Q. For the reaction $2S{O}_2+O_2\rightleftharpoons 2S{O}_3$, the unit of equilibrium constant is:

1. $Lmo{l}^{-1}$
2. $mol{L}^{-1}$
3. $Jmo{l}^{-1}$
4. $L^{2}mo{l}^{-1}$

Q. Solubility of calcium oxalate is ________ in the presence of ammonium oxalate because of _______ .

Q. The deficiency of vitamin D causes:

1. Gout
2. Rickets
3. Night blindness
4. Scurvy

Q. Half life period of a _________ order reaction is ________ of the concentration of the reactant.

Q. The compound which is optically active is :

1. $1-butanol$
2. $2-butanol$
3. $2-methyl-1-propanol$
4. $1-propanol$

Q. Ethylene glycol is used as an antifreeze agent. Calculate the amount of ethylene glycol to be added to $4kg$ of water to prevent it from freezing at $-6^{\circ }C.(K_f$ for $H_{2}O=1.85Kmol{e}^{-1}kg)$

Q. The freezing point of a solution containing $0.3gms$ of acetic acid in $30gms$ of benzene is lowered by $0.45K$. Calculate the Van't Hoff factor.
(at. wt. of $C=12,H=1,O=16,K_f$ for benzene $=5.12kkgmol{e}^{-1})$

Q. The rate of the reaction $H_2+I_2\rightleftharpoons 2HI$ is given by:
$rate=1.7\times {10}^{-19}\left[H_2\right]\left[I_2\right]$ at ${25}^{\circ }C$
The rate of decomposition of gaseous $HI$ to $H_2$ and $I_2$ is given by:
$rate=2.4\times {10}^{-21}[HI{]}^2$ at ${25}^{\circ }C$.
Calculate the equilibrium constant for the formation of $HI$ from $H_2$ and $I_2$ at ${25}^{\circ }C$?

Q. Two metallic elements $A$ and $B$ have the following standard oxidation potentials:
$A=0.40VB=-0.80V$. What would you expect if element $A$ was added to an aqueous salt solution of element $B$? Give a reason for your answer.

Q. The salt which will not hydrolyse in aqueous solution is :

1. copper sulphate
2. sodium sulphate
3. potassium cyanide
4. sodium carbonate

Q. In a galvanic cell, electrons flow from ______ to ______ through the connecting wires.

Q. Define cryoscopic constant.

Q. Name the law or principle confirmed by the following observations:
When $96500$ coulombs of electricity is passed through acidulated water, $5-6$ litres of oxygen at s.t.p. is liberated at the anode.

Q. Given balanced equation for the preparation of salicylaldehyde from phenol?

Q. If the half life period for a first order reaction is $69.3$ seconds, what is the value of its rate constant?

Q. Racemic mixtures are optically _______ because of _________compensation.

Q. In a first order reaction, $10$% of the reactant is consumed in $25$ minutes. Calculate:
The time required for completing $17$% of the reaction.

Q. Match the following

Q. In a first order reaction, 1010 % is complete Calculate:The half life of the reaction :

Q. Arrange $Ag,Cr$ and $Hg$ metals in the increasing order of reducing power. Given:
$E_{A{g}^{+}/Ag}^{\circ }=+0.80V$
$E_{C{r}^3/Cr}^{\circ }=-0.74V$
$E_{H{g}^{3+}/Hg}^{\circ }=+0.79V$

Q. The solubility of $A{g}_{2}Cr{O}_4$ at ${25}^{\circ }C$ is $8.0\times {10}^{-5}$ moles/litre. Calculate its solubility product

Q. A solution of $N{H}_{4}Cl$ and $N{H}_{4}OH$ acts as a buffer.

Q. What is Schottky defect in a solid?

Q. Benzaldehyde when treated with an alcoholic solution of ________ forms ________ .

Q. $Cu$ is precipitated as $CuS$ while $Zn$ is not precipitated when $H_{2}S$ is passed through an acidic solution of $CU(N{O}_3{)}_2$ and $Zn(N{O}_3{)}_2$ respectively.

Q. A $bcc$ element (atomic mass $65$) has a cell edge of $420pm$. Calculate its density in $gms/c{m}^3$.

Q. Give Lewis' definition for acids and bases.

Q. Copper has the face-centered cubic structure. The coordination number of each ion is:

1. $12$
2. $4$
3. $14$
4. $8$

Q. Two moles of $N{H}_3$ are introduced into one litre flask in which it dissociates at high temperature as follows:
$2N{H}_3\left(g\right)\rightleftharpoons N_2\left(g\right)+3H_2\left(g\right)$. Determine $K_C$, if at equilibrium $1mole$ of $N{H}_3$ remains.

Q. Name the law or principle confirmed by the following observations:
When water is added to $0.01M$ aqueous solution of acetic acid the number of hydrogen ions increases.