Suppose you have the following reagents available under standard conditions. (i.

Question

Suppose you have the following reagents available under standard conditions.
(i.e., P = 1 atm for all gases; t = 25 o
C; C = 1 mol L?1 for all aqueous species, including H+.)
Co(s), Ag+(aq), Cl?(aq), Cr(s), BrO3?(aq), I2(s), F?(aq)
Consult the standard reduction potentials on the next page and then answer the following questions.
(a) (2 marks) Which is the strongest oxidizing agent?
(b) (2 marks) Which is the strongest reducing agent?
(c) (6 marks) Which of the available reagent(s), if any, will oxidize Fe(s) while leaving Pb(s)
unreacted? If none of the available reagents can be used for this purpose, then identify another
reagent from the table that could be used. For one of the reagents you

Explanation / Answer

Co(s), Ag+(aq), Cl?(aq), Cr(s), BrO3?(aq), I2(s), F?(aq)

Co2+ + 2 e?   --->   Co(s)   E0 = ?0.28 v

Ag+ + e? ---->   Ag(s)   E0 = +0.7996 v

Cl2(g) + 2 e? ----> 2 Cl-   E0 = +1.36 v

Cr3+ + 3 e? -----> Cr(s)   E0 = ?0.74 V

BrO3- + 5 H+ + 4 e? --> HBrO(aq) + 2 H2O E0 = +1.45 v

I2(s) + 2 e? --> 2 I-   E0 = +0.54 v

F2(g) + 2 e? ---> 2 F-   E0 = +2.87 v

a) higher SRP , strongest oxidizing agent = BrO3-

b) lower SRP, strongest reducing agent = F-

c) Te reagent whose reduction potential is higher than Fe+2,lower than Pb+ 2 can do this. but in the given list its not available.

but Cd+ 2 can do this.

Fe(s) + Cd+2(aq) ----> Cd(s) + Fe+2(aq)

Pb(s) + Cd+2(aq) ----> No reaction.

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