a. 2.4 M
b. 0.004 M
c. 1.0 M
d. 0.07 M
e. 0.1 M
What is the [Cu2+] in the cell Zn(s) | Zn2+(1.0 M) || Cu2+(aq) | Cu(s) The standard emf of the cell is 1.10 V. Ecell = 1.03 V.?
2020-09-11 3:59 pm
回答 (1)
2020-09-11 4:28 pm
Balance equation for the cell reaction:
Zn(s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu(s)
Nernst equation:
Ecell = E°cell - (0.0592/n) log₁ₒ([Zn²⁺]/[Cu²⁺])
1.03 = 1.10 - (0.0592/2) log₁₀(1.0/[Cu²⁺])
0.0296 log₁₀(1.0/[Cu²⁺]) = 0.07
log₁₀(1.0/[Cu²⁺]) = 2.37
log₁₀[Cu²⁺] = -2.37
[Cu²⁺] = 10⁻²·³⁷ M
[Cu²⁺] = 0.004 M
The answer: b. 0.004 M
Zn(s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu(s)
Nernst equation:
Ecell = E°cell - (0.0592/n) log₁ₒ([Zn²⁺]/[Cu²⁺])
1.03 = 1.10 - (0.0592/2) log₁₀(1.0/[Cu²⁺])
0.0296 log₁₀(1.0/[Cu²⁺]) = 0.07
log₁₀(1.0/[Cu²⁺]) = 2.37
log₁₀[Cu²⁺] = -2.37
[Cu²⁺] = 10⁻²·³⁷ M
[Cu²⁺] = 0.004 M
The answer: b. 0.004 M
收錄日期: 2021-05-01 09:35:50
原文連結 [永久失效]:
https://hk.answers.yahoo.com/question/index?qid=20200911075924AA5Sjkd