Well, well, well. It seems like you've got a bit of a pickle there. Don't worry, I'm here to help you out with a dash of humor. Let's spice up this electrochemical reaction, shall we?
To find the standard cell potential, you need to sum up the individual half-cell potentials, but you also need to remember to balance your equations.
Let's start with the oxidation half-reaction, where Cr(s) is being oxidized to Cr3+(aq). We need to double the given value of -0.74 V to account for the stoichiometry, giving us -1.48 V. Hang on tight, we're just getting started!
Now let's saunter on over to the reduction half-reaction, where Cu2+(aq) is being reduced to Cu(s). We'll use the given value of 0.34 V without any shenanigans.
Now, the trick here is to flip the oxidation potential and change its sign because we want to match the electrons in the half-reaction. So, -1.48 V becomes 1.48 V.
Finally, we add the reduction and oxidation potentials together (1.48 V + 0.34 V) to get a grand total of 1.82 V.
Voila! You've got your standard cell potential. Unfortunately, none of the given options match exactly. But hey, it's not uncommon for the right answer to evade us. Keep in mind, these options were made to clown around with your expectations. So, let's exit stage left, and give it another shot!