SHE

Q. In a solvent 50% of an acid HA dimerizes and the rest dissociates. The van't Hoff factor of the acid is $x\times {10}^{-2}$. The value of x(Round off to the Nearest Integer) is

Q.

What is the application of gel electrophoresis?

Q. Battery acid is 4.27M H2SO4(aq) and has density 1.25 g/ML. What is the molality of H2SO4 in the solution?

Q.

$0.01$ moles of a weak acid $\mathrm{HA}(\mathrm{Ka}=2.0\mathrm{x}{10}^{-6})$ is dissolved in $1.0\mathrm{L}\mathrm{of}0.1\mathrm{M}\mathrm{HCl}$ solution. The degree of dissociation of $\mathrm{HA}$ is_______ $\mathrm{x}{10}^{-5}$ (Round off to the Nearest Integer). Assume the degree of dissociation $<<1$

Q.

What is standard reduction potential?

Q. (a) The cell in which the following reaction occurs:
$2F{e}^{3+}\left(aq\right)+2I^{-}\left(aq\right)\to 2F{e}^{2+}\left(aq\right)+I_2\left(s\right)$ has $E_{\text{cell}}^{⊝}=0.236V$ at 298 K.
Calculate the standard Gibbs energy of the cell reaction. (Given: 2F= 96500 C $mo{l}^{-1}$)
(b) How many electrons flow through a metallic wire if a current of 0.5 A is passed for 2 hours? (Given: 1F= 96500 C $mo{l}^{-1}$)

Q.

No/2 atoms of $X_{\left(g\right)}$ are converted into $X_{(g{)}^{+}}^{+}$ by energy $E_1$, No/2 atoms of $X_g$ are converted into $X_{\left(g\right)}^{-}$ by energy $E_2$. Hence ionization potential and electron affinity of $X_{\left(g\right)}$ per atom are

1. None of these

2. 

3. 

4. 

Q.

How would you determine the standard electrode potential of the systemMg²⁺ | Mg?

Q. The spin-only magnetic moment value of $M^{3+}$ ion (in gaseous state) from the pairs $C{r}^{3+}/C{r}^{2+},M{n}^{3+}/M{n}^{2+},F{e}^{3+}/F{e}^{2+}\text{and}C{o}^{3+}/C{o}^{2+}$ that has negative standard electrode potential, is ______B.M. [Nearest integer]

Q. If Cu^{+2}/Cu electrode is diluted 100 times, then the change in emf is-increase of 59 mV-decrease of 59 mV-increase of 29.5 mV-decrease of 29.5m

Q.

pH of 0.1 M weak acid solution is 4. What is the dissociation constant of the acid ?

1. 

2. 

3. 

4. 

Q.

What is the solubility product of a saturated solution of ${\mathrm{Ag}}_2{\mathrm{CrO}}_4$in water at $298\mathrm{K}$ if the emf of the cell Ag Is $0.164\mathrm{V}$ At $298\mathrm{K}$?

Q.

The unit of cell constant is ___________.

Q. Aqueous copper sulphate solution and aqueous silver nitrate solutions are electrolyzed by 1 ampere current for 10 minutes in separate electrolytic cells. Will the mass of copper and silver deposited on the cathode be the same or different? Explain your answer.

Q. The equivalent weight of copper and silver are 32 and 108 respectively. When copper and silver voltameter are connected in series and electric current is passed through for sometimes, $1.6g$ of copper is deposited. Then, the mass of silver deposited will be:

1. $3.5g$
2. $2.8g$
3. $5.4g$
4. $8g$

Q. A 38% solution of sulphuric acid is used as electrolyte.(Density=1.294 gmL-¹).The battery , holds 3.5 L of the acid. During the discharge of the battery, the density of H2so4 falls to 1.139 mL-¹. (20% h2so4 by mass). What is the Molarity of sulphuric acid before discharge?

Q. In the electrolysis of a CuSO4 solution, how many grams of Cu are plated out on the cathode in the time that it takes to liberate 5.6 litre of O2, measured at STP, at the anode? (a)31.75 (b) 14.2 (c)4.32 (d)25.2

Q.

The pH of 0.1 M solution of the following salts increases in the order

1. NaCl < NH₄Cl < NaCN < HCl\

2. HCl < NaCN < NH₄Cl < NaCl

3. NaCN < NH₄Cl < NaCl < HCl

4. HCl < NH₄Cl < NaCl < NaCN

Q. For $I_2+2e^{-}\to 2I^{-},\text{standard reduction potential}=+0.54\text{Volt}.$
For $2B{r}^{-}\to B{r}_2+2e^{-},\text{standard oxidation potential}=-1.09\text{Volt}.$
For $Fe\to F{e}^{2+}+2e^{-},\text{standard oxidation potential}=+0.44\text{Volt}.$
Out of the below given reactions, how many reactions are spontaneous in nature (predict from the above data) ?
$B{r}_2+2I^{-}\to 2B{r}^{-}+I_2$
$Fe+B{r}_2\to F{e}^{2+}+2B{r}^{-}$
$Fe+I_2\to F{e}^{2+}+2I^{-}$
$I_2+2B{r}^{-}\to 2I^{-}+B{r}_2$

Q. A solution containing $1.2046\times {10}^{24}$ HCl molecules in one $d{m}^3$ of the solution. The strength of the solution in

1. 6N
2. 2N
3. 4N
4. 8N

Q. Define Reference electrode.

Q. The reduction potential of hydrogen electrode will be positive if

1. $p\left(H_2\right)=1atm,\left[H^{+}\right]=1M$
2. $p\left(H_2\right)=1atm,\left[H^{+}\right]=2M$
3. $p\left(H_2\right)=2atm,\left[H^{+}\right]=1M$
4. $p\left(H_2\right)=2.5atm,\left[H^{+}\right]=1.5M$

Q. For the reaction given below the values of standard Gibbs free energy of formation at 298 K are given. What is the nature of reaction?
$I_2+H_{2}S\to 2HI+S$
$△G_f^o\left(HI\right)=1.8kJmo{l}^{-1},△G_f^o\left(H_{2}S\right)=33.8kJmo{l}^{-1}$

1. Non-spontaneous in forward direction.
2. Spontaneous in forward direction.
3. Non-spontaneous in both forward and backward directions.
4. Spontaneous in backward direction.

Q. What is the reaction that takes place at the standard hydrogen electrode if it's coupled with metal-metal ion electrode of zinc (zinc in zinc sulphate solution).

1. $Pt\to P{t}^{+}+e^{-}$
2. $P{t}^{+}+e^{-}\to Pt$
3. $H_2\to 2H^{+}+2e^{-}$
4. $2H^{+}+2e^{-}\to H_2$

Q. The product of electrolysis pf aqueous Na2SO4 with inert electrodes is

Q. The value of $E_{reduction}$ of a hydrogen electrode at $pH=0$ and $298K$, $1atm$ is:

1. $0.59V$
2. $0V$
3. $-0.59V$
4. $-0.059V$

Q. $H_2{O}_2$ turns blackened lead paintings to white colour. In this reaction it oxidizes PbS to $PbS{O}_4$. The number of moles of $H_2{O}_2$ needed to oxidize one mole of PbS is

1. 1
2. 2
3. 0.5
4. 4

Q. for the given half cell, Al3+ + 3e- -------> Al, on increasing [Al3+], the electrode potential

Q. 7. Predict the products of electrolysis:- a)Aqueous solution of AgNO3 with Ag electrodes. b)Aqueous solution of AgNO3 with Platinum electrodes. c)Aqueous solution of CuCl2 with Platinum electrodes. d) Dilute solution of H2SO4 with Platinum electrodes.

Q.

When $10\mathrm{mL}$ of ${\mathrm{H}}_2$​ and $12.5\mathrm{mL}$ of ${\mathrm{Cl}}_2$ are allowed to react, the final mixture contains under the same conditions.