Use the data in Appendix D to predict whether the following reactions can occur under standard-state conditions. (b) Reduction of Ni²⁺(aq) by Sn²⁺(aq)

Question

Accepted Answer

Welcome back. Everyone. Using the given reduction potentials below identify whether the reduction of silver carry on by copper carry on will occur spontaneously at standard state conditions. Notice that since the prompt says the reduction of silver Catalan occurs by copper caddy on. Copper carry on is our reducing agent, meaning that therefore, copper is going to become oxidized. So note that the prompt gives us our reduction potential for silver caddy into solid silver as 0.800 volts in our standard reduction potential for copper caddy in two copper two plus Catalan to our copper one plus Catalan as 10. 53 volts. So beginning with our reduction of silver caddy on, we have our silver caddy on gaining one electron to form solid silver as a product in which we have our standard reduction potential given in the prompt as 10.800 volts. Notice that because electrons are on the reaction side, it makes sense that this reaction occurs as a reduction. And now for our oxidation reaction, we have our copper plus one catty on which forms are copper, two plus catty on And Releases one Electron. So notice that elections are now on the product side. And so now we have a standard, put a standard cell potential for the oxidation of copper plus one carry on equal to. Now what's opposite for our reduction of copper two plus being negative 0.1 53 volts. So we would just flip the magnitude to be negative. Now, we need to come up with an overall reaction and we can do so easily by just adding up these reactions together since we have matching electrons in both equations. So for our overall reaction will come up with, we can cancel one electron with one electron here in the second reaction. And we're left with one mole of silver plus one cat ion reacting with one mole of copper plus one cat ion to form one mole of copper two plus Kati on plus solid silver. Now, we need to find our standard cell potential for this overall reaction degree cell which we recall is equal to the standard cell potential for reduction at our cathode subtracted from our standard cell potential. Standard cell potential for the oxidation are an ode. So plugging in our values for our standard reduction potential for our cathode, we have a value of 0.800 volts subtracted from our standard cell potential of our oxidation of copper plus one carry on equal to negative 0.1 53 volts. So taking the difference here, we get our standard cell potential equal to a value of 0.6 47 volts. And just to make a correction, our standard reduction potential at our cathode should be added to our standard potential of our oxidation at our a note. So these two terms are added to get to this value because our magnitude of our standard cell potential for this overall reaction is positive, we can say that S 0. 47 volts is positive. And so therefore, the reaction is spontaneous in the four direction. So thus, the reduction of silver caddy on by copper caddy on occurs spontaneously. And so this entire statement is going to be our final answer highlighted in yellow corresponding to choice A as the correct answer. I hope this made sense and let us know if you have any questions.

Use the data in Appendix D to predict whether the following reactions can occur under standard-state conditions. (b) Reduction of Ni²⁺(aq) by Sn²⁺(aq)

Verified Solution

Key Concepts

Standard-State Conditions

Reduction and Oxidation Reactions

Electrochemical Series

Use the data in Appendix D to predict whether the following reactions can occur under standard-state conditions. (b) Reduction of Ni2+(aq) by Sn2+(aq)

Verified Solution

Key Concepts

Standard-State Conditions

Reduction and Oxidation Reactions

Electrochemical Series

Use the data in Appendix D to predict whether the following reactions can occur under standard-state conditions. (b) Reduction of Ni²⁺(aq) by Sn²⁺(aq)