The EMF of a cell can be calculated using the Nernst equation:

E = E° - (RT/nF) * ln(Q)

where:
E° is the standard cell potential,
R is the gas constant (8.314 J/(mol·K)),
T is the temperature in Kelvin,
n is the number of moles of electrons transferred in the balanced redox reaction,
F is the Faraday constant (96485 C/mol), and
Q is the reaction quotient.

Given:
E° = 1.10 V,
T = 25°C = 298.15 K,
n = 2 (from the balanced redox reaction),
[Cu2+] = 0.1 M, and
[Zn2+] = 0.1 M.

We can substitute these values into the Nernst equation:

E = 1.10 V - (8.314 J/(mol·K) * 298.15 K / (2 * 96485 C/mol)) * ln([Cu2+]/[Zn2+])

Since [Cu2+] = [Zn2+], the ln term becomes ln(1) = 0, and the equation simplifies to:

E = 1.10 V - 0 = 1.10 V

So, the EMF for the cell reaction, when 0.1M Cu2+ and 0.1M Zn2+ solutions are used, at 25°C is 1.10 V.

Question

The EMF of a cell can be calculated using the Nernst equation:

E = E° - (RT/nF) * ln(Q)

where:
E° is the standard cell potential,
R is the gas constant (8.314 J/(mol·K)),
T is the temperature in Kelvin,
n is the number of moles of electrons transferred in the balanced redox reaction,
F is the Faraday constant (96485 C/mol), and
Q is the reaction quotient.

Given:
E° = 1.10 V,
T = 25°C = 298.15 K,
n = 2 (from the balanced redox reaction),
[Cu2+] = 0.1 M, and
[Zn2+] = 0.1 M.

We can substitute these values into the Nernst equation:

E = 1.10 V - (8.314 J/(mol·K) * 298.15 K / (2 * 96485 C/mol)) * ln([Cu2+]/[Zn2+])

Since [Cu2+] = [Zn2+], the ln term becomes ln(1) = 0, and the equation simplifies to:

E = 1.10 V - 0 = 1.10 V

So, the EMF for the cell reaction, when 0.1M Cu2+ and 0.1M Zn2+ solutions are used, at 25°C is 1.10 V.

Knowee AI · Accepted Answer

The EMF of a cell can be calculated using the Nernst equation:

E = E° - (RT/nF) * ln(Q)

where:
E° is the standard cell potential,
R is the gas constant (8.314 J/(mol·K)),
T is the temperature in Kelvin,
n is the number of moles of electrons transferred in the balanced redox reaction,
F is the Faraday constant (96485 C/mol), and
Q is the reaction quotient.

Given:
E° = 1.10 V,
T = 25°C = 298.15 K,
n = 2 (from the balanced redox reaction),
[Cu2+] = 0.1 M, and
[Zn2+] = 0.1 M.

We can substitute these values into the Nernst equation:

E = 1.10 V - (8.314 J/(mol·K) * 298.15 K / (2 * 96485 C/mol)) * ln([Cu2+]/[Zn2+])

Since [Cu2+] = [Zn2+], the ln term becomes ln(1) = 0, and the equation simplifies to:

E = 1.10 V - 0 = 1.10 V

So, the EMF for the cell reaction, when 0.1M Cu2+ and 0.1M Zn2+ solutions are used, at 25°C is 1.10 V.

The standard EMF for the given cell reaction Zn+Cu2+⇒Cu+Zn2+ is1.10 V at 25∘C. The EMF for the cell reaction, when 0.1MCu2+ and 0.1M Zn2+ solutions are used, at 25∘C is1.10 V0.110 V−1.10 V−0.110 V

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