4.

Which reactions are redox reactions?

Choose at least one answer.

When tert-butanol is placed in the presence of excess equimolar amounts of chloride and bromide ions in aqueous acid experimental data indicates 45% tert-butyl chloride and 55% tert-butyl bromide is obtained. On the other hand, when n-butanol is placed in the presence of excess equimolar amounts of chloride and bromide ions in aqueous acid experimental data indicates 16% of n-butyl chloride and 84% n-butyl bromide is obtained. Now when n-butanol is placed in the presence of excess equimolar amounts of chloride ions and bromide ions in acid dimethyl sulfoxide the experimental data provides an 84% n-butyl chloride and 16% n-butyl bromide as the outcome.

1.) write balanced chemical equations for all three reactions (hint: account for mole ratios!).

2.) draw complete mechanisms for all three reactions.

3.) calculate the theoretical yield for the chlorides and bromides if each reaction was started with 5.55ml of the corresponding alcohol, using an aqueous acid media.

Sample: tert

Theoretical g of chloride

Theoretical g of bromide

Sample: n-

Theoretical g of chloride

Theoretical g of bromide

Carbonic acid, H₂CO₃, is a weak diprotic acid. In a 0.1 M solution of the acid, which of the following species is present in the largest amount?

A .053M solution of a weak base has a pH of 9.87. What is the Kb of this weak monprotic acid?

The formation constant* of [M(CN)6]4– is 2.50 × 1017, where M is a generic metal. A 0.130-mole quantity of M(NO3)2 is added to a liter of 1.150 M NaCN solution. What is the concentration of M2 ions at equilibrium?

1. Add 0.5 mL of 0.10 M NiCl2 solution to each of 7 test tubes using dropper provided. Label these tubes 1 through 7. 2. Add the following to the respective tubes containing the NiCl2 solution,

Tube 1: 5 drops of water (used here as a control experiment for dilution)

Tube 2: 1 mL of conc. HCl

Tube 3: 5 drops of conc. ammonia

Tube 4: 5 drops of dilute (5% v/v) ethylenediamine solution

Tube 5: 5 drops of 0.25 M C2O4 2- (oxalate) solution

Tube 6: 5 drops of 0.1 M SCN- (thiocyanate) solution

Tube 7: 5 drops of 0.1 M EDTA solution Mix each solution thoroughly and be sure to note the colour of each tube.

3. Check the stability of each complex by adding 3-5 drops of 1 M NaOH solution. Note any changes (e.g., formation of precipitate, colour change, etc.)

4. Add 0.5 mL of 0.10 M CuSO4 solution to each of 7 new test tubes labeled 8 through 14 using dropper provided. Repeat steps 2 and 3.

The “field strength” of a ligand describes how strong the coordination bond is, for a given metal and the ligand that is considered.  The field strength is evaluated by considering how much it causes the d orbitals to split (DE), which of the ligands is strongest?  Which is the weakest?  Explain your choices in each case.

The balanced equation for the neutralization reaction of aqueous H₂SO₄ with aqueous KOH is shown.

H₂SO₄(aq)====>2H₂O (l) +K₂SO₄(aq)

What volume of 0.370 M KOH is needed to react completely with 15.5 mL of 0.135 M H₂SO₄? Assume the reaction goes to completion.

Calculate the pH when 2.63 g of C₆H₅COONa is added to 41 mL of 0.50 M benzoic acid, C₆H₅COOH. Ignore any changes in volume. The K_a value for C₆H₅COOH is 6.5 x 10^-5

This question related to Diels-Alder Reaction of Anthracene and Maleic Anyhydride.

1. Show the product of the reaction of water with the anhydride product

2. The procedure warns against adding a lot of xylene during recystalization. Why?

3. What is the differences in the carbonyl region of the IR between the starting material and the product.

4. What specific band in the IR is unique to the product and confirms that you have made the product and do not have a mixture of the starting material? Explain.

5. Predict the product of the self-dimerization(via Diels-Alder reaction) of cyclopentadiene.;

Calculate the molar solubility of Ca(IO₃)₂ in

a) 0.060 M Ca(NO₃)₂

b) 0.060 M NaIO₃

If you eat a 48 g serving rice every fourth day and you weigh 75 kg, what is your dose of inorganic arsenic (in µg per kg body weight per day) if the rice contains 386 µg kg^-1 of total arsenic, 45% of which is inorganic arsenic.

The following picture represents a sample of gas at a pressure of 1 atm, a volume of 1 L, and a temperature of 25 ?C

What would happen to the pressure if the volume were reduced to 0.4L and the temperature increased to 260?C?

a cube of osmium metal 1.500 cm on one of its sides. It also has the mass of 76.31g at 25°C please help me solve this problem by showing your work so I can compare my answers.
a. what is the density g/cm³ at this temp
b. the density of titanium metal 4.51g/cm³ at 25°C. what mass of titanium 'displaces' 68.8mL of water at 25°C
c. the density of benzene at 15°C is 0.8787 g/mL. determine the mass of 0.1900L of benzene at this temp.
Thank you so much!

1a- Discuss the vaporization of water in standard condition at 298 K in term of: -A exothermicity and endothermicity -Achange of entropy of the system and the surrounding - A spontaneity of the reaction. 1b- Explain how the temperature and the composition of the two phases (liquid and vapour) influence the spontaneity of the vaporization of water. Please show steps and give ample explanation. Thank you

Please solve

What is the percent dissociation of HNO₂ when 0.074 g of sodium nitrite is added to 115.0 mL of a 0.068 M HNO₂ solution? K_a for HNO₂ is 4.0 × 10^–4. (4%)