Given:E0Zn2+/ Zn = -0.76VE0Ag+/Ag = 0.80VWhich of the following reactions actually takes place?
Zn(s) + 2Ag+ (aq) → Zn2+ (aq)+ 2Ag(s)
Zn2+ (aq) + 2Ag(s) → Zn(s) + 2Ag+(aq)
Zn (s) + Ag(s) → Zn2+ (aq) + Ag+(aq)
Zn2+ (aq) + Ag(s) → Ag+ (aq) + Zn+ (aq)
The brown ring complex compound is for mulated as [Fe(H2O)5 (NO)] SO4. The oxidation number of iron is
+2
+6
+3
+12
The standard electrode potential of Cu / Cu2+ electrode is - 0.34 V. Its corresponding reaction is
Cu → Cu2+ + 2e -
Cu2+ +2e- → Cu
Given that
Which is the strongest reducing agent?
Zn
Cr
H2
Fe 3+
The oxidising agent in the following reactions is H2O2 + O3 → H2O +2O2
H2O2
O3
Both H2O2 and O3
Unpredictable
A substance that will reduce Ag+ to Ag but will not reduce Ni+2 to Ni is
Pb
Mg
AI
3Br2 + 6NaOH → NaBrO3 + 5NaBr + 3H2O in this reaction, the element which loses as well as gains electron is
Na
Br
O
H
