A 200 mL flask having oxygen at 220 mm and a 300 mL flask having nitrogen at 100 mm are connected in such a way that ${\mathrm{O}}_2 \mathrm{and} {\mathrm{N}}_2$ may combine in their volumes if temperature is kept constant. The total pressure of the gaseous mixture is-

Given below is the graphical representation of volumes occupied by several gases at STP  at Y axis and mass at X axis. find out which gas/gases is/are not placed at the correct position?

If 1 g of each of the following gases are taken at STP, then the gas that will have the highest volume is -

$\mathrm{CO}, {\mathrm{H}}_2\mathrm{O}, {\mathrm{CH}}_4, \mathrm{NO}$

The conditions at which real gas would behave ideally is-

If pressure is in atmosphere and volume in dm³ , then the unit of 'a' is-

The pressure of 1 gm of an ideal gas A at 27 °C is found to be 2 bar. When 2 g of another ideal gas B is introduced in the same flask at the same temperature, the pressure becomes 3 bar.

The correct relationship between their molecular masses is -

 A = $\frac{{\mathrm{pV}}^2{\mathrm{T}}^2}{\mathrm{n}}$ 

The SI unit for the quantity A is -

Assertion: Critical temperatures for carbon dioxide and methane are 31.1 °C and –81.9 °C  respectively.

Reason: The intermolecular forces of attraction are stronger in CO₂ than CH₄

What will be the minimum pressure required to compress 500 dm³ of air at 1 bar to 200 dm³ at 30^°C?

A vessel of 120 mL capacity contains a certain amount of gas at 35 °C and 1.2 bar pressure. The gas is transferred to another vessel of volume 180 mL at 35 °C. What would be its pressure?

At 0^°C, the density of a certain oxide of a gas at 2 bar is the same as that of dinitrogen at 5 bar.

The molecular mass of the oxide would be -

The volume of H₂ that would be released when 0.15 g of aluminium reacts at 20 °C and 1 bar pressure with caustic soda is-

The pressure exerted by a mixture of 3.2 g of methane and 4.4 g of carbon dioxide contained in a 9 dm³ flask at 27 °C would be -

$$\begin{gathered} 1. 8.31 \times {10}^4 \mathrm{Pa} \\ 2. 7.43 \times {10}^{-4 }\mathrm{Pa} \\ 3. 6.87 \times {10}^3 \mathrm{Pa} \\ 4. 8.31 \times {10}^6 \mathrm{Pa} \end{gathered}$$

0.5 L of H₂ at 0.8 bar and 2.0 L of dioxygen at 0.7 bar are introduced in a 1L vessel at 27°C.

The pressure inside the vessel would be -

A student forgot to add the reaction mixture to the round-bottomed flask at 27 °C but instead, he placed the flask on the flame. After a lapse of time, he realized his mistake and using a pyrometer he found the temperature of the flask was 477 °C. The fraction of air that would  expel out would be

The total pressure of a mixture that contains 8 g of O₂ and 4 g of H₂ confined in a vessel of 1 dm³ at 27^°C would be -

(R = 0.083 bar dm³ K^-1mol^-1)

Find the mass of payload of a balloon of radius 10 m, if a mass of 100 kg is filled with helium at 1.66 bar and 27°C temperature:

(Density of air = 1.2 kg m^–3 and R = 0.083 bar dm³ K^–1 mol^–1).

2.9 g of a gas at 95^°C occupies the same volume as 0.184 g of dihydrogen at 17^°C, at the same pressure. The molar mass of the gas is -

A mixture of dihydrogen and dioxygen at one bar pressure contains 20% by weight of dihydrogen. The partial pressure of dihydrogen is -

Van der Waals parameter 'a' signifies -

A plot of volume versus temperature (T) for a gas at constant pressure is a straight line passing through the origin. The plots at different values of pressure are shown in the figure given below.

  
The correct order of pressure is -

         Temperature (K) 

The interaction energy of London force is inversely proportional to sixth power of the distance between two interacting particles. Their magnitude depends upon-

Dipole-dipole forces act between the molecules possessing permanent dipole. Ends of dipoles possess 'partial charges'. The partial charge will be-

As the temperature increases, average kinetic energy of molecules increases. With increase in temperature at constant volume, the pressure -  

Gases possess characteristic critical temperature which depends upon the magnitude of intermolecular forces between the particles. Following are the critical temperatures of some gases.

From the above data, the order of liquefaction of the given gases is-

(write the order from the gas liquefying first)

 In the given figure, the curve represents an ideal gas is-

How does the surface tension of a liquid vary with increase in temperature?

The state of a gas can be described by quoting the relationship between-

The density of a gas is found to be 5.46 g/dm³ at 27^°C at 2 bar pressure. The density of gas at STP would be -

$$\begin{gathered} 1. 2.0 \mathrm{g} {\mathrm{dm}}^{-3} \\ 2. 3.0 \mathrm{g} {\mathrm{dm}}^{-3} \\ 3. 4.5 \mathrm{g} {\mathrm{dm}}^{-3} \\ 4. 1.5 \mathrm{g} {\mathrm{dm}}^{-3} \end{gathered}$$

34.05 mL of phosphorus vapour weighs 0.0625 g at 546 °C and 0.1 bar pressure. The molar mass of phosphorus would be -

$$\begin{gathered} 1. 1247.5 \mathrm{g} {\mathrm{mol}}^{-1} \\ 2. 2234.7 \mathrm{g} {\mathrm{mol}}^{-1} \\ 3. 3126.9 \mathrm{g} {\mathrm{mol}}^{-1} \\ 4. 1134.6 \mathrm{g} {\mathrm{mol}}^{-1} \end{gathered}$$