Calculate the equilibrium ¹³⁵I concentration and the equilibrium ¹³⁵Xe for 3.0 w/o enriched fuel in a reactor that operates with a thermal neutron flux of 1 x 10¹³/(cm²*s). Use the value of Σ_f = 3.

Please explain your work!

An aqueous sodium sulfide solution has a vapor pressure of 80.9mmHg at 50 ?C. The vapor pressure of pure water at this temperature is 92.6 mmHg. (Assume sodium sulfide completely dissociates.)

What is the concentration of sodium sulfide in mass percent?

Please show all work.

. The freezing point of benzene is 5.5^oC What is the freezing point of a solution of 5.00 g C₁₀H₈ in 444 g   of benzene. You will need to look up the freezing point depression constant for benzene in a reference book.                 Calculated FP:

Benzene K_f = ___________ *remember you will need “m”, which is in Kg     Name of reference used: __________________      

Calculated FP:    

i factor used and explain i factor:

1)Write the complete equation (balanced with states) for the reaction between potassium chloride and lead (II) nitrate?

2) Which precipitate forms in the above mentioned reaction?

3) You mix 16.00 mL of 0.778 M lead (II) nitrate with 18.00 mL of 0.813 M potassium chloride, and collect and dry the precipitate. Calculate the following:

a) Moles of lead (II) nitrate used:

b)Moles of potassium chloride used:

c) Moles of precipitate expected from lead (II) nitrate:

d) Moles of precipitate expected from potassium chloride:

e) Compare parts c and d to indicate the limiting reactant.

f) What mass of precipitate do you expect to obtain from this reaction?

g) If the actual yield of the precipitate you recover is 0.916g, what is the percent yield of the precipitate?

show work please

Liquid A has a normal boiling point of 64 deg C and liquid B has a normal boiling point of 98 deg C. a) which has the greater vapor pressure? b) which has the weaker intermolecular attractive forces in the liquid state?

Evaluate the fugacity for a gas of Ar at 100 bar and 298 K

1A. A 1.54 gram sample of an unknown gas is found to occupy a volume of 0.780 L at a pressure of 728 mm Hg and a temperature of 33°C. The molecular weight of the unknown gas is

1B.A sample of an unknown gas is found to have a density of 1.03 g/L at a pressure of 0.609 atm and a temperature of 38°C. The molecular weight of the unknown gas is

1c.A 7.64×10^-2 mol sample of O₂ gas is contained in a 2.00 L flask at room temperature and pressure. What is the density of the gas, in grams/liter, under these conditions?

What is the importance of the Sandmeyer Reaction?

What is the azide group and why it is a good leaving group?

Explain how the mechanism of the Sandmeyer reaction differs of a typical Electrophylic Aromatic Substitution reaction

Skeletal Equation: IO₃⁺(aq)+HSO₃^-(aq)->I^-(aq)+SO₄^2-(aq)

A) Which of the following correctly identifies the number of electrons transferred per entity?

6e-/S

2e-/S

4e-/I

3e-/I

B) Balance the Skeletal Equation

C) When the skeletal equation is balanced under acidic conditions, the amount of electrons transferred is ___ mol.

Unfortunately, I am unable to find anything in my textbook regarding the number of electrons transferred in a redox reaction, especially per entity. Would someone give me a hand?

A sample of an ideal gas occupies a volume of 25.0 liters at a pressure of 1.20 atm and a temperature of 75 degrees C. How many moles of gas are present in the container?

A sealed 1.0-L flask, initially containing 0.20 M COCl2, 0.20 M Cl2, and 0.20 M CO, is heated to 700 K

and allowed to come to equilibrium.

COCl2(g) ⇌ Cl2(g) + CO(g) Kc = 0.12 at 700 K

a. What are the molar concentrations of COCl2, Cl2, and CO once the reaction has reached equilibrium

at 700 K?

COCl2:_______________________________

Cl2:_______________________________

CO:_______________________________

b. 0.10 mol COCl2 is added to the equilibrium mixture. What are the molar concentrations of COCl2,

Cl2, and CO once equilibrium is re-established?

COCl2:_______________________________

Cl2:_______________________________

CO:_______________________________

After mixing 5.00 mL of the 5.0×10–5 M crystal violet solution with 5.00 mL of 0.20 M NaOH, what is the concentration of crystal violet and hydroxide ions in the solution at the start of the reaction? Is it a reasonable assumption that the concentration of OH– is much greater than that of CV+? Why is this an important assumption? Explain.

Consider the reaction

N₂(g) + 3H₂(g)

→

2NH₃(g)ΔH

= −92.6 kJ/mol

If 2.0 moles of N₂ react with 6.0 moles of H₂ to form NH₃, calculate the work done (in joules) against a pressure of 1.0 atm at 25 degrees celsius.

What is ΔU for this reaction? Assume the reaction goes to completion.

1. The pH of a solution made of 1.0 M acetic acid and 0.1 M potassium acetate is (K_a = 1.8 x 10^-5) to which 0.001 mol of KOH has been added: a) pH = 4.74 b) pH = 4.73 c) pH = 8.92 d) pH = 4.46 e) pH = 11.55 The answer is not 4.74!!

2. The pH of a solution made of 1.0 M acetic acid and 0.1 M potassium acetate is (K_a = 1.8 x 10^-5)​ to which 0.001 mol of HCl has been added: a) pH = 1.64 b) pH = 4.75 c) pH = 3.28 d) pH = 8.90