What is the standard cell potential ( )for the following below, 2Ag(s)+ Pb²⁺(aq)$\to$ 2Ag⁺(aq)+ Pb(s) Given the following standard reduction potentials. Ag⁺(aq)+ e^-$\to$ Ag(s)$~~~~~~~~$$~~~~~~~~$E $\circ$ =0.8 V Pb²⁺(aq)+2e^-$\to$ Pb(s)$~~~~~~~~$$~~~~~~~~$E $\circ$ =-0.126 V A) -0.926 V B) 0.926 V C) -1.726 V D) 1.726 V E) 1.474 V

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Quizplus · Accepted Answer

The standard cell potential can be calculated by subtracting the reduction potential of the anode from the reduction potential of the cathode. In this case, the anode is Pb(s) with a reduction potential of -0.126 V, and the cathode is 2Ag⁺(aq) with a reduction potential of 0.8 V. Therefore, the standard cell potential is: 0.8 V - (-0.126 V) = 0.926 V However, since the reaction is written in reverse, the sign of the standard cell potential must be flipped to obtain the correct answer: -0.926 V

What Is the Standard Cell Potential ( )For the Following