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Ahat [919]
3 years ago
14

Write the concentration equilibrium constant expression for this reaction. 2cui (s) + i2 (aq) → 2cu+2 (aq) + 4i− (aq)

Chemistry
2 answers:
spayn [35]3 years ago
5 0
2CuI (s) + I₂ (aq) → 2 Cu⁺² (aq) + 4 I⁻ (aq)

When writing an equilibrium expression, we use the following values:

A (aq) + 3B (aq) → 2C (aq) + 2D (aq)

The numbers were arbitrary molar equivalents and the uppercase letters are the molecules in the reaction. The species used in the equilibrium expression but all be in the same state, e.g., solid, liquid, aqeuous.

Kc = [C]²[D]² / [A][B]³

We write the formula by taking the concentration of the products, each to the power of their molar equivalent, and multiply them together. We then divide the products by the concentration of the reactants, also to the power of their molar equivalent.

Going back to the initial equation given, we can now write a Kc expression.

Kc = [Cu⁺²]²[I⁻]⁴ / [I₂]

It should be noted that the CuI (s) in the reaction was left out of the Kc expression. Pure solids and liquids are left out of the expression and only the aqueous species are included. The reason being that, in this case, solid CuI does not affect the amount of reactant at equilibrium. Therefore, we just leave the concentration for [CuI] = 1, and remove it from the expression.
Alex Ar [27]3 years ago
5 0

Answer : The expression for equilibrium constant for this reaction will be,

K_{eq}=\frac{[Cu^{2+}]^2[I^-]^4}{[I_2]}

Explanation :

The given balanced equilibrium reaction is,

2CuI(s)+I_2(aq)\rightleftharpoons 2Cu^{2+}(aq)+4I^-(aq)

The general expression for equilibrium constant for this reaction will be,

K_{eq}=\frac{\text{Concentration of products}}{\text{Concentration of reactants}}

As we know that the concentration of solid is equal to 1.

So, the expression for equilibrium constant for this reaction will be,

K_{eq}=\frac{[Cu^{2+}]^2[I^-]^4}{[I_2]}

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Pcl5 exist but ncl5 does not.why?
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N is as electronegative as Cl is. So Cl doesnt react with O, N
6 0
3 years ago
A student is asked to determine the molarity of a strong base by titrating it with 0.250 M solution of H2SO4. The students is in
tamaranim1 [39]

Answer:

The molarity of the strong base is 0.625 M

Which procedural error will result in a strong base molarity that is too high?

⇒ Using a buret with a tip filled with air rather than the H2SO4 solution

Explanation:

<u>Step 1:</u> Data given

Molarity of H2SO4 = 0.250 M

The initial buret reading is 5.00 mL

The final reading is 30.00 mL

<u />

<u>Step 2:</u> Calculate volume of H2SO4 used

30.00 mL - 5.00 mL = 25.00 mL

<u>Step 3:</u> Calculate moles of H2SO4

0.250 M = 0.250 mol/L

Since there are 2 H+ ions per H2SO4

0.250 mol/L  * 2 = 0.500 mol/L

The number of moles H2SO4 = 0.500 mol/L * 0.025 L

Number of moles H2SO4 = 0.0125 mol

<u>Step 4</u>: Calculate moles of OH-

For 1 mol H2SO4, we need 1 mol of OH-

For 0.0125 mol of H2SO4, we have 0.0125 mol of OH-

<u>Step 5</u>: Calculate the molarity of the strong base

Molarity = moles / volume

Molarity OH- = 0.0125 mol / 0.02 L

Molarity OH - = 0.625 M

Which procedural error will result in a strong base molarity that is too high?

⇒ Using a buret with a tip filled with air rather than the H2SO4 solution

   

5 0
3 years ago
Determine whether the stopcock should be completely open, partially open, or completely closed for each activity involved with t
densk [106]

Answer:

Close to the calculated endpoint of a titration - <u>Partially open</u>

At the beginning of a titration - <u>Completely open</u>

Filling the buret with titrant - <u>Completely closed</u>

Conditioning the buret with the titrant - <u>Completely closed</u>

Explanation:

'Titration' is depicted as the process under which the concentration of some substances in a solution is determined by adding measured amounts of some other substance until a rection is displayed to be complete.

As per the question, the stopcock would remain completely open when the process of titration starts. After the buret is successfully placed, the titrant is carefully put through the buret in the stopcock which is entirely closed. Thereafter, when the titrant and the buret are conditioned, the stopcock must remain closed for correct results. Then, when the process is near the estimated end-point and the solution begins to turn its color, the stopcock would be slightly open before the reading of the endpoint for adding the drops of titrant for final observation.

3 0
3 years ago
Which best describes a compound such as magnesium oxide
Mamont248 [21]
A pure substance made up of different elements

hope this helped!!
7 0
3 years ago
Which model failed to explain the
11Alexandr11 [23.1K]

Answer:

C). The Bohr-Rutherford model

Explanation:

The 'Bohr-Rutherford model' of the atom failed to elaborate on the attraction between some substances. It essentially targeted hydrogen atoms and failed to explain its stability across multi-electrons. The nature and processes of the chemical reactions remained unillustrated and thus, this is the key drawback of this model. Thus, <u>option C</u> is the correct answer.

5 0
3 years ago
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