Question 1 :
Ortho-Nitrophenol is less soluble in water than {tex} p {/tex} - and {tex} m - {/tex} Nitrophenols because:

Question 6 :
Polarization is the distortion of shape of an anion by the cation. Which statement is correct?

Question 9 :
When 2 hydrogen atoms combine to form $H_2$ molecule, the system ______ .

Question 10 :
In which of the following species the interatomic bond angle is {tex} 109 ^ { \circ } 28 ^ { \text {' } } {/tex} ?

Question 11 :
The regular three dimensional order of molecules is present in :

Question 12 :
For the non-zero values of force of attraction between gas molecules, gas equation will be :

Question 14 :
A sample of an ideal gas was heated from 300C to 600C at constant pressure. Which of the following statement(s) is/are true.

Question 16 :
In van der Waals equation of state of the gas law, the constant {tex}'b'{/tex} is a measure of

Question 19 :
When you open a soft drink bottle, the bubbles oozes through the opening. The bottle contains gas which is highly compressed. Guess the gas.

Question 20 :
Choose the correct statement for change of states of matter :-<br><br><br>

Question 22 :
Pressure remaining constant, the volume of a fixed mass of a gas is directly proportional to its absolute temperature. This law is popularly known as :

Question 24 :
A graph is plotted between pressure and volume at different temperatures. On the basis of the graph what changes will you observe in the volume if <br>(i) The pressure is increased at constant temperature.<br>(ii) The temperature is decreased at constant pressure. <br><img style='object-fit:contain' src='https://storage.googleapis.com/teachmint/question_assets/JEE%20Main/5e798592c6cb6261b35b2e2c' height='108' width='131' >

Question 26 :
At what temperature will the total KE of 0.30 mol of He be the same as the total KE of 0.40 molAr at 400 K ?

Question 28 :
What volume of hydrogen gas, at 273 K and 1 atm pressure will be consumed in obtaining 21.6g of elemental boron (atomic mass = 10.8) from the reduction of boron trichloride by hydrogen?

Question 29 :
The sun and stars glow because of the presence of :

Question 30 :
A certain volume of argon gas (Mol. Wt. = 40) requires 45 s to effuse through a hole at a certain pressure and temperature. The same volume of another gas of unknown molecular weight requires 60 s to pass through the same hole under the same conditions of temperature and pressure. The molecular weight of the gas is :

Question 31 :
<font>My mass 100 kg. But I want to fly in the sky with the help of balloons. Each balloon contain 20 moles of H</font>_{<font>2</font>}<font>(g) at the atmospheric temperature 300 K and at pressure of 0.05 atm. The mass of each balloon is 2.5 kg. The density of air = 1.25 gm/L and g = 10 m/s</font>^{<font>2</font>}<font> . How many minimum such balloon do I need to attach with myself to fly in the sky ?</font></p>

Question 32 :
</font><font color="#000000"><font>The correct order of normal boiling points of O</font></font><font>2, N2, NH3 and CH4, for whom the values of vander Waal's constant ‘a’ are 1.360, 1.390, 4.170 and 2.253 L2. atm. mol</font><font face="Symbol, serif"><font></font></font><font>2 respectively, is :</font></p> <p align="justify"> <font color="#000000">

Question 33 :
<font> 25 ml of O</font>_{<font>2</font>}<font> contracts to 20 ml when subjected to silent electric discharge in an ozoniser. What further contraction would be observed if the partially ozonised oxygen is treated with oil of cinnamon (which absorbs ozone). All volumes are reported at the same temperature and pressure -</font></p>

Question 34 :
</font><font color="#000000"><font>If P is the pressure of gas, then the kinetic energy per unit volume of the gas is :</font></font></p>

Question 35 :
</font><font color="#000000"><font>A gaseous hydrocarbon gives upon combustion 0.72 g of water and 3.08 g. of CO</font></font><font>2. The empirical formula of the hydrocarbon is :</font></p> <p align="justify"> <font color="#000000">

Question 36 :
</font><font color="#000000"><font>A chemist has synthesized a greenish yellow gaseous compound of chlorine and oxygen and finds that its density is 7.71 g/L at 36°C and 2.88 atm. Then the molecular formula of the compound will be</font></font></p> <p align="justify"> <font color="#000000">

Question 37 :
</font><font color="#000000"><font>A sample of an ideal gas was heated from 30</font></font><font>0C to 600C at constant pressure. Which of the following statement(s) is/are true.</font></p> <p align="justify"> <font color="#000000">

Question 38 :
<font>The time taken for a certain volume of a gas ‘X’ to diffuse through a small hole is 2 minutes. It takes 5.65 minutes for oxygen to diffuse under the similar conditions. The molecular weight of ‘X’ is</font></p>

Question 39 :
<font>Calculate the compressibility factor for CO2, if one mole of it occupies 0.4 litre at 300 K and 40 atm. Comment on the result.</font></p>

Question 40 :
<font>Regarding the solubility of gas which of the following is/are incorrect ?</font></p>

Question 41 :
<font>According to Charle’s law, at constant pressure, 100 ml of a given mass of a gas with </font> <img style='object-fit:contain' align="bottom" height="19" src="https://storage.googleapis.com/teachmint/question_assets/JEE%20Main/5fc0e87f75b85f121f540c59" width="37"/> <font> rise in temperature will become </font> <img style='object-fit:contain' align="bottom" height="41" src="https://storage.googleapis.com/teachmint/question_assets/JEE%20Main/5fc0e87f75b85f121f540c5a" width="104"/> </p>

Question 42 :
<font>An ideal gas is taken around the cycle ABCA as shown in P-V diagram. The net work done during the cycle is equal to -</font></p> <p> <img style='object-fit:contain' align="bottom" height="160" src="https://storage.googleapis.com/teachmint/question_assets/JEE%20Main/5fc0e8cb75b85f121f540da0" width="177"/> </p>

Question 43 :
</font><font color="#000000"><font>See the figure-1 :</font></font></p> <p align="center"> <img style='object-fit:contain' align="bottom" height="82" src="https://storage.googleapis.com/teachmint/question_assets/JEE%20Main/5fc0e9244265580f62ccbbf8" width="274"/> </p> <p align="justify"> <font color="#000000"><font>The valves of X and Y are opened simultaneously. The white fumes of NH</font></font><font>4Cl will first form at:</font></p> <p align="justify"> <font color="#000000">

Question 44 :
<font>For a gas isotherm of d/p (y-axis) v/s pressure (P) (x-axis) passes through the points (4, 2.5) and <br/> (10, 5.5). The molar mass of gas is - </font> </p> <p align="justify"> <font>(T = 300 K, density d in g/L and P in atm)</font></p>

Question 45 :
<font>A real gas most closely approaches the behaviour of an ideal gas at -</font></p> <p align="justify"> <font color="#000000">

Question 46 :
<font>An electric bulb was filled with 100 cc of argon gas (At. mass = 40) at 25°C and 1 atm pressure. The number of atoms of argon present in the bulb is -</font></p>

Question 47 :
</font><font color="#000000"><font>The ratio between the r.m.s. velocity of H</font></font><font>2 at 50 K and that of O2 at 800 K is:</font></p> <p align="justify"> <font color="#000000">

Question 48 :
</font><font color="#000000"><font>Consider the following statements: If the van der Waal’s parameters of two gases are given as</font></font></p> <p align="justify"> <font color="#000000"><font> a (atm lit</font></font><font>2mol-2) b (lit mol-1)</font></p> <p align="justify"> <font>Gas X: 6.5 0.056</font></p> <p align="justify"> <font>Gas Y: 8.0 0.011</font></p> <p align="justify"> <font>then (i) : VC (X) &lt; VC (Y) (ii) : PC (X) &lt; PC (Y) </font></p> <p align="justify"> <font>(iii) : TC (X) &lt; TC(Y)</font></p> <p align="justify"> <font>Select correct alternate:</font></p> <p align="justify"> <font color="#000000">

Question 49 :
</font><font color="#000000"><font>A liquid is kept in a closed vessel. If a glass plate of negligible mass with small hole is kept on top of the liquid surface, then vapour pressure of the liquid in the vessel is -</font></font></p>

Question 50 :
<font>The pressure of 2 moles of an ideal gas at 546 K having volume 44.8 L is</font></p>