When Cu reacts with AgNO3 solution, the reaction takes place is:

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411.

When Cu reacts with AgNO3 solution, the reaction takes place is:

  • oxidation of Cu

  • reduction of Cu

  • oxidation of Ag

  • reduction of NO3-


A.

oxidation of Cu

Cu is placed above Ag in electrochemical series, hence it can replace Ag from its salts solution. Therefore the reaction occur as follows:

Cu0 + AgNO3 oxidation CuNO3+1 + Ag


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412.

For a cell involving one electron E°cell = 0.59 V at 298 K, the equilibrium constant for the cell reaction is :[ Given that 2.303F= 0.059V at T = 298 K].

  • 1.0 × 105

  • 1.0 × 1010

  • 1.0 × 1030

  • 1.0 × 102


413.

For the cell reaction

2Fe3+ (aq) +2l-(aq) → 2Fe2+(aq) + I2(aq)

Ecell= 0.24V at 298 K. The standard Gibbs energy (ΔrGΘ) of the cell reaction is:

[Given that Faraday constant F = 96500 C mol–1]

  • – 23.16 kJ mol–1

  • 46.32 kJ mol-1

  • 23.16 kJ mol-1

  • - 46.32 kJ mol-1


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