help!!! Before Beginning this experiment is the laboratory, you should be able t

Question

help!!!

Before Beginning this experiment is the laboratory, you should be able to answer the following questions: Determine the oxidation number of the indicated element in each of the following compounds. The reduction of the silver ions is the following reaction occurs at the (anode or cathode) Zn(s) + Ag 2+ (aq) rightarrow Zn2+(aq) + Ag(s) In an electrochemical cell, occurs at the mode and occurs at the cathode. An voltaic cell was set up in which one half-cell had a nickel metal electrode that was suspended in NiCl2(aq). The standard reduction potentials at 25 degree C are Ag 1+(aq) + 1e - rightarrow Ag(s) E degree red = +0.80 V Ni 2+(aq) + 2e- rightarrow Ni(s) E degree red = -0.28 V Write the chemical equation for the reaction occurring at the anode. Write the chemical equation for the reaction occurring at the cathode Determine the standard cell potential for this electrochemical cell. Write the balanced chemical reaction for this electrochemical cell.

Explanation / Answer

1. a. +5

     b. +6

Explanation:

      In AlPO4 having Al 3+ PO43- , hence Oxidation number of P is P5+    ( 5 + 4 (-2) = - 3

     In Cr2O72-   Oxidation number of Chromium is Cr6+                (( 2x 6 + 7x (-2)) = -2

2. Cathode

3.Oxidation occurs at anode and reduction occurs at cathode.

4.

i. Anode reaction Ni (s)/ Ni 2+ (aq):

the Ni metal loses mass becoming Ni+2 .... the nickel metal loses electrons, which makes it the stronger reducing agent

ii. Cathode reaction: Ag+ (aq)/ Ag (s):

the silver ions attract electrons, forming more silver metal, which makes the silver electrode gains in mass

iii. Standard Cell potential = 1.06V (Reduction pot - Oxidation pot )

iv. 2Ag{+}(aq) + Ni(s) --> 2Ag(s) + Ni{2+}(aq)

   

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