First, per a educational source
copper does not react with dilute sulphuric acid
As such, you may wish to follow a path employed for the commercial leaching of copper ore. The reaction is accomplished with copper metal in aqueous ammonia, optionally an ammonium salt (carbonate), an electrolyte (like $\ce{NaCl}$) and air (or, dilute $\ce{H2O2}$ works just fine).
The underlying chemistry was debated for decades but is now resolved to consist of a mixed reaction involving some spontaneous electrochemistry (and so, for the associated electrolyte, I use a pinch of sea salt). Here is a review article from ResearchGate. Also, this article, "Kinetics and Mechanism of Copper Dissolution In Aqueous Ammonia".
The cited provided chemistry is even a little more complex (and unfortunately, in my opinion, does require an exposition due to safety issues involving implementation and handling) with a mention of a minor secondary radical related reactions resulting in an unstable nitrite ($\ce{NH4NO2}$). My take is that the $\ce{O2/Cu}$ reaction with $\ce{NH3}$ is, in effect, a metal/air battery. The latter can introduce solvated electrons into the mix (as sourced from copper, so it is correct to claim that copper is catalytic to the oxidation of ammonia to nitrite from $\ce{O2/H2O2}$). The battery cell provided $\ce{e-(aq)}$ with $\ce{H+}$ produces the hydrogen atom radical, which can react with $\ce{NH3}$ forming $\ce{•NH2}$ radical, which can further interact with $\ce{O2/H2O2}$ as follows:
$\ce{•NH2 + O2 → NH2O2•}$ (aminylperoxyl radical unstable) → $\ce{NO + H2O }$
As a supporting reference on the above, see "On the aqueous reactions of the aminyl radical with molecular oxygen and the superoxide anion", particularly Page 24, Table 2.1.
where the $\ce{NO}$ is a precursor to nitrite, and in particular, a small amount of unwanted $\ce{NH4NO2}$. The latter has the annoying property (based on a lowing of the pH following ammonia consumption) of suddenly decomposing releasing volumes of $\ce{N2}$ gas, which apparently is sufficient so as to cause leakage and even breakage of sealed reaction vessels (as I have experienced).
Consequentially, don't tightly seal your suitably large reaction vessel (and I would recommend avoiding any skin contact with the solution due to also potentially toxic ammonium nitrite here (unclear as to whether its toxicity extends to a skin ingestion pathway).
Note, the ascribed electrochemical reaction has an inception period (waiting time).
Have problems with ammonia? An alternate electrochemical path is Copper metal, lemon juice, dilute $\ce{H2O2}$, a piece of carbon (large surface area) and some sea salt. Heat (especially for a few minutes in a microwave, if possible, which eliminates the inception period) and you will have a colorful solution of copper citrate/ascorbate.
