Write a balanced net ionic equation for the oxidation of metallic copper to Cu(II) ion by hot concentrated H2SO4, in which the sulfur is reduced to SO2

Cu ==> Cu^2+ + 2e

H2SO4 + 2H^+ + 2e ==> SO2 + 2H2O
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Add the two half equations and cancel anything common to both sides. Finally, add extra sulfate ions, if needed to form CuSO4 on the right. I shall be happy to look at your final answer.

To write a balanced net ionic equation for the oxidation of metallic copper to Cu(II) ion by hot concentrated H2SO4, we need to follow a few steps:

Step 1: Write the balanced molecular equation:
Start by writing the chemical equation for the reaction between metallic copper (Cu) and hot concentrated sulfuric acid (H2SO4). In this reaction, copper is being oxidized, and sulfur is being reduced.
Cu + H2SO4 → CuSO4 + H2O + SO2

Step 2: Write the ionic equation:
Next, we need to separate the soluble compounds into their respective ions. CuSO4 and H2O are both soluble, so they will dissociate into their ions.
Cu(s) + H2SO4(aq) → Cu^2+(aq) + SO4^2-(aq) + H2O(l) + SO2(g)

Step 3: Write the net ionic equation:
Now, identify any spectator ions, which are ions that are present in both the reactants and products but do not participate in the reaction. In this case, the sulfate ion (SO4^2-) and water (H2O) are spectator ions. Since they are present on both sides of the equation, we can remove them from the equation.
Cu(s) + H2SO4(aq) → Cu^2+(aq) + SO2(g)

So, the balanced net ionic equation for the oxidation of metallic copper to Cu(II) ion by hot concentrated H2SO4, in which sulfur is reduced to SO2, is:
Cu(s) + 2H+(aq) → Cu^2+(aq) + SO2(g) + H2O(l)