Table 1. Standard Reduction Potentials. E(Volts) +2.87 +1.36 +1.07 +0.80 +0.77 +
ID: 1046853 • Letter: T
Question
Table 1. Standard Reduction Potentials. E(Volts) +2.87 +1.36 +1.07 +0.80 +0.77 +0.34 0.00 0.44 -0.76 1.66 -2.37 -2.87 2.93 Half-Reaction F2(g) + 2e ? 2F (ag) CL(g)+2e 2C(ag) Br(/) + 2e ? 2Br(aq) Ag (aq)+e Agls) Fe"(aq) + e? Fe2+(aq) Cu"(aq) + 2e->Cu(s) H (aq)+2eH,(g) Fe2 (aq)+2eFe(s) Zn"(aq) + 2e ? Zn(s) AP"(aq) + 3e-> Al(s) Mg2+(aq) + 2e ? Mg(s) Ca2(ag)+ e Cas) K lag)+e K(s) 11) Which of the halogens in Table 1 is the strongest oxidizing agent? A) Br 8) 2 E) All of have equal strength as oxidizing agents 12) Which one of the following types of elements is most likely to be a good oxidizing agent? A) transition elements B) alkaline earth elements C) lanthanides D] alkali metals E)halogens 13) The standard cell potential (E cell) for the voltaic cell based on the reaction below is Sn2 (aq)+ 2 Fe (aq))2 Fe (aq)+Sn (aq) A) +1.39 8).046 C)+0.617 D)+1.21 E)-0.46 14) The standard cell potential (E° cell) for the voltaic cell based on the reaction below is V. 3 Sn (aq) 2 Cr (s)2 Cr (aq)+3 Sn2 (aq) A) +0.89 B) +1.94 c)-0.59 D) +2.53 E)-1.02Explanation / Answer
13)
standard cell potential = E0 (Fe3+ / Fe2+) - E0 (Sn4+ / Sn2+) = 0.77 - 0.13 = 0.64 volt.
option C is the answer
14)
standard cell potential = E0 (Sn4+ / Sn2+) - E0 (Cr3+ / Cr) = 0.13 - (-0.74) = + 0.87 volt
option A is the answer.
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