Types of Redox Reactions

Q.

For the reaction $C_2{H}_6\left(g\right)+n{O}_2⟶C{O}_2\left(g\right)+H_{2}O\left(l\right)$, the ratio of the coefficients of $C{O}_2$ and $H_{2}O$ is:

1. 1:1

2. 2:3

3. 1:3

4. 3:2

Q.

When $KMn{O}_4$ acts as an oxidising agent and ultimately forms $[Mn{O}_4{]}^{-2},Mn{O}_2,M{n}_2{O}_3,M{n}^{+2}$ then the number of electrons transferred in each case respectively is

1. 4, 3, 1, 5

2. 1, 5, 3, 7

3. 1, 3, 4, 5

4. 3, 5, 7, 1

Q.

When $KMn{O}_4$ acts as an oxidising agent and ultimately forms $[Mn{O}_4{]}^{-2},Mn{O}_2,M{n}_2{O}_3,M{n}^{+2}$ then the number of electrons transferred in each case respectively is

1. 4, 3, 1, 5

2. 1, 5, 3, 7

3. 1, 3, 4, 5

4. 3, 5, 7, 1

Q.

For the reaction $C_2{H}_6\left(g\right)+n{O}_2⟶C{O}_2\left(g\right)+H_{2}O\left(l\right)$, the ratio of the coefficients of $C{O}_2$ and $H_{2}O$ is:

1. 1:1

2. 2:3

3. 1:3

4. 3:2

Q. Which of the following reaction is not disproportionation:

1. 
2. 
3. 
4. 

Q. The following is a partial redox equation:
$Mn{O}_4^{-}+8H^{+}+x{e}^{-}⟶M{n}^{2+}+4H_{2}O$

The value of the coefficient 'x' is:

1. 0

2. 5

3. 3

4. 1

Q.

For the redox reaction
$Mn{O}_4^{-}+C_2{O}_4^{-2}+H^{+}⟶M{n}^{2+}+C{O}_2+H_{2}O$
the correct coefficients of the reactants $Mn{O}_4^{-},C_2{O}_4^{2-}and{H}^{+}$ for the balanced reaction are

1. 2, 16, 5

2. 2, 5, 16

3. 16, 5, 2

4. 5, 16, 2

Q. The coefficients that will balance the following reactions are:
$aKMn{O}_4+b{H}_2{O}_2+c{H}_{2}S{O}_4\to dMnS{O}_4+e{H}_{2}O+f{O}_2+g{K}_{2}S{O}_4$

1. 2, 8, 5, 1, 5, 3, 2
2. 2, 5, 3, 2, 5, 8, 1
3. 1, 8, 5, 2, 5, 3, 2
4. 1, 8, 5, 2, 3, 5, 2

Q.

One mole of$N_2{H}_4$ loses 10 mol of electrons to form a new compound Y. Assuming that all nitrogen appears in the new compound, what is the oxidation state of$N_2$ in Y ? (There is no change in the oxidation state of hydrogen)

1. + 3

2. - 3

3. - 1

4. + 5

Q.

The number of moles of $KMn{O}_4$ reduced by one mole of $KI$ in alkaline medium is

1. One fifth

2. five

3. One

4. Two