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

1. Put a circle around the Lewis Acids and a Box around the Lewis Bases:

Ca²⁺                 S^2-               OH^-                      Fe³⁺                      I^-

Consider the following reaction:
CO(g)+H2O(g)⇌CO2(g)+H2(g)
Kp=0.0611 at 2000 K
A reaction mixture initially contains a CO partial pressure of 1346 torr and a H2O partial pressure of 1762 torr at 2000 K.

A.) Calculate the equilibrium partial pressure of CO2.

B.) Calculate the equilibrium partial pressure of H2

With respect to proteomics and Mass Spec, what is Data Dependent Acquisition and how does it affects dynamic range of proteome measurements?

The Ka of a monoprotic weak acid is 2.50 × 10-3. What is the percent ionization of a 0.176 M solution of this acid?

A compound with the formula XOCl3 is synthesized, isolated and purified.

When 3.270 g of this compound are decomposed chemically, a solution of chloride ions is produced.

The chloride ions are precipitated with silver ions and 9.170 g of silver chloride, AgCL, are produced.

What are the identity and molar mass of the element X?

This is likely on my final and my professor did not explain how to solve in class, he just laid it out there and 96% of the class failed the question. Thank you for any help!

sodium hydroxide dissolves very easily, and exothermically, in water. Using values from the appendix in your text, calculate the Ksp for this salt, as well as the temperature at which this reaction becomes spontaneous. Does the temperature need to be above or below this value in order for the process to proceed without outside intervention? Na0H(s): -379.4 kJ/mol