Frankland Halide Reaction

Q. The $E^{\ominus }\left(M^{2+}/M\right)$ value for copper is positive $(+0.34V)$. What is possible reason for this? (Hint: consider its high ${\Delta }_a{H}^{\ominus }$ and low ${\Delta }_{hyd}{H}^{\ominus }$)

Q.

Write balanced equations for:

(i) BF₃ + LiH →

(ii) B₂H₆ + H₂O →

(iii) NaH + B₂H₆ →

(iv) H₃BO₃

(v) Al + NaOH →

(vi) B₂H₆ + NH₃ →

Q. In a given reaction; $Ag(CN{)}_2^{-}\rightleftharpoons A{g}^{+}+2C{N}^{-}$, the equilibrium constant at ${25}^{\circ }C$ is $4.0\times {10}^{-19}$, then the silver ion concentration in a solution which was originally $0.1M$ in $KCN$ and $0.03M$ in $AgN{O}_3$ is:

1. $7.5\times {10}^{18}$
2. $7.5\times {10}^{-18}$
3. $7.5\times {10}^{19}$
4. $7.5\times {10}^{-19}$

Q.

Calcium hydroxide reacts with ammonium chloride to give ammonia, according to the following equation:

$\mathrm{Ca}{\left(\mathrm{OH}\right)}_2+2{\mathrm{NH}}_4\mathrm{Cl}\to {\mathrm{CaCl}}_2+2{\mathrm{NH}}_3+2{\mathrm{H}}_2\mathrm{O}$

If $5.35\mathrm{g}$ of ammonium chloride is used, calculate the weight of calcium chloride is formed.

$\left[\mathrm{H}=1,\mathrm{N}=14,\mathrm{O}=16,\mathrm{Cl}=35.5,\mathrm{Ca}=40\right]$

Q.

The number of electrons involved in the reduction of $C{r}_2{O}_7^{2-}$ in acidic solution to $C{r}^{3+}$ is

1. 5

2. 0

3. 2

4. 3

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

Q. Complete the following reactions 

(i) $O_2^{2-}+H_{2}O\to$

(ii) $O_2^{-}+H_{2}O\to$

Q.

Complete and balance the following equation:

Ca + H₂ $\to$________

Q. The equivalent weight for underlined molecule in the following reaction is M/n (M = molar mass of $P_4)$.
Find n.
${\underset{–}{P}}_4\to P{H}_3+H_{2}P{O}_2^{-}$

Q. For the reactions,
$B{r}_2+O{H}^{-}\to B{r}^{-}+Br{O}_3^{-}+H_{2}O$
what is the equivalent weight of $B{r}_2$ ?

1. $M/8$
2. $M/5$
3. $3M/5$
4. $5M/8$

Q. Formation of alkane by the action of Zn on alkyl halide is called

1. Cannizzaro reaction
2. Frankland's reaction
3. Wurtz reaction
4. Kolbe's reaction

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

Q. Oxidation of thiosulphate $\left(S_2{O}_3^{2-}\right)$ ion by iodine gives

1. $S{O}_3^{2-}$
2. $S{O}_4^{2-}$
3. $S_4{O}_6^{2-}$
4. $S_2{O}_6^{2-}$

Q. For the reaction,
$Fe{S}_2+KMn{O}_4+H^{+}\to F{e}^{3+}+H_{2}S{O}_4+M{n}^{2+}+H_{2}O$.
If the molar mass of $Fe{S}_2$ is M, then equivalent mass of $Fe{S}_2$ would be equal to:

1. $M$
2. $\frac{M}{10}$
3. $\frac{M}{11}$
4. $\frac{M}{15}$

Q. $O_2+Fe{S}_2\to FeO+S{O}_2$
The number of moles of $Fe{S}_2$ required to produce $20\text{mol}$ electrons to reduce $O_2$ in the above reaction is:

1. $2$
2. $10$
3. $\frac{10}{3}$
4. $\frac{5}{3}$

Q. Permanganate ion acts as oxidising agent in acidic, neutral as well as alkaline medium. Consider the reactions of permanganate ion:

I. $I^{-}+Mn{O}_4^{-}\underset{\text{Medium}}{\overset{\text{Acidic}}{\to }}$

II. $I^{-}+Mn{O}_4^{-}\underset{\text{or faintly alkaline medium}}{\overset{\text{Neutral}}{\to }}$

The oxidation state of iodine in reactions I and II are respectively

1. Zero in both reactions
2. Zero in I and $+3$ in II
3. $+3$ in I and zero in II
4. Zero in I and $+5$ in II

Q. Balance the following equations:
$C_2{H}_6+O_2\to C{O}_2+H_{2}O$

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. $\begin{array}{ccc}Mn{O}_4^{-}& C_2{O}_4^{2-}& H^{+}\\ 2& 5& 16\end{array}$
2. $\begin{array}{ccc}Mn{O}_4^{-}& C_2{O}_4^{2-}& H^{+}\\ 16& 5& 2\end{array}$
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. If M represents molecular mass of $B{r}_2$ then what will be its equivalent mass if it undergoes disproportionation reaction as shown:

$3B{r}_2+6O{H}^{-}\to 5B{r}^{-}+Br{O}_3^{-}+3H_{2}O$

1. $\frac{M}{2}$
2. $\frac{M}{10}$
3. $\frac{M}{2}$ + $\frac{M}{10}$

4. $\frac{M}{6}$

Q. Balance the given equation.
$KCl{O}_3\to KCl+O_2$.

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

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

Q. The value of equilibrium constant of a reaction depends upon the initial values of concentration of reactants.
If true enter 1, else enter 0.

Q. $Mn{O}_2+H_2{O}_2\to {MnO}_4^{-}+H_{2}O$ (Basic medium)

1. $3H_2{O}_2+2Mn{O}_2+2O{H}^{-}\to 2{MnO}_4^{-}+4H_{2}O$
2. $3H_2{O}_2+Mn{O}_2+3O{H}^{-}\to 2{MnO}_4^{-}+5H_{2}O$
3. $H_2{O}_2+2Mn{O}_2+O{H}^{-}\to 2{MnO}_4^{-}+4H_{2}O$
4. none of these

Q. Write the balanced equations for the reaction occurring when gold is dissolved in aqua regia.

1. None of these
2. $2Au+3H{NO}_3+11HCl\to 2HAu{Cl}_4+3NOCl+6H_{2}O$
3. $2Au+3H{NO}_3+13HCl\to 2HAu{Cl}_4+2NOCl+8H_{2}O$
4. $2Au+5H{NO}_3+11HCl\to 2HAu{Cl}_4+2NOCl+8H_{2}O$

Q. $3mol$ of _____ reacts with $2mol$ of phosphine to produce $1mol$ of mercuric phosphide.

1. Mercuric sulphate
2. Mercuric chloride
3. Mercuric phosphate
4. Mercurous sulphate

Q. Match the reaction given in Column I with the names given in Column II.

1. A-iii, B-ii, C-i, D-iv
2. A-iii, B-iv, C-i, D-ii
3. A-iii, B-i, C-ii, D-iv
4. A-ii, B-i, C-iii, D-iv

Q. The below reaction is known as :

1. Wurtz reaction
2. Wurtz fittig reaction
3. Fittig reaction
4. Kolbe's electrolysis

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

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. Two
4. One

Q. In case of Wurtz reaction, which alkyl halide gives maximum yield of alkane?

1. Isopropyl bromide
2. Tert-butyl brominde
3. Ethyl bromide
4. Methyl bromide