Copper dissolves in dilute Nitric acid but not in dilute `HCl`. Why?

Explanation

Since `E^(@)` of `Cu^(2+)//Cu` electrode (+0.34 V) is higher than that of `H^(+)//H_(2)` electrode (0.0V) therefore `H^(+)` ions cannot oxidise Cu to `Cu^(2+)` ions and hence Cu does not dissolve in dil HCI in contrast the electrode potential of `NO_(3)^(-)//NO` electrode (+0.97 V) is higer than that of copper electrode and hence it can oxidise Cu to `Cu^(2+)` ions and hence Cu dissolve in dil `HNO_(3)` thus cu dissolves in dil `HNO_(3)` due to oxidation of Cu by `NO_(3)^(-)` ions and not by `H^(+)` ions