#18.37 Balance each of the following redox reactions occurring in acidic aqueous solution.

A) Cd(s)+Cu+(aq)→Cd2+(aq)+Cu(s)

B) I−(aq)+SO42−(aq)→H2SO3(aq)+I2(s)

Select all of the correct statements about equilibrium from the choices below.

At equilibrium the rates of forward and reverse reactions are equal.



As a reaction proceeds forward toward equilibrium the product concentrations rise.



At equilibrium no more reactants are transformed into products.



As a reaction proceeds forward toward equilibrium the forward rate drops.



At equilibrium the rate of change of reactant concentration is zero.



At equilibrium all reactions stop.

One of the assumptions of the kinetic molecular theory is that there are no intermolecular forces (attractive or repulsive) between gas particles (atoms or molecules). How would the presence of intermolecular forces affect the ideal gas equation (PV = nRT)? Again, in your response, please use terms that a high school senior who hasn’t taken AP chemistry might use.

Predict the number of d-electrons AND number of unpaired electrons on the metal in each of the following complexes (explanations helpful!):

1. [Cr(H₂O)₄F₂]

2. [Rh(en)₃]³⁺

3. [Pt(CN)₄]^2-

4. [TiCL₄]^3-

In a Mohr titration of chloride with silver nitrate, an error is made while preparing the indicator. Instead of 0.011 M chromate indicator in the titration flask at the endpoint, there is only 0.0011 M. If the flask contains 100 mL at the end point, what is the error in the titration in milliliters of 0.100 M silver nitrate?

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1)Consider the formation of hydrogen fluoride:

H₂(g) + F₂(g) ? 2HF(g)

If a 2.8 L nickel reaction container (glass cannot be used because it reacts with HF) filled with 0.0085 M H₂ is connected to a 3.6 L container filled with 0.030 M F₂. The equilibrium constant, K_p, is 7.8 x 10¹⁴ (Hint, this is a very large number, what does that imply?)Calculate the molar concentration of HF at equilibrium.

2)Suppose a 5.00 L nickel reaction container filled with 0.0052 M H₂ is connected to a 3.00 L container filled with 0.287 M F₂. Calculate the molar concentration of H₂ at equilibrium.

how many grams of Al can be produced in an electrolytic cell containing a solution of aluminum chloride if a current of 10.0 A is applied for 5 hours?

For the following chemical equation:

CaCO3(s) + 2HCl(aq).......>H2)(l) +CO2 (g) +CaCl2 (aq)

A). How many liters of CO2 can form at STP when 18.5 mL of a 3.51 M HCl solution reacts with excess CaCO3?

B). What is the molarity of a HCl solution if the reaction of 210 mL of the HCl solution with excess CaCO3 produces 12.1 L of CO2 gas at 725 mmHg and 18 C?

When you mutate a Gly residue that immediately follows an alpha-helix to an Ala residue, the protein becomes less stable of 2.0 kcal/mol. Explain the molecular basis of this result.

A sample of a peptide of unknown sequence was treated with trypsin; another sample of the same peptide was treated with chymotrypsin.

The sequences (N-terminal to C-terminal) of the smaller peptides produced by trypsin digestion were as follows:

Cys—Thr—Ala—Ser—Ile—Lys

Arg—Thr—Arg—Gln—Arg

Gln—Phe—Ala—Val—Tyr—Asn—Lys

Phe—His—Cys—Asn

The sequences of the smaller peptides produced by chymotrypsin digestion were as follows:

Asn—Lys—Cys—Thr—Ala—Ser—Ile—Lys—Phe

Arg—Thr—Arg—Gln—Arg—Gln—Phe

His—Cys—Asn

Ala—Val—Ty

The reversible chemical reaction

A+B⇌C+D

has the following equilibrium constant:

Kc=[C][D][A][B]=5.9

Initially, only A and B are present, each at 2.00 M. What is the final concentration of A once equilibrium is reached?

Part B

What is the final concentration of D at equilibrium if the initial concentrations are [A] = 1.00 M and [B] = 2.00 M ?

Suppose you have a solution containing CuBr42- and CuSO4 at room temperature. You want to isolate a solution of only CuSO4. You have the following AgNO3 (s), a pot of boiling water, a bucket of ice, and a coffee filter. Using only the things listed suggest a way to isolate a solution of pure CuSO4. (K+ is a spectator ion and will be present in all solutions. Ksp Ag2SO4 1.5 ×10-5 and Ksp AgBr 5.0 × 10-13).

During reflux, you oxidized ethanol to acetic acid, using postassium dichromate.

A) How many grams of ethanol can be oxidized by 100.00mL of a 0.750M K₂Cr₂O₇ solution?

B) In a similar reaction, a chemist oxidizes methanol (CH₃OH) to formic acid (HCOOH), also using K₂Cr₂O₇. Starting with half reactions, write a balanced redox equation for the reaction performed by the chemist. Show all steps

i. Which reactant is the oxidizing agent

ii. Which reactant is the reducing agent?

33)

(a) A piston at 5.9 atm contains a gas that occupies a volume of 3.5 L. What pressure would have to be placed on the piston to force the volume to adjust to 0.32 L?
_____________ atm

(b) A piston at -44.0°C contains a gas that occupies a volume of 2.5 L. To what temperature would the gas have to be heated to increase the volume to 4.4 L at constant pressure?
__________ °C

(c) A piston at 795 torr contains a gas that occupies a volume of 4.7 L. What pressure would have to be placed on the piston to force the volume to adjust to 0.78 L?
___________atm

a. 0.130 g of HCl is in 35.0 mL of water. This is mixed with 50.0 mL of 0.185 M Sr(OH)₂. What is the pH of the resulting solution?

b. Calculate the pH of a solution prepared by mixing 125.0 mL of 0.0120 M HCl with 25.0 mL of 0.0420 M Ba(OH)_2?

_c.