Calculate the standard reaction potential and use the half-reaction method to determine the moles of electrons per reaction.  2Al(s) + 6H+(aq) --> 2Al3+(aq) + 3H2(g)

Consider the following redox reaction, and answer the three questions below.2MnO−4​(aq)+2H2​O(l)+6H+(aq) -----> 2Mn2+(aq)+5H2​O2​(l)The standard reduction potentials of the species in the reaction above are:H2​O2​(l)+2H+(aq)+2e− ----> 2H2​O(l) E°red,H2​O2​​ = 1.776 VMnO−4​(aq)+8H+(aq)+5e−.   ----> Mn2+(aq)+4H2​O(l) E°red,MnO4- = 1.507 V Calculate E°. Calculate ΔG° Determine the equilibrium constant for the reaction.

Complete and balance the following half-reaction in acidic solution NH_3(g)->NO_3(aq)

Use the following standard reduction potentials to determine which species is the strongest oxidizing agent. Fe2+(aq) + 2 e– → Fe(s); E° = –0.41 V Pt2+(aq) + 2 e– → Pt(s); E° = 1.18 V Cr2O72–(aq) + 14 H+(aq) + 6 e– → 2 Cr3+(aq) + 7 H2O(); E° = 1.33 V Which of the following is the strongest oxidizing agent? Fe Pt Cr^3+ Fe^2+ Cr2O7^2-