Making use of table of standard reduction potentials, predict (a) which of the f

Question

Making use of table of standard reduction potentials, predict (a) which of the following sets of reagents react spontaneously, and (t what the products of each reaction are. 1. Pb^2+ (aq)+2Cu_(s) rightarrow Pb^4+ 2 Cu+ 2. Cl_2 + 7Cr^3 rightarrow Cl_2 + should be Cl + Cr^3 3. Cl_(aq) + Br_(l) 4. Ni_(s) + Mg^2+_(aq) rightarrow Ni^2+ Mg Balance the following equations A. Sn^2+_(aq) + Cr_2 O_7^2_(aq) + H_3 O^+_(aq) rightarrow + 2Cr^3+_(aq) + H_2 O B. BiO_3_(aq) + MnO_2_(s) + H_3 O_(aq) rightarrow Bi^3+_(aq) + MnO_4_(aq) +H_2 O_3 C. Fe^2+_(aq) + Cr_2 O_7 + H_3 O rightarrow Cr^3_(aq) + Fe^3+ + H_2 O_(l) D. Cr (OH)_4 + BrO_3_(aq) + OH_(aq) rightarrow CrO_4^2_(aq) + Br_(aq) + H_2 O_(l) E. Cr^3+_(aq) + Na_2 O_2 (s) + OH (aq) rightarrow CrO_4_(aq) + Na_(aq) + H_2 O_(l) F. MnO_2 (s)+ H_3 O_(aq) + Cl^-_(aq) rightarrow Mn^2+_(aq) + H_2 O_(l) + Cl_2_(g) Calculate (a) E degree_cell (b) K_eq and (c) Delta G degree for the system 1) AgCl_(s) rightarrow Ag_(aq) +Cl^-_(aq)

Explanation / Answer

Q1.

Note that

LArgest potential will always REDUCE

lowest potential will Always OXIDIZE

i)

Pb2+ + 2 e Pb(s) 0.126

Cu2+ + 2 e Cu(s) +0.337

Clearly, Pb will oxidize, Cu will reduce

ii)

Cl2(g) + 2 e 2 Cl +1.36

Cr3+ + 3 e Cr(s) 0.74

Cr will reduce, and Cl will oxidize

iii)

Br2(aq) + 2 e 2 Br +1.0873

Cl2(g) + 2 e 2 Cl +1.36

Cl reduces, Br oxidizes

iv)

Ni2+ + 2 e Ni(s) 0.25

Mg2+ + 2 e Mg(s) 2.372

Mg will oxidize , Ni will reduce

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