When you take $C{u}_{(aq)}^{2+}$ solution and add uranium metal to it$,$ a spontaneous reaction occurs and the solution color changes from blue to green. You measure the total cell voltage for this reaction to be $2\mathrm{.}00$ volts.

If uranium appeared in our data book on the Table of Selected Standard Electrode Potentials, what would its half$-$reaction look like and what potential $($voltage$)$ would be given for it$?$