Redox Reactions and Couple

Q.

2 K₄ [Fe (CN)₆]_(aq) + H₂O_{2 (aq)} → 2 K₃ [Fe (CN)₆]_(aq) + 2KOH_(aq) is an example of

1. Replacement

2. Oxidation

3. Addition

4. Reduction

Q.

Which of the following reactions involves oxidation-reduction

1. 

2. 

3. 

4. 

Q. 38. Balance this reaction by oxidation number method, FeS2+O2=Fe2O3+SO2

Q. WHAT IS THE OXIDATION NUMBER OF Fe IN REACTANT SIDE OF THE REACTION OF RUSTING OF IRON?

Q. what is differance between oxidation and partial oxidation?

Q. Oxidation state of Fe in Fe3O4 is 8/3. What about the oxidation no. of Fe in Fe3O4?

Q. 16 Which is higher oxidation state -1 or -2 ?

Q.

Which of the following changes represents reduction?

1. MnO₄^-1(aq) → MnO₂(s)

2. I^-1(aq) → I₂ (s)

3. Fe²⁺ (aq) → Fe³⁺(aq)

4. Br^-(aq) → BrO₃^-(aq)

Q.

Oxidation number of N in $(N{H}_4{)}_{2}S{O}_4$ is

1. +1

2. −1/3

3. −1

4. −3

Q. The measured voltage for the reaction with the indicated concentrations is $1.5\text{V}$. Calculate $E_{\text{cell}}^{\circ }\text{in V}$.
$Cr\left(s\right)+3A{g}^{+}(aq,0.1\text{M})\to 3Ag\left(s\right)+C{r}^{3+}(aq,0.1\text{M})$

1. $1.54$
2. $1.65$
3. $1.35$
4. $1.46$

Q. Oxidation state of S in $N{a}_2{S}_2{O}_3$ is

1. 5
2. -1
3. \N
4. 2

Q. Which of the following set of metal electrodes can be used in the given galvanic cell?
Given:
$M{g}^{2+}\left(aq\right)+2e^{-}\to Mg\left(s\right);E^0=-2.37V$
$C{u}^{2+}\left(aq\right)+2e^{-}\to Cu\left(s\right);E^0=0.34V$
$A{g}^{+}\left(aq\right)+e^{-}\to Ag\left(s\right);E^0=0.80V$

1. $A-Ag$
   $B-Cu$
2. $A-Ag$
   $B-Mg$
3. $A-Mg$
   $B-Ag$
4. $A-Mg$
   $B-Cu$

Q. To know that the oxidation state of cr2 o7 (6) is reduced to 3 do we need to byheart the following reaction??Cr2O72- + 6Fe2+ + 14H+ ----> 2Cr3+ + 6Fe3+ + 7H2O

Q. Oxidation state of Fe in $FeS{O}_4(N{H}_4{)}_{2}S{O}_4.6H_{2}O$ is

1. 2
2. 1
3. -2
4. -1

Q. Select the correct statement for a galvanic cell involving the following reaction:
$Zn\left(s\right)+C{u}^{2+}\left(aq\right)\rightleftharpoons Z{n}^{2+}\left(aq\right)+Cu\left(s\right)$

1. The given redox process is spontaneous
2. $C{u}^{2+}\left(aq\right)+2e^{-}\to Cu\left(s\right),$ takes place at anode
3. Zinc rod act as sink for electrons
4. $Zn\left(s\right)\to Z{n}^{2+}\left(aq\right)+2e^{-},$ takes place at cathode

Q. In case of castner's process the following is true.

1. Nickel : anode
2. Iron : anode

3. Iron : cathode

4. Nickel : cathode

Q. what is oxidation reduction?

Q. The Oxidation state of Mn in $K_{2}Mn{O}_4$ is

1. 2
2. 7
3. -2
4. 6

Q. How to find the possible oxidation states of an element?

Q.

Give the relation between oxidation potentional and reduction potentional??