Consider the following galvanic cell at 25°C. Pt | Cr2+ (0.35 M), Cr3+ (2.0 M) || Co2+ (0.24 M) | Co The overall reaction and equilibrium constant value are given below. 2 Cr2+(aq) + Co2+(aq) → 2 Cr3+(aq) + Co(s)    K = 2.79 ✕ 107 Calculate the cell potential ℰ for this galvanic cell and ΔG for the cell reaction at these conditions. ℰ       V ΔG       kJ Hello! I submitted this question once before. However, the answer was incorrect when I recieved an answer partially because they used the wrong values for the products and reactants to find Q. I tried to figure out the question myself and I got ℰ to be .07 V if we use 2 significant figures and ΔG to be -38.91 kJ. However, when I turned in these answers after the ones Bartleby helped me with were incorrect, these were also incorrect. I believe I am doing the right steps to reach the answer, but I guess there must be an error in my work. Please help me! Thank you.

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Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.