± Pressure-Based versus Concentration-Based Equilibrium Constants

Part A.) For the reaction

3A(g)+3B(g)⇌C(g)

Kc = 67.6 at a temperature of 287 ∘C .

Calculate the value of Kp.

Part B.) For the reaction

X(g)+3Y(g)⇌3Z(g)

Kp = 1.65×10⁻² at a temperature of 209 ∘C .

Calculate the value of Kc.

these solutions (2-5) will each be in their own 50 mL volumetric flask.

assigned pH for buffer system: 4.75

acid/base pair to use: acetic acid and sodium acetate

Sample calculation for acid (solution 2-5):

Sample calculation for base (solution 2-5):

You will prepare 4 different 50 mL solutions from the table above. Once you have the calculated amount of acid (g or mL) and base (g or mL) in the correct flask, what should you do to finish preparing each solution? Describe the steps you will take to make this solution.

Finally, transfer each solution to a container for storage.

What is the concentration of each of the following solutions? (a) The molality of a solution prepared by dissolving 25.0 g of H2SO4 in 1.30 L of water (b) The mole fraction of each component of a solution prepared by dissolving 2.25 g of nicotine, C10H14N2, in 80.0 g of CH2Cl2

Consider a buffer solution that contains 0.25 M C₆H₄(CO₂H)(CO₂K) and 0.15 M C₆H₄(CO₂K)₂. pK_a(C₆H₄(CO₂H)CO₂^-)=5.41.

1. Calculate its pH

2. Calculate the change in pH if 0.140 g of solid NaOH is added to 190 mL of this solution.

3. If the acceptable buffer range of the solution is ±0.10 pH units, calculate how many moles of H₃O⁺ can be neutralized by 250 mL of the initial buffer.

The hydrolysis of table sugar (sucrose) occurs by the following overall reaction sucrose + water → glucose + fructose and is first order in sucrose concentration with a rate constant of 3.50 × 10⁻³ min⁻¹. If a 0.500 M solution of sucrose is allowed to react for 345 min, what will be the average rate of production of glucose over that period of time in units of M/min?

A) What is the pH of a solution created by combining 1.28 mole of HOBr and 0.52 mole NaOH in a 1.00L solution? K_{a HOBr} = 2.5 x 10^-9

B) What is the pH of a buffer made by combining 0.62 moles HOBr with 0.88 moles NaOBr in a 100.00mL solution? K_{a HOBr} = 2.5 x 10^-9

Part A

Write the anode and cathode reactions that cause the corrosion of iron metal to aqueous iron (II).

Express your answer as a chemical equation. Identify all of the phases in your answer.

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Part B

Express your answer as a chemical equation. Identify all of the phases in your answer.

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Part C

Write the balanced half-reactions involved in the air oxidation of Fe2+(aq) to Fe2O3?3H2O.

Express your answer as a chemical equation. Identify all of the phases in your answer.

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Part D

Express your answer as a chemical equation. Identify all of the phases in your answer.

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a) I found this data when comparing 5 different reactions, using various concentrations

When S₂O₈] remains constant (0.0400M):

Reaction 1 and 2: The [I^-] concentration doubles from 0.0400M to 0.0800M, while the rate and relative rate triple at 4.31e-6M/s to 1.32e-5M/s and 2.00 to 6.14

Reaction 2 and 3: The [I^-] concentration quadruples from 0.0200M to 0.0800M, while the rate and relative rate multiply by 6 from 2.15e-6M/s to 1.32e-5M/s and 1.0 to 6.14

Does this prove that the [I^-] concentration is proportional to the rate in a fashion of 3/2, 2/3 or another ratio?

b) Using this data, In the rate law
rate=k[I^-]ⁿ[S₂O₈^2-]^m
what is the value of n?

how many grams of sodium bromide are there in 55.0mL of a 1.90M aqueous solution? please answer as soon as possible and show work thank you

1. Define and compare elemental, inductive and resonance effects.

2. Define and compare various intermolecular forces.

3. Illustrate how intermolecular forces effect physical properties.

4. Draw and name all isomers of C5H12.

5. Define and discuss kinetic vs thermodynamic control of a reaction.

CH 14

The reaction 2H2O2(aq)→2H2O(l)+O2(g) is first order in H2O2 and under certain conditions has a rate constant of 0.00752 s−1 at 20.0 ∘C. A reaction vessel initially contains 150.0 mL of 30.0% H2O2 by mass solution (the density of the solution is 1.11 g/mL). The gaseous oxygen is collected over water at 20.0 ∘C as it forms.

What volume of O2 will form in 83.2 seconds at a barometric pressure of 725.2 mmHg . (The vapor pressure of water at this temperature is 17.5 mmHg)

1) How many liters of 0,.775 M solution can be prepared from 55.0 g of MgBr2?

2) Calculate the molarity of all ions present when 12.5g of potassium chlorate is dissolved in 85.0 ml of solution

3) What is the molarity of a solution prepared by diluting 50.0 ml of 0.300 M sodium nitrate (NaNO3) to 60.0ml?

4) A solution is made by mixing 50.0 ml of 0.300 M Na2So4 with 30.0 ml of 0.900 M K2SO4. Assuming that the volumes are additive, what are the molar concentrations of the following ions in the new solution? a. Na+ ion, b. K+ ion, c. SO42- ion

Please make sure to display your thought process? It is imperative to be able to follow how the answer was deduced. Please be as thorough as possible. Please address all parts as they are critical to answering this question correctly:

1) Discuss the type of surface treatments that are applied to nanoclays in order to improve nanoclay dispersion in polymer matrices. What happens when untreated nanoclay is used to reinforce a polymer? What happens when a properly organically modified clay is used? List and discuss three techniques that are used to characterize the microstructure/nanostructure of nanoclay-filled polymers.