Chew. Iu, Pre-Lecture Exercise 1. Consider the following spontaneous redox react

Question

Chew. Iu, Pre-Lecture Exercise 1. Consider the following spontaneous redox reaction and galvanic cell sketched below a. Given the redox reaction above, write the oxidation half-reaction. b. Given the redox reaction above, write the reduction half-reaction. b. c. Idensify the oxidizing agent (OA) d. Identify the reducing agent (RA). Electrode #1 is the (anode or cathode). Electrode r2 is the--(anode or cathode). Electrons now through the external circuit from (+ or-). h. As the galvanic cell operates, electrode 2loses or gains) weight. The nitrate anions (NOS) in the salt bridge flow to compartment- -(#1 or #2). With respect to the external circuit, electrode #1 is labeled ( + or-). Electrode #1 is a (an)--, active, inert, or gas) electrode. Electrode #2 is a (an)--(active, inert, or gas) electrode. j. k. d. h. k. Na NO electrode e lee trode i SnLs)

Explanation / Answer

(a)

Oxidation Half reaction:

Cr (s) ------------> Cr3+ (aq.) + 3 e-

(b)
Reduction half reaction:

Sn2+ (aq.) + 2 e- ----------> Sn (s)

(c)

Oxidising agent is the one which undergoes reduction, so, Sn2+

(d)

Reducing agent is the one which undergoes oxidation, so, Cr

(e)

Cr/Cr3+ is anode

(f)

Sn2+/Sn is cathode

(g)

Cr to Sn

(h)

Sn electrode gains weight

(i)

Cr electrode loses weight

(j)

Cr/Cr3+ is labelled as ( - )

(k)

Cr electrod eis active

(l)

Sn electrode is inert electrode

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