Ion Electron Method

Q.

How would you balance: ${\mathrm{H}}_2+{\mathrm{O}}_2\to {\mathrm{H}}_2\mathrm{O}$

Q.

How would you balance the following equation: $\mathrm{Fe}+{\mathrm{O}}_2\to {\mathrm{Fe}}_2{\mathrm{O}}_3$

Q. Sulphuric acid reacts with sodium hydroxide as follows:

$H_{2}S{O}_4+2NaOH\to N{a}_{2}S{O}_4+2H_{2}O$

When 1L of 0.1M sulphuric acid solution is allowed to react with 1L of 0.1M sodium hydroxide solution, the amount of sodium sulfate formed and its molarity in the solution obtained is

1. 7.10 g
2. 3.55 g
3. $0.1mol{L}^{-1}$
4. $0.025mol{L}^{-1}$

Q.

Balance the following redox reactions by ion-electron method:
$Mn{O}_4^{-}\left(aq\right)+I^{-}\left(aq\right)\to Mn{O}_2\left(s\right)+I_2\left(s\right)$ (in basic medium)

$Mn{O}_4^{-}\left(aq\right)+S{O}_2\left(g\right)\to M{n}^{2+}\left(aq\right)+\left(aq\right)HS{O}_{4\left(aq\right)}^{-}$ (in acidic solution)

$H_2{O}_2\left(aq\right)+F{e}^{2+}\left(aq\right)\to F{e}^{3+}\left(aq\right)+H_{2}O\left(l\right)$ (in acidic solution)

$C{r}_2{O}_7^{2-}+S{O}_2\left(g\right)\to C{r}^{3+}\left(aq\right)+S{O}_4^{2-}$ (aq) (in acidic solution)

Q.

How would you balance the following equation: ${\mathrm{NH}}_3+{\mathrm{H}}_2{\mathrm{SO}}_4\to {\left({\mathrm{NH}}_4\right)}_2{\mathrm{SO}}_4$

Q.

Which of the following expression correctly represents the equivalent conductivity at infinite dilution of $A{l}_2(S{O}_4{)}_3$?

Given that ${\lambda }_{A{l}^{3+}}^{\circ }$ and ${\lambda }_{S{O}_4^{2-}}^{\circ }$ are the equivalent conductivities at infinite dilution of the respective ions.

1. $2{\lambda }_{A{l}^{3+}}^{\circ }+3{\lambda }_{S{O}_4^{2-}}^{\circ }$
2. ${\lambda }_{A{l}^{3+}}^{\circ }+{\lambda }_{S{O}_4^{2-}}^{\circ }$
3. $({\lambda }_{A{l}^{3+}}^{\circ }+3{\lambda }_{S{O}_4^{2-}}^{\circ })\times 6$
4. $\frac{1}{3}{\lambda }_{A{l}^{3+}}^{\circ }+\frac{1}{2}{\lambda }_{S{O}_4^{2-}}^{\circ }$

Q.

Balance the following equations in basic medium by ion-electron method and oxidation number methods and identify the oxidising agent and the reducing agent.
$P_{4\left(s\right)}+OH{-}_{\left(aq\right)}⟶P{H}_{3\left(g\right)}+HP{O}_{2\left(aq\right)}^{-}$

$N_2{H}_{4\left(I\right)}+CI{O}_{3\left(aq\right)}^{-}⟶N{O}_{\left(g\right)}+C{I}_{\left(g\right)}^{-}$

$C{l}_2{O}_{7\left(g\right)}+H_2{O}_{2\left(aq\right)}⟶CI{O}_{2\left(aq\right)}^{-}+O_{2\left(g\right)}+H_{\left(aq\right)}^{+}$

Q. Number of Faradays needed to reduce $1$ mole of nitrobenzene into aniline is:

Q. The equivalent weight of chlorine molecule in the given equation is
$3C{l}_2+6NaOH\to 5NaCl+NaCl{O}_3+3H_{2}O$

1. $42.6$
2. $35.5$
3. $59.1$
4. $71$

Q. The given redox reaction

$B{r}_2+O{H}^{-}\to Br{O}_3^{-}+B{r}^{-}+H_{2}O$
is balanced by ion electron method. Choose the correct statement(s) regarding stoichiometric ratios $\frac{n_a}{n_b}$ :
Here $a,b$ represents different species in the reaction.

1. $\frac{n_{B{r}_2}}{n_{Br{O}_3^{-}}}=\frac{3}{2}$
2. $\frac{n_{B{r}_2}}{n_{Br{O}_3^{-}}}=3$
3. $\frac{n_{O{H}^{-}}}{n_{H_{2}O}}=2$
4. $\frac{n_{O{H}^{-}}}{n_{H_{2}O}}=3$

Q.

Which of the following is not a balanced equation?

1. $\mathrm{Fe}+{\mathrm{Cl}}_2\to {\mathrm{FeCl}}_3$

2. $\mathrm{Mg}+{\mathrm{CuSO}}_4\to {\mathrm{MgSO}}_4+\mathrm{Cu}$

3. $\mathrm{NaOH}+\mathrm{HCl}\to \mathrm{NaCl}+{\mathrm{H}}_2\mathrm{O}$

4. $\mathrm{Zn}+\mathrm{S}\to \mathrm{ZnS}$

Q. Given redox reaction :

$Cl{O}^{-}+Cr{O}_2^{-}\to C{l}^{-}+Cr{O}_4^{2-}$

When balanced in a basic medium by oxidation number method, the ratio of stoichiometric coefficient of $O{H}^{-}$ and $H_{2}O\left(\frac{n_{O{H}^{-}}}{n_{H_{2}O}}\right)$ will be:

1. $1:1$
2. $2:1$
3. $1:2$
4. $1:4$

Q.

Give the balanced equation for the action of heat on the following compound:

Silver oxide.

Q. What is the coefficient of oxalate ion in the balanced form of following reaction?
$Mn{O}_4^{-}+C_2{O}_4^{2-}+H^{+}⟶M{n}^{2+}+C{O}_2+H_{2}O$

1. 4
2. 2
3. 3
4. 5

Q. $P_4{O}_6$ reacts with water according to equation $P_4{O}_6+6H_{2}O\to 4H_{3}P{O}_{3-}$.
Calculate the volume of 0.1 M NaOH solution required to neutralize the acid formed by dissolving 1.1 g of $P_4{O}_{6}in{H}_{2}O$.

Q. Balance the following reaction by ion electron method:
$KMn{O}_4+H_{2}S{O}_4+HCl\to K_{2}S{O}_4+MnS{O}_4+C{l}_2+H_{2}O$

1. $2KMn{O}_4+10HCl+2H_{2}S{O}_4\to 5C{l}_2+2MnS{O}_4+8H_{2}O$
2. $2KMn{O}_4+10HCl+3H_{2}S{O}_4\to 5C{l}_2+2MnS{O}_4+8H_{2}O$
3. $2KMn{O}_4+10HCl+H_{2}S{O}_4\to 5C{l}_2+2MnS{O}_4+8H_{2}O$
4. $2KMn{O}_4+HCl+3H_{2}S{O}_4\to 5C{l}_2+2MnS{O}_4+8H_{2}O$

Q. Balance the following equation.
$Fe{S}_2+O_2\to F{e}_2{O}_3+S{O}_2$

Q. Balance the following equation :
$PbS+H_2{O}_2\to PbS{O}_4+H_{2}O$

1. $2PbS+4H_2{O}_2\to 2PbS{O}_4+4H_{2}O$
2. $PbS+4H_2{O}_2\to PbS{O}_4+4H_{2}O$
3. $PbS+2H_2{O}_2\to PbS{O}_4+2H_{2}O$
4. $2PbS+2H_2{O}_2\to 2PbS{O}_4+4H_{2}O$

Q.

$KMn{O}_4$ acts as an oxidizing agent in:

1. acidic medium only
2. neutral and acidic media
3. neutral and alkaline media
4. neutral, acidic and alkaline media

Q. A current of 2 amperes passing through for 5 hours through molten tin salt deposited 22.2 gm of tin. The oxidation state of tin in the salt is ( at. Mass of Sn = 119 )

Q.

Which reaction does not represent auto redox or disproportionation?

1. ${\mathrm{Cl}}_2+{\mathrm{OH}}^{-}\to {\mathrm{Cl}}^{-}+{\mathrm{ClO}}_3^{-}+{\mathrm{H}}_2\mathrm{O}$

2. $2{\mathrm{H}}_2{\mathrm{O}}_2\to 2{\mathrm{H}}_2\mathrm{O}+{\mathrm{O}}_2$

3. $2{\mathrm{Cu}}^{+}\to {\mathrm{Cu}}^{2+}+\mathrm{Cu}$

4. ${\left({\mathrm{NH}}_4\right)}_2{\mathrm{Cr}}_2{\mathrm{O}}_7\to {\mathrm{N}}_2+{\mathrm{Cr}}_2{\mathrm{O}}_3+4{\mathrm{H}}_2\mathrm{O}$

Q. In the following reaction :
$H_2{O}_2\left(aq\right)+C{l}_2{O}_7\left(aq\right)\to Cl{O}_2^{-}\left(aq\right)+O_2\left(g\right)$
Moles of $O{H}^{-}$ and $H_{2}O$ respectively present in a balanced equation in a basic medium are x and y. Calculate the value of x+y:

Q.

The equivalent weight of ${\mathrm{K}}_2{\mathrm{CrO}}_4$, when it reacts with ${\mathrm{AgNO}}_3$ to give ${\mathrm{Ag}}_2{\mathrm{CrO}}_4$ is _______.

1. $\mathrm{M}$

2. $\frac{\mathrm{M}}{2}$

3. $\frac{\mathrm{M}}{3}$

4. Infinite

Q.

In an electrolysis experiment current was passed for 5 hours through two cells connected in series. The first cell contains a solution of gold and the second contains copper sulphate solution. 9.85 g of gold was deposited in the first cell. If the oxidation number of gold is +3, find the amount of copper deposited on the cathode of the second cell.

(At.wt. of Au = 197 and At.wt of Cu = 63.5)

1. 4.76 g

2. 2.34

3. 8.9 g

4. 6.6 g

Q.

What product is formed on disproportionation of ${\mathrm{H}}_3{\mathrm{PO}}_3$?

Q.

What happens when carbon dioxide reacts with sodium oxide?

Q. What volume of $O_2\left(g\right)$ measured at 1 atm and 273 K will be formed by the action of 100 ml of 0.5 N of $KMn{O}_4$ on hydrogen peroxide in an acidic solution?
$KMn{O}_4+H_{2}S{O}_4+H_2{O}_2\to K_{2}S{O}_4+MnS{O}_4+O_2+H_{2}O$

1. 0.12 L
2. 0.03 L
3. 0.56 L
4. 1.12 L

Q. Balance the following equation by ion electron method-
$C{u}_{2}O+H^{+}+N{O}_3^{-}\to C{u}^{2+}+NO+H_{2}O$

1. $3C{u}_{2}O+14H^{+}+2N{O}_3^{-}\to 6C{u}^{2+}+2NO+7H_{2}O$
2. $6C{u}_{2}O+14H^{+}+N{O}_3^{-}\to 6C{u}^{2+}+2NO+7H_{2}O$
3. $3C{u}_{2}O+14H^{+}+4N{O}_3^{-}\to 6C{u}^{2+}+4NO+7H_{2}O$
4. None

Q. How does ammonia react with a solution of $C{u}^{2+}$?

Q. How to balance a reaction taking place in basic medium by ion electron method? Explain.