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photoshop1234 [79]
2 years ago
6

What is the value of the equilibrium constant for the reaction between Cr(s) and Cu^2+ (aq) at 25 degree C? Cr(s) + Cu^2+ (q)rig

htarrow Cr^3+ (aq) + Cu(s) If your calculator has overflow issues with this problem, you can use this identity to solve for K: if log(K) = x + y then K = 10^x times 10^y 3 times 10^109 -6 times 10^5 2 times 10^18 1 times 10^2 3 times 10^40
Chemistry
1 answer:
Ludmilka [50]2 years ago
3 0

Answer:

3 × 10¹⁰⁹

Explanation:

2Cr (s) → 2Cr³⁺ + 6e⁻        

and,

Ec° for the above reaction = 0.74 V

also,

3Cu²⁺ (aq) + 6e⁻ →   3Cu(s)

and,

Ea° for the above reaction = 0.34 V

Now,

The cell potential, E° = 0.34 + 0.74 = 1.08

E° = \frac{\textup{0.059}}{\textup{n}}\log k

thus,

0.34 = \frac{\textup{0.059}}{\textup{n}}\log k

here, n is the number of electrons exchanged

n = 6

1.08 = \frac{\textup{0.05921}}{\textup{6}}\log k

or

㏒ k = 109.44

taking anti-log both sides

we get

k =  3 × 10¹⁰⁹

Hence, the answer is option (A) 3 × 10¹⁰⁹

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The pOH of an aqueous solution at 25°C was found to be 1.20. The pH of this solution is . The hydronium ion concentration is M.
frosja888 [35]

Answer:

pH = 12.80

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Explanation:

Step 1: Data given

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Step 2: Calulate pH

pH + pOH = 14

pH = 14 - pOH

pH = 14 - 1.20 = 12.80

Step 3: Calculate hydronium ion concentration

pH = -log[H+] = -log[H3O+]

12.80 = -log[H3O+]

10^-12.80 = [H3O+] = 1.58 * 10^-13 M

Step 4: Calculate the hydroxide ion concentration

pOH = 1.20 = -log [OH-]

10^-1.20 = [OH-] = 0.063M

Step 5: Control [H3O+] and [OH-]

[H3O+]*[OH-] = 1* 10^-14

1.58 *10^-13 * 0.063 = 1* 10^-14

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