea= 85.6 kJ/mol
What is the final temperature of the copper and water after they come to thermal equilibrium? (the specific heat of copper is 0.385 J/gxK).
Calculate mass of chromium III hyrodixide, c- Calculate the molar concentration of ions remaining in solution after reaction has taken place (total cocentrations of Cr3+, OH, K, NO3-)
for the reaction X(g) + 3Y(g) equilibrium 3Z(g). Kp=2.08x10^-2 at a temperature of 277 degrees Celsius. Calculate the value of Kc
25mL of a .10M solution of the weak acid hydrofluoric acid, HF, is titrsted with .10M solution of the weak base amonia, NH3. Will the pH at the equivilance point be less than 7 equal to 7 or greater than 7? Explain. Ka for HF is 7.2e-4 and Kb for ..
You have 500 mL of a 5.0 M solution of nitric acid HNO3 (63.01 g /?mol) dissolved in water. How many grams of nitrogen does the solution contain.
The addition of chlorine gas to magnesium bromide will it cause a reaction and if so what will the product be
How many air molecules are in a a11.5*12.0*10.0 ft room. Assume atmospheric pressure at 1.00 atm, a room temperature of 20 degrees celsius, and ideal behavior
Assume you had a balloon made of some highly flexible semiperiable membrane. The balloon is filled entirely with a 0.2 M solution of some solute as well as is submerged in a 0.1 M solution of the same solute. Initially the volume of the solution i..
Determine the pH at the equivalence (stoichiometric) point in the titration of 30.9 mL of 0.804 M HCOOH by 0.369 M LiOH. The Ka of HCOOH is 1.8 x 10-4.
Look carefully at the frontier MOs of the diatomic molecule, BF and determine the most basic site. Based on your observations, predict the structure that results when H+ adds to BF.
A weak acid with a starting concentration is 12.5% dissociated. a) Calculate the [H3O+], pH, [OH-] and pOH of the solution. ([OH-] = 1.1 × 10-13 M, pOH = 12.96
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