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  3. Chemistry
  4. In a cell reaction, Cu(s)+2Ag+(aq) → Cu2+(aq)+2Ag(s) E°cell=+0.46 V If the concentration of Cu2+ ions is doubled then E°cell will be

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Q. In a cell reaction, $Cu_{\left(s\right)}+2Ag^{+}_{\left(aq\right)} \to Cu^{2+}_{\left(aq\right)}+2Ag_{\left(s\right)}\,E^{\circ}_{cell}=+0.46\,V$ If the concentration of $Cu^{2+}$ ions is doubled then $E^{\circ}_{cell}$ will be

Electrochemistry

Solution:

$E^{\circ}_{cell}=E^{\circ}_{cathode}-E^{\circ}_{anode}$
It will remain unchanged.