Question 2 :
The density of a $3 \,M$ sodium thiosulphate $(Na_2S_2O_3)$ solution is $1.25 \,gm/ml$. Calculate the percentage by weight of sodium thiosulphate.

Question 3 :
$2.5$ litre of $1\ M\ NaOH$ solution mixed with another $3$ litre of $0.5\ M\ NaOH$ solution. Then find out molarity of resultant solution.

Question 5 :
An aqueous solution of glucose is 10% in strength. The volume in which 1 gram mole of it is dissolved will be:<br/>

Question 6 :
What mass of sodium carbonate, $Na_2CO_3$&#160; is needed to make 120 mL of a 1.5 M solution? (Given formula weight of sodium carbonate = 106 amu)

Question 7 :
When 180 grams of glucose is subjected to combustion, the volume of $CO_2$ liberated at STP is

Question 8 :
A gaseous mixture contains $4.0$ gm of $H_{2}$ and $56.0$ gm of $N_{2}$. The mole fraction of $H_{2}$ in the&#160;mixture is:

Question 11 :
If 6 M $KOH$ solution is 28% by weight, then what is the&#160;specific gravity of this&#160;solution?

Question 12 :
A quantity of $23.6\ g$ of succinic acid is dissolved in $500\ ml$ of $0.1\ M$ acetic acid solution. Assuming that neither acid is dissociated in solution, calculate the molarity of $'-COOH'$ in the solution.

Question 13 :
A solution contain $36\%$ water and $64\%$ acetaldehyde $(CH_2CHO)$ by mass. The mole fraction of acetaldehyde is:

Question 14 :
If&#160;250 mL of a solution contains 24.5 g $H_2SO_4$ &#160;the molarity and normality respectively are:

Question 15 :
The molarity of $4\ N\ H_2SO_4$ in the following reaction is $8H^+ +H_2SO_4 + 8e^- \to H_2S +4H_2O$

Question 17 :
Which of the following does not have valence electron in 3d-subshell?

Question 18 :
The electronic configuration is given as:<div><br/>$1s^2\ 2s^2\ 2p^6\ 3s^2\ 3p^6\ 3d^{10}\ 4s^2\ 4p^6\ 4d^{10}\ 5s^2$ is for:</div>

Question 19 :
The elements which exhibit both vertical and horizontal similarities are called:

Question 21 :
The electronic configuration of the outermost orbit in the case of alkaline earth metals is :

Question 24 :
Arrange the elements $F,\ Na,\ Fe,\ Cl,\ Ne$ in increasing order of ionization energy.

Question 26 :
On moving from top to bottom in a group in the periodic table, valency :

Question 29 :
The electronic configuration of an atom $A$ is $1s^2 2s^2 2p^6 3s^2p^6 3d^{10} 4s^2 4p^3$. The chemistry of $A$ is therefore likely to be similar to that of&#160;

Question 30 :
Which of the following orbitals will have zero probability of finding the electron in the yz plane?

Question 32 :
In an irreversible process taking place at constant {tex} \mathrm {T } {/tex} and {tex} \mathrm { P } {/tex} and in which only pressure-volume work is being done, the change in Gibbs free energy {tex} \mathrm { (dG) } {/tex} and change in entropy {tex} \mathrm { (dS) } {/tex}, satisfy the criteria

Question 33 :
Substance {tex} \mathrm { A } _ { 2 } \mathrm { B } ( \mathrm { g } ) {/tex} can undergoes decomposition to form two set of products:<br><img style='object-fit:contain' src="https://storage.googleapis.com/teachmint/question_assets/NEET/5dfc68918701466b65e5eb85"><br>If the molar ratio of {tex} \mathrm {A_2(g)}{/tex} to {tex} \mathrm {A(g)}{/tex} is {tex}5 : 3{/tex} in a set of product gases, then the energy involved in the decomposition of 1 mole of {tex} \mathrm{ {A_2 B} (g)} {/tex} is :

Question 34 :
The heat of atomization of {tex} \mathrm { PH } _ { 3 } ( \mathrm { g } ) {/tex} is {tex} 228 \mathrm { kcal } {/tex} {tex} \mathrm { mol } ^ { - 1 } {/tex} and that of {tex} \mathrm { P } _ { 2 } \mathrm { H } _ { 4 } ( \mathrm { g } ) {/tex} is {tex} 335 \mathrm { kcal } \mathrm { mol } ^ { - 1 } . {/tex} The energy of the {tex} \mathrm { P } - \mathrm { P } {/tex} bond is

Question 35 :
The bond dissociation energies of {tex} \mathrm { CH } _ { 4 } {/tex} and {tex} \mathrm { C } _ { 2 } \mathrm { H } _ { 6 } {/tex} respectively are 360 and 620 {tex} \mathrm { kcal mol } ^ { - 1 } {/tex}. The C-C bond energy would be :- -

Question 37 :
For a particular reversible reaction at temperature {tex} T , \Delta H {/tex} and {tex} \Delta S {/tex} were found to be both + ve. If {tex} T _ { e } {/tex} is the temperature at equilibrium, the reaction would be spontaneous when

Question 38 :
Hydrogen has an ionisation energy of {tex} 1311 \mathrm { kJ } {/tex} {tex} \mathrm { mol } ^ { - 1 } {/tex} and for chlorine it is {tex} 1256 \mathrm { kJ } \mathrm { mol } ^ { - 1 } . {/tex} Hydrogen forms {tex} \mathrm { H } ^ { + } ( \mathrm { aq } ) {/tex} ions but chlorine does not form {tex} \mathrm { Cl } ^ { + } ( \mathrm { aq } ) {/tex} ions because

Question 39 :
If the enthalpy change for the transition of liquid water to steam is 30kJ {tex}mol^{-1}{/tex} at {tex}27^\circ{/tex} C, the entropy change for the proces would be

Question 40 :
In a closed insulated container a liquid is stirred with a paddle to increase the temperature which of the following is true?

Question 41 :
The absolute enthalpy of neutralisation of the reaction: <br>{tex} \mathrm { MgO } _ { ( s ) } + 2 \mathrm { HCl } _ { ( a q ) } \rightarrow \mathrm { MgCl } _ { 2 ( a q ) } + \mathrm { H } _ { 2 } \mathrm { O } _ { ( \mathrm { l } ) } {/tex} will be

Question 42 :
The heats of neutralisation of {tex} \mathrm { CH } _ { 3 } \mathrm { COOH } , \mathrm { HCOOH } , \mathrm { HCN } {/tex} and {tex} \mathrm { H } _ { 2 } \mathrm { S } {/tex} are {tex} - 13.2 , - 13.4 , - 2.9 {/tex} and {tex} - 3.8 \mathrm { kcal } {/tex} per equivalent respectively. Arrange the acids in increasing order of strength

Question 43 :
When one mole of an ideal gas is compressed to half its initial volume and simultaneously heated to twice in initial temperature, the change in entropy {tex} ( \Delta \mathrm { S } ) {/tex} is

Question 44 :
Enthalpy of {tex} \mathrm { CH } _ { 4 } + 1 / 2 \mathrm { O } _ { 2 } \rightarrow \mathrm { CH } _ { 3 } \mathrm { OH } {/tex} is negative. If enthalpy of combustion of {tex} \mathrm { CH } _ { 4 } {/tex} and {tex} \mathrm { CH } _ { 3 } \mathrm { OH } {/tex} are {tex} x {/tex} and {tex} y {/tex} respectively. Then which relation is correct?

Question 45 :
Consider the following reactions:<br> {tex}\mathrm {(i)}\ \mathrm{ H^+}_{(aq)} + \mathrm{ OH^-}_{(aq)} = \mathrm{ H_2O_{(l)}}, \ \Delta H = -X_1\ \mathrm {{kJ}\ mol^{-1}} {/tex}<br> {tex}\mathrm {(ii)}\ \mathrm{ H}_{2(g)} + \mathrm{ 1/2 O}_{2(g)} = \mathrm{ H_2O_{(l)}}, \ \Delta H = -X_2\ \mathrm {{kJ}\ mol^{-1}} {/tex} <br>{tex}\mathrm {(iii)}\ \mathrm{ CO}_{2(g)} + \mathrm{ H}_{2(g)} = \mathrm{ CO_{(g)} + \mathrm{ H_2O_{(l)}}}, \ \Delta H = -X_3\ \mathrm {{kJ}\ mol^{-1}} {/tex} <br>{tex}\mathrm {(iv)}\ \mathrm{C_2 H}_{2(g)} + \mathrm{ 5/2O}_{2(g)} = \mathrm{2CO_{2(g)} + \mathrm{ H_2O_{(l)}}}, \ \Delta H = +X_4\ \mathrm {{kJ}\ mol^{-1}} {/tex} <br> Enthalpy of formation of {tex}\mathrm {H_2O}_{(l)}{/tex} is