Question

The equilibrium constant at 25°C for the given cell is:

Zn | Zn²⁺ (1M) | | Ag⁺ (1M) |

Ag is ______ × 10⁵².

Given that

\[\ce{E^0_{Zn/Zn^{2+}}}\] = 0.76 V

and \[\ce{E^0_{Ag/Ag^{+}}}\] = −0.80 V

Options

• 5.15

• 6.17

• 7.92

• 8.65

Answer 1

The equilibrium constant at 25°C for the given cell is:

Zn | Zn²⁺ (1M) | | Ag⁺ (1M) |

Ag is 6.17 × 10⁵².

Given that

\[\ce{E^0_{Zn/Zn^{2+}}}\] = 0.76 V

and \[\ce{E^0_{Ag/Ag^{+}}}\] = −0.80 V

Explanation:

E⁰ = (0.76 + 0.80) = 1.56

\[\ce{E^0_{cell}}\] = `0.0591/"n" log "k"`

`(1.56 xx 2)/0.0591` = log k

log k = 52.79

k - 6.17 × 10⁵²