To find the equilibrium constant (K) for the reaction, we can use the Nernst equation. However, since we're dealing with standard conditions, we can simplify the process by using the formula:

K = exp((n*F*E°cell) / (R*T))

Where:
- n is the number of moles of electrons transferred in the reaction. In this case, it's 2.
- F is Faraday's constant, which is approximately 96485 C/mol.
- E°cell is the standard cell potential, which is given as 1.20 V.
- R is the gas constant, which is 8.314 J/(mol*K) when dealing with electrochemical reactions.
- T is the temperature in Kelvin. Since we're at standard conditions, this is 298.15 K.

Substituting these values into the formula, we get:

K = exp((2*96485*1.20) / (8.314*298.15))

Calculating this gives a K value of approximately 2.4 × 10^44.

Question

To find the equilibrium constant (K) for the reaction, we can use the Nernst equation. However, since we're dealing with standard conditions, we can simplify the process by using the formula:

K = exp((n*F*E°cell) / (R*T))

Where:
- n is the number of moles of electrons transferred in the reaction. In this case, it's 2.
- F is Faraday's constant, which is approximately 96485 C/mol.
- E°cell is the standard cell potential, which is given as 1.20 V.
- R is the gas constant, which is 8.314 J/(mol*K) when dealing with electrochemical reactions.
- T is the temperature in Kelvin. Since we're at standard conditions, this is 298.15 K.

Substituting these values into the formula, we get:

K = exp((2*96485*1.20) / (8.314*298.15))

Calculating this gives a K value of approximately 2.4 × 10^44.

Knowee AI · Accepted Answer

To find the equilibrium constant (K) for the reaction, we can use the Nernst equation. However, since we're dealing with standard conditions, we can simplify the process by using the formula:

K = exp((n*F*E°cell) / (R*T))

Where:
- n is the number of moles of electrons transferred in the reaction. In this case, it's 2.
- F is Faraday's constant, which is approximately 96485 C/mol.
- E°cell is the standard cell potential, which is given as 1.20 V.
- R is the gas constant, which is 8.314 J/(mol*K) when dealing with electrochemical reactions.
- T is the temperature in Kelvin. Since we're at standard conditions, this is 298.15 K.

Substituting these values into the formula, we get:

K = exp((2*96485*1.20) / (8.314*298.15))

Calculating this gives a K value of approximately 2.4 × 10^44.

For the reaction below at standard conditions, what would be K?2Ag+(aq) + Cd(s) → Cd2+(aq) + 2Ag(s) ; E°cell = 1.20 V3.9 × 10402.0 × 10202.4 × 10441.6 × 1022

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