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Consider your experimental results from part A of this lab. Suppose your strongest reducing agent were added to your strongest oxidizing agent. (Use...
1. Consider your experimental results from part A of this lab. Suppose your strongest reducing agent were added to your strongest oxidizing agent. (Use the lowest possible coefficients. Omit states-of-matter from your answers.)(a) Write the half-reaction for your strongest reducing agent. (b) Write the half-reaction for your strongest oxidizing agent.(c) Note the number of electrons in each half reaction.In order to balance the number of electrons lost and gained, the oxidation half-reaction must be multiplied by 1,2,3,4, or 5 and the reduction half-reaction must be multiplied by 1,2,3,4,or 5.(d) Write the net redox reaction.2.Students should always be careful of the chemical reaction between jewelry and laboratory reagents. The Standard Reduction Potentials Table shows the reduction reactions and potentials for some common lab reagents and metals.(a) What is the net redox reaction that occurs when Au comes into contact with acidic KMnO4? (Use the lowest possible coefficients. Omit states-of-matter from your answer.)(b) What is E°cell for the reaction?WebAssign will check your answer for the correct number of significant figures. 2 V(c) Which metal is the least reactive?AgAuCuNiPt(d) Which reagent is the most reactive?Cr2O72SO42-3.During part B of your lab, you measured electrochemical cell potentials with a Cu2+/Cu couple as the anode. Predict the results you would observe if Zn2+/Zn were the anode.
