Copper is too stable to react with dilute aqueous solutions of sulfuric acid (such as this one of concentration #0.500 color(white)(l) "mol" * "dm"^(-3)#) under standard conditions.
It takes concentrated sulfuric acid (which is indeed oxidizing but only at high concentrations) to directly react with copper and produce #"CuSO"_4#. Some orange-colored #"SO"_2(g)# gas evolves in this process. The reaction takes place as follows:
#stackrel(color(navy)(0))("Cu")(s) + 2 color(white)(l) "H"_2 stackrel(color(purple)(+6))("S") "O"_4("conc." ,aq ) #
#to stackrel(color(navy)(+2))("Cu") stackrel(color(grey)(+6))("S") "O"_4 (aq) + stackrel(color(purple)(+4))("S")"O"_2(g) + "H"_2"O"(l)#
This equation can be balanced by tracking changes in the oxidation state of #"Cu"# and #"S"#. From the reaction equation:
#(n(color(purple)("H"_2"SO"_4))) /(n(color(blue)("CuSO"_4))) = color(purple)(2)/color(blue)(1)#
#n(color(blue)("CuSO"_4)) = (m(color(blue)("CuSO"_4)))/(M(color(blue)("CuSO"_4))) = (15.0 color(white)(l) "g")/ (159.6 color(white)(l) "g" * "mol"^(-1)) = 0.0940 color(white)(l) "mol"#
#n(color(purple)("H"_2"SO"_4)) = n(color(blue)("CuSO"_4)) *(n(color(purple)("H"_2"SO"_4))) /(n(color(blue)("CuSO"_4))) = 0.0940 color(white)(l) "mol" * 2 = 0.188 color(white)(l) "mol"#
Meaning that it takes #0.188 color(white)(l) "mol"# of (concentrated) sulfuric acid to produce #15.0 color(white)(l) "g"# of #"CuSO"_4# through direct oxidation of copper metal #"Cu"#.
