CBSE (Science) Class 11CBSE
It's free!


Create free account

      Forgot password?

View all notifications
Books Shortlist
Your shortlist is empty

NCERT solutions Chemistry Class 11 Part 1 chapter 5 States of Matter


NCERT Chemistry Class 11 Part 1

Chemistry Textbook for Class 11 Part 1

Chapter 5 - States of Matter

Pages 152 - 153

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

Q 1 | Page 152

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?

Q 2 | Page 153

Using the equation of state pV nRT; show that at a given temperature density of a gas is proportional to gas pressurep.

Q 3 | Page 153

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

Q 4 | Page 153

The pressure of 1 g 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. Find a relationship between their molecular masses.

Q 5 | Page 153

The drain cleaner, Drainex contains small bits of aluminum which react with caustic soda to produce dihydrogen. What volume of dihydrogen at 20 °C and one bar will be released when 0.15g of aluminum reacts?

Q 6 | Page 153

What will be 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 ?

Q 7 | Page 153

What will be the pressure of the gaseous mixture when 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?

Q 8 | Page 153

The density of a gas is found to be 5.46 g/dm3 at 27 °C at 2 bar pressure. What will be its density at STP?

Q 9 | Page 153

34.05 mL of phosphorus vapour weighs 0.0625 g at 546 °C and 0.1 bar pressure. What is the molar mass of phosphorus?

Q 10 | Page 153

A student forgot to add the reaction mixture to the round-bottomed flask at 27 °C but instead, he/she 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. What fraction of air would have been expelled out?

Q 11 | Page 153

Calculate the temperature of 4.0 mol of a gas occupying 5 dmat 3.32 bar.

(R = 0.083 bar dm3 K–1 mol–1).

Q 12 | Page 153

Calculate the total number of electrons present in 1.4 g of dinitrogen gas.

Q 13 | Page 153

How much time would it take to distribute one Avogadro number of wheat grains, if 1010 grains are distributed each second?

Q 14 | Page 153

Calculate the total pressure in a mixture of 8 g of dioxygen and 4 g of dihydrogen confined in a vessel of 1 dm3 at 27°C. R = 0.083 bar dm3 K1 mol1.

Q 15 | Page 153

Payload is defined as the difference between the mass of displaced air and the mass of the balloon. Calculate the payload when a balloon of radius 10 m, mass 100 kg is filled with helium at 1.66 bar at 27°C. (Density of air = 1.2 kg m3 and R = 0.083 bar dm3 K1 mol1).

Q 16 | Page 153

Calculate the volume occupied by 8.8 g of CO2 at 31.1°C and 1 bar pressure.

R = 0.083 bar L K–1 mol–1.

Q 17 | Page 153

2.9 g of a gas at 95 °C occupied the same volume as 0.184 g of dihydrogen at 17 °C, at the same pressure. What is the molar mass of the gas?

Q 18 | Page 153

A mixture of dihydrogen and dioxygen at one bar pressure contains 20% by weight of dihydrogen. Calculate the partial pressure of dihydrogen.

Q 19 | Page 153

What would be the SI unit for the quantity pV22/n?

Q 20 | Page 153

In terms of Charles’ law explain why –273°C is the lowest possible temperature.

Q 21 | Page 153

The critical temperature  for carbon dioxide and methane are 31.1 °C and –81.9 °C respectively. Which of these has stronger intermolecular forces and why?

Q 22 | Page 153

Explain the physical significance of Van der Waals parameters.

Q 23 | Page 153

NCERT Chemistry Class 11 Part 1

Chemistry Textbook for Class 11 Part 1