. Three moles of an ideal gas (CV,m =3/2R ) is compressed at 25℃, at pressure of 1 atm to 75 atm, with a surrounding maintained at 25℃. The process was performed at condition (i) Reversible and (ii) against constant external pressure of 0.80 atm. Calculate the following q, W, ∆U,∆H, for each path

“Atomic fission” is when a nucleus gets hit by a neutron and splits in half, releasing a great deal of energy. It is the basic principle behind nuclear reactors and nuclear weapons. The “Fat Man” atomic bomb dropped on Nagasaki in 1945 had a plutonium core of 6.4 kg of the isotope Pu-239. (Note that “239” is the molar mass.) When the bomb exploded, it released an amount of energy equivalent to 21 kilotons of TNT.

Although the bomb needed 6.4 kg of plutonium to function at all, only a portion of those plutonium atoms actually fissioned. Calculate how many kilograms of Pu-239 actually underwent fission when the bomb exploded.

You will need some conversion factors to do this problem:

The energy from the explosion of 1 kiloton of TNT is equal to 4.2 x 10¹²J.

The fission of a single atom of Pu-239 releases 210 MeV (mega electron volts) of energy.

1 MeV = 1.602 x 10^-13 J

What is the pH of a 0.15 M solution of potassium nitrite (KNO2)? (The Ka value for nitrous acid (HNO2)

is 4.0x10^-4).

A sample of pure NO2NO2 is heated to 336 ∘C∘C at which temperature it partially dissociates according to the equation
2NO2(g)⇌2NO(g)+O2(g)2NO2(g)⇌2NO(g)+O2(g)
At equilibrium the density of the gas mixture is 0.525 g/Lg/L at 0.755 atm

Calculate Kc for the reaction.

The following data were obtained from experiments to find the molecular formula of an unknown compound which acts as a common local anesthetic. The unknown compound contains only carbon, hydrogen, nitrogen, and oxygen. Complete combustion of a 4.82 g sample of the unknown compound with excess oxygen formed 12.67 g of carbon dioxide and 4.076 g of water. Another sample of the unknown compound with a mass of 1.12 g was found to contain 0.1339 g of nitrogen. The molar mass of the unknown compound was found to be 234 g/mol. Find the molecular formula of the unknown compound.

The laundry bleach is listed at 5.25% m/m NaClO. Calculate the concentration of the NaClO in the laundry bleach solution in mol/L. Assume the density of the bleach solution is of 1.05 g/L.

Consider the following system at equilibrium where K_c = 0.159 and delta H° = -111 kJ/mol at 723 K.

N₂(g) + 3 H₂(g) = 2 NH₃(g)

The production of NH₃(g) is favored by:

Indicate True (T) or False (F) for each of the following:

___TF 1. increasing the temperature.
___TF 2. decreasing the pressure (by changing the volume).
___TF 3. increasing the volume.
___TF 4. adding NH₃.
___TF 5. removing H₂.

Given that Buffer A contains 200 ml of 0.05 M HOCl and 400 ml 0.03 M NaOCl, calculate the pH of the buffer solution, the pH of the solution after adding 10 mL of 0.5 M HCl, and the pH of the solution after adding 20 mL of 0.4 M NaOH.

Given that Buffer B contains 200 mL 0.5 HOCl and 400 mL 0.3 M NAOCl, calculate the pH of the buffer solution, the pH of the solution after adding 10 mL of 0.5 M HCl, and the pH of the solution after adding 20 mL of 0.4 M NaOH.

Which buffer will resist pH changes better?

place the following compounds in order of increasing (weakest to strongest) strength of intermolecular forces
c2h6, ch3oh ch3f

Calculate the pH at the equivalence point for the titration of 0.100 M methylamine (CH3NH2) with 0.100 M HCl. The Kb of methylamine is 5.0

Carbonyl fluoride, COF 2 , is an important intermediate used in the production of fluorine-containing compounds. For instance, it is used to make the refrigerant carbon tetrafluoride, CF 4 via the reaction 2COF 2 (g)⇌CO 2 (g)+CF 4 (g), K c =9.00 If only COF 2 is present initially at a concentration of 2.00 M , what concentration of COF 2 remains at equilibrium? Thanks! ( I keep getting .1 but that is incorrect)

What is the wavelength in meters of 91.0 kJ/mol

A solution contains 0.026 M  Hg2+2 and 0.019 M Pb2+. If you add Cl−, Hg2Cl2 and PbCl2 will begin to precipitate.

A) What is the concentration of Cl− required, in molarity, when Hg2Cl2 precipitation begins?

B) What is the concentration of Cl− required, in molarity, when Hg2Cl2 precipitation is 99.99% complete?

C) What is the concentration of Cl− required, in molarity, when PbCl2 precipitation begins?

D) What is the concentration of Cl− required, in molarity, when PbCl2 precipitation is 99.99% complete?

Finally, give the Cl− concentration range in which Hg2+2 can be completely separated from Pb2+ by precipitation.

E) Give the lowest Cl− concentration for the separation of Hg2+2 from Pb2+

F) Give the highest Cl− concentration for the separation of Hg2+2 from Pb2+.

Lactic acid, C3H6O3, occurs in sour milk as a result of the metabolism of certain bacteria. Calculate the pH of a solution of 56 mg lactic acid in 250.0 mL water. Ka for D-lactic acid is 1.4 × 10-4.

I mostly need help with solving the quadratic formula portion of this problem