Balancing Redox Equations

Q.

An equimolar mixture of $\mathrm{NaOH}$ and ${\mathrm{Na}}_2{\mathrm{CO}}_3$ weighs $4$$\mathrm{g}$, then the weight of $\mathrm{NaOH}$ is:

Q. In the reaction $I_2+2S_2{O}_3^{--}\to 2I^{-}+S_4{O}_6^{--}$ equivalent weight of iodine will be equal to

1. $\frac{1}{2}$ of molecular weight
2. Molecular weight
3. None
4. $\frac{1}{4}$ of molecular weight

Q.

${}_5{B}^{10}$ + ${}_{2}H{e}^4$ $\to$ X + ${}_0{n}^1$

'X' in the above reaction is

1. ₇N¹²

2. ₇N¹³

3. ₆B¹³

4. ₆B¹⁴

Q.

What mass of dilute nitric acid will be required to dissolved $5\mathrm{g}$ of calcium carbonate?

Q.

Write the balanced equation for the following chemical reaction.

Barium chloride + Aluminium sulphate → Barium sulphate +

Aluminium chloride

Q. Question 20.2

Write the balanced chemical equation for the following reaction and identify the type of reaction.

Magnesium ribbon is burnt in an atmosphere of nitrogen gas to form solid magnesium nitride.

Q. In the reaction $xHI+yHN{O}_3\to NO+I_2+H_{2}O$

1. x = 1, y = 5
2. x = 2, y = 10
3. x = 6, y = 1
4. x = 6, y = 2

Q.

How many moles of $K_{2}C{r}_2{O}_7$ can be reduced by 1 mole of $S{n}^{+2}$

1. 1/3

2. 1/6

3. 2/3

4. 1

Q. Sodium reacts with silver nitrate to produce silver chloride and sodium nitrate.
c) Find the weights of reactants and products

Q.

For the redox reaction
MnO−4+C2O−24+H+⟶Mn2++CO2+H2O
the correct coefficients of the reactants MnO−4, C2O2−4 and H+ for the balanced reaction are

2, 5, 16

16, 5, 2

5, 16, 2

2, 16, 5

Q.

balance the equation :- Cu + HNO3 = Cu(NO3)2 + NO H2O

Q. Question 2.3

Write the balanced equation for the following chemical reaction:

Sodium + Water $\to$ Sodium hydroxide + Hydrogen

Q. For the redox reaction $x{P}_4+yHN{O}_3\to H_{3}P{O}_4+N{O}_2+H_{2}O$

1. x = 2, y = 10
2. x = 1, y = 20
3. x = 1, y = 5
4. x = 1, y = 15

Q. The equivalent weight of $KI{O}_3$ in the reaction
$2Cr(OH{)}_3+4OH+KI{O}_3\to 2Cr{O}_4^{2-}+5H_{2}O+KI$ is

1. $\frac{Mol.wt.}{6}$
2. Mole wt.
3. $\frac{Mol.wt.}{2}$
4. $\frac{Mol.wt.}{3}$

Q.

In the balanced chemical reaction,
$I{O}_3^{-}+a{I}^{-}+b{H}^{+}⟶c{H}_{2}O+d{I}_2$
a, b, c and d respectively correspond to

1. 5, 6, 3, 3

2. 5, 3, 6, 3

3. 5, 6, 5, 5

4. 3, 5, 3, 6

Q.

If the reaction below is a double displacement, what will the equation when it is balanced $AlC{l}_3+AgN{O}_3\to$?

1. AlCl₃+ AgNO₃ → Al(NO₃)₃+ 3AgCl

2. AlCl₃+ 3AgNO₃ → Al(NO₃)₃ + 3AgCl

3. AlCl₃+ 3AgNO₃ → Al(NO₃)₃ + AgCl

4. None of the above

Q. $C_2{H}_6\left(g\right)+n{O}_2\to C{O}_2\left(g\right)+H_{2}O\left(I\right)$
In this equation, the ratio of the coefficients of $C{O}_2$ and $H_{2}O$ is

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

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. 3:2

3. 2:3

4. 1:3

Q.

Electra has trouble finding the correct Nernst equation for the cell $Zn\left(s\right)|Z{n}^{2+}||C{u}^{2+}|Cu\left(s\right)at{25}^{\circ }C$
Can you help her?

1. $E_{cell}=E^{\circ }-0.0296log\left(\frac{\left[Z{n}^{2+}\right]}{\left[C{u}^{2+}\right]}\right)$

2. $E_{cell}=E^{\circ }-0.0296log\left(\frac{Zn}{Cu}\right)$

3. $E_{cell}=E^{\circ }-0.0296log\left(\frac{Cu}{Zn}\right)$

4. $E_{cell}=E^{\circ }-0.0296log\left(\frac{\left[C{u}^{2+}\right]}{\left[Z{n}^{2+}\right]}\right)$

Q. What is the equivalent mass of $I{O}_4^{-}$ when it is converted into $I_2$ in acid medium

1. $\frac{M}{6}$
2. $\frac{M}{7}$
3. $\frac{M}{5}$
4. $\frac{M}{4}$
5. None of these

Q. Consider the following reaction:
$xMn{O}_4^{-}+y{C}_2{O}_4^{2-}+z{H}^{+}\to xM{n}^{2+}+2yC{O}_2+\frac{z}{2}{H}_{2}O$
The values of x, y and z in the reaction are, respectively:

1. 5, 2 and 16
2. 2, 5 and 16
3. 2, 5 and 8
4. 5, 2 and 8

Q. $2S{O}_3\rightleftharpoons 2S{O}_2+O_2$ . If $K_c=100,\alpha =1$ , half of the reaction is completed, the concentration of $S{O}_3$ and $S{O}_2$ are equal, the concentration of $O_2$ is​:

1. $0.001M$
2. $2$ times of $S{O}_2$
3. Data incomplete
4. $\frac{1}{2}S{O}_2$

Q. How many moles of $KMn{O}_4$ are reduced by $1$ mole of ferrous oxalte in acidic medium?

1. $\frac{1}{5}$
2. $\frac{5}{3}$
3. $\frac{1}{3}$
4. $\frac{3}{5}$

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

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

1. $\begin{array}{ccc}Mn{O}_4^{-}& C_2{O}_4^{2-}& H^{+}\\ 16& 5& 2\end{array}$
2. $\begin{array}{ccc}Mn{O}_4^{-}& C_2{O}_4^{2-}& H^{+}\\ 2& 5& 16\end{array}$
3. $\begin{array}{ccc}Mn{O}_4^{-}& C_2{O}_4^{2-}& H^{+}\\ 5& 16& 2\end{array}$
4. $\begin{array}{ccc}Mn{O}_4^{-}& C_2{O}_4^{2-}& H^{+}\\ 2& 16& 5\end{array}$

Q. In a balanced equation
$H_{2}S{O}_4+xHI\to H_{2}S+y{I}_2+z{H}_{2}O$, the values of x, y, z are

1. x = 8, y = 4, z = 4
2. x = 5, y = 3, z = 4
3. x = 3, y = 5, z = 2
4. x = 4, y = 8, z = 5

Q. In a certain operation 358 gm of $TiC{l}_4$ is reacted with 96 gm of $Mg$. The $\%$ yield of $Ti$ if 32 gm of $Ti$ actually obtained is :

1. $35.38\%$
2. $66.5\%$
3. $100\%$
4. $60\%$

Q. In the reaction,
$xO{H}^{-}+yA{s}_2{S}_3+zCl{O}_3^{-}⟶aAs{O}_4^{3-}+bCl{O}^{-}+3S{O}_4^{2-}+c{H}_{2}O$,

x, y, z, a, b, and c are respectively:

1. 2, 14, 24, 14, 4, 12
2. 24, 4, 14, 2, 14, 12
3. 20, 4, 12, 4, 12, 10
4. 24, 2, 14, 4, 14, 12

Q.

Write the balanced equation for complete hydrolysis of XeF6

Q. For decolourization of 1 mole of $KMn{O}_4$, the moles of $H_2{O}_2$ required is

1. $\frac{1}{2}$
2. $\frac{3}{2}$
3. $\frac{5}{2}$
4. $\frac{7}{2}$