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**Question 5.1: What will be the minimum pressure required to compress 500 dm ^{3} of air at 1 bar to 200 dm^{3} at 30Â°C?**

Initial pressure,

Initial volume,

Final volume,

Since the temperature remains constant, the final pressure (

According to Boyleâ€™s law,

Therefore, the minimum pressure required is 2.5 bar.**Question 5.2:** **A vessel of 120 mL capacity contains a certain amount of gas at 35 Â°C and 1.2 bar pressure. The gas is transferred to another vessel of volume 180 mL at 35 Â°C. What would be its pressure?****Ans:-** Given,

Initial pressure, *p*_{1} = 1.2 bar

Initial volume, *V*_{1 }= 120 mL

Final volume, *V*_{2} = 180 mL

Since the temperature remains constant, the final pressure (*p*_{2}) can be calculated using Boyleâ€™s law.

According to Boyleâ€™s law,

Therefore, the pressure would be 0.8 bar.**Question 5.3: Using the equation of state pV = nRT; show that at a given temperature density of a gas is proportional to gas pressure p**.

Where,

R â†’ Gas constant

From equation (i) we have,

Replacing

Where,*m* â†’ Mass of gas*M* â†’ Molar mass of gas

But, (*d* = density of gas)

Thus, from equation (ii), we have

Molar mass (*M*) of a gas is always constant and therefore, at constant temperature = constant.

Hence, at a given temperature, the density (*d*) of gas is proportional to its pressure (*p)***Question 5.4: At 0Â°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?****Ans:-** Density (d) of the substance at temperature (*T*) can be given by the expression,

*d* =

Now, density of oxide (*d*_{1}) is given by,

Where, *M*_{1} and *p*_{1} are the mass and pressure of the oxide respectively.

Density of dinitrogen gas (*d*_{2}) is given by,

Where, *M*_{2} and *p*_{2} are the mass and pressure of the oxide respectively.

According to the given question,

Molecular mass of nitrogen, *M*_{2} = 28 g/mol

Hence, the molecular mass of the oxide is 70 g/mol.**Question 5.5: Pressure of 1 g of an ideal gas A at 27 Â°C is found to be 2 bar. When 2 g of another ideal gas B is introduced in the same flask at same temperature the pressure becomes 3 bar. Find a relationship between their molecular masses.****Ans:-** For ideal gas A, the ideal gas equation is given by,

Where, *p*_{A} and *n*_{A} represent the pressure and number of moles of gas A.

For ideal gas B, the ideal gas equation is given by,

Where, *p*_{B }and *n*_{B} represent the pressure and number of moles of gas B.

[*V* and *T* are constants for gases A and B]

From equation (i), we have

From equation (ii), we have

Where, M_{A }and M_{B} are the molecular masses of gases A and B respectively.

Now, from equations (iii) and (iv), we have

Given,

(Since total pressure is 3 bar)

Substituting these values in equation (v), we have

Thus, a relationship between the molecular masses of A and B is given by

.**Question 5.6: The drain cleaner, Drainex contains small bits of aluminum which react with caustic soda to produce dihydrogen. What volume of dihydrogen at 20 Â°C and one bar will be released when 0.15g of aluminum reacts?****Ans:-** The reaction of aluminium with caustic soda can be represented as:

At STP (273.15 K and 1 atm), 54 g (2 Ã— 27 g) of Al gives 3 Ã— 22400 mL of H_{2..}

0.15 g Al gives i.e., 186.67 mL of H_{2.}

At STP,

Let the volume of dihydrogen be at *p*_{2} = 0.987 atm (since 1 bar = 0.987 atm) and *T*_{2} = 20Â°C = (273.15 20) K = 293.15 K._{.}

Therefore, 203 mL of dihydrogen will be released.**Question 5.7: 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 dm ^{3} flask at 27 Â°C ?**

For methane (CHÂ_{4}),

For carbon dioxide (CO_{2}),

Total pressure exerted by the mixture can be obtained as:

Hence, the total pressure exerted by the mixture is 8.314 Ã— 10^{4} Pa.**Question 5.8: What will be the pressure of the gaseous mixture when 0.5 L of H _{2} at 0.8 bar and 2.0 L of dioxygen at 0.7 bar are introduced in a 1L vessel at 27Â°C?**

Now,

p

V

It is known that,

Now, let the partial pressure of O_{2} in the vessel be Po_{2}.

Total pressure of the gas mixture in the vessel can be obtained as:

Hence, the total pressure of the gaseous mixture in the vessel is 1.8 bar.**Question 5.9 : Density of a gas is found to be 5.46g/dm ^{3} at 27Â°C at 2 bar pressure.What will be its density at STP?**

The density (*d*_{2}) of the gas at STP can be calculated using the equation,

Hence, the density of the gas at STP will be 3 g dm^{â€“3}.**Question 5.10: 34.05 mL of phosphorus vapour weighs 0.0625 g at 546 Â°C and 0.1 bar pressure. What is the molar mass of phosphorus?**

**Ans:-** Given,*p* = 0.1 bar*V* = 34.05 mL = 34.05 Ã— 10^{â€“3} L = 34.05 Ã— 10^{â€“3} dm^{3}

R = 0.083 bar dm^{3} K^{â€“1} mol^{â€“1}*T* = 546Â°C = (546 + 273) K = 819 K

The number of moles (*n*) can be calculated using the ideal gas equation as:

Therefore, molar mass of phosphorus = 1247.5 g mol^{â€“1}

Hence, the molar mass of phosphorus is 1247.5 g mol^{â€“1}.**Question 5.11:** **A student forgot to add the reaction mixture to the round bottomed flask at 27 Â°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 Â°C. What fraction of air would have been expelled out?****Ans:-** Let the volume of the round bottomed flask be *V.*

Then, the volume of air inside the flask at 27Â° C is *V.*

Now,*V*_{1} = *V**T*_{1} = 27Â°C = 300 K*V*_{2} =?*T*_{2} = 477Â° C = 750 K

According to Charlesâ€™s law,

Therefore, volume of air expelled out = 2.5 *V* â€“ *V* = 1.5 *V*

Hence, fraction of air expelled out **Question 5.12: Calculate the temperature of 4.0 mol of a gas occupying 5 dm ^{3 }at 3.32 bar. (R = 0.083 bar dm^{3} K^{â€“1} mol^{â€“1}).**

R = 0.083 bar dm

The temperature (T) can be calculated using the ideal gas equation as:

Hence, the required temperature is 50 K.**Question 5.13: Calculate the total number of electrons present in 1.4 g of dinitrogen gas.****Ans:-** Molar mass of dinitrogen (N_{2}) = 28 g mol^{â€“1}

Thus, 1.4 g of

Now, 1 molecule of contains 14 electrons.

Therefore, 3.01 Ã— 10^{23} molecules of N_{2} contains = 14 Ã— 3.01 Ã— 1023

= 4.214 Ã— 10^{23} electrons**Question 5.14: How much time would it take to distribute one Avogadro number of wheat grains, if 10 ^{10} grains are distributed each second?**

Thus, time required

=

Hence, the time taken would be 1.9090 X 10^{6} years..**Question 5.15: Calculate the total pressure in a mixture of 8 g of dioxygen and 4 g of dihydrogen confined in a vessel of 1 dm ^{3} at 27Â°C. R = 0.083 bar dm^{3} K^{â€“1} mol^{â€“1.}**

**Ans:-** Given,

Mass of dioxygen (O_{2}) = 8 g

Thus, number of moles of

Mass of dihydrogen (H_{2}) = 4 g

Thus, number of moles of

Therefore, total number of moles in the mixture = 0.25 2 = 2.25 mole

Given,*V* = 1 dm^{3}*n* = 2.25 mol

R = 0.083 bar dm^{3} K^{â€“1} mol^{â€“1}*T* = 27Â°C = 300 K

Total pressure (*p*) can be calculated as:*pV* =* n*R*T*

Hence, the total pressure of the mixture is 56.025 bar.**Question 5.16:** **Pay load is defined as the difference between the mass of displaced air and the mass of the balloon. Calculate the pay load when a balloon of radius 10 m, mass 100 kg is filled with helium at 1.66 bar at 27Â°C. (Density of air = 1.2 kg m ^{â€“3} and R = 0.083 bar dm^{3} K^{â€“1} mol^{â€“1}).**

Radius of the balloon,

Volume of the balloon

Thus, the volume of the displaced air is 4190.5 m^{3}.

Given,

Density of air = 1.2 kg m^{â€“3}

Then, mass of displaced air = 4190.5 Ã— 1.2 kg

= 5028.6 kg

Now, mass of helium (*m*) inside the balloon is given by,

Now, total mass of the balloon filled with helium = (100 1117.5) kg = 1217.5 kg

Hence, pay load = (5028.6 â€“ 1217.5) kg = 3811.1 kg

Hence, the pay load of the balloon is 3811.1 kg.**Question 5.17: Calculate the volume occupied by 8.8 g of CO _{2} at 31.1Â°C and 1 bar pressure. (R = 0.083 bar L K^{â€“1} mol^{â€“1}).**

**Ans:-** It is known that,

Here,*m* = 8.8 g

R = 0.083 bar LK^{â€“1} mol^{â€“1}*T* = 31.1Â°C = 304.1 K*M* = 44 g*p* = 1 bar

Hence, the volume occupied is 5.05 L.**Question 5.18: 2.9 g of a gas at 95 Â°C occupied the same volume as 0.184 g of dihydrogen at 17 Â°C, at the same pressure. What is the molar mass of the gas****Ans:-** Volume (*V*) occupied by dihydrogen is given by,

Let M be the molar mass of the unknown gas. Volume (*V*) occupied by the unknown gas can be calculated as:

According to the question,

Hence, the molar mass of the gas is 40 g mol^{â€“1}.**Question 5.19: A mixture of dihydrogen and dioxygen at one bar pressure contains 20% by weight of dihydrogen. Calculate the partial pressure of dihydrogen.****Ans:-** Let the weight of dihydrogen be 20 g and the weight of dioxygen be 80 g.

Then, the number of moles of dihydrogen, and the number of moles of dioxygen, .

Given,

Total pressure of the mixture, *p*_{total }= 1 bar

Then, partial pressure of dihydrogen,

Hence, the partial pressure of dihydrogen is.**Question 5.20: What would be the SI unit for the quantity pV^{2}T ^{2}/n?**

The SI unit for volume,

The SI unit for temperature,

The SI unit for the number of moles,

Therefore, the SI unit for quantity is given by,

**Question 5.21: In terms of Charlesâ€™ law explain why â€“273Â°C is the lowest possible temperature.****Ans:-** Charlesâ€™ law states that at constant pressure, the volume of a fixed mass of gas is directly proportional to its absolute temperature.

It was found that for all gases (at any given pressure), the plots of volume vs. temperature (in Â°C) is a straight line. If this line is extended to zero volume, then it intersects the temperature-axis at â€“ 273Â°C. In other words, the volume of any gas at â€“273Â°C is zero. This is because all gases get liquefied before reaching a temperature of â€“ 273Â°C. Hence, it can be concluded that â€“ 273Â°C is the lowest possible temperature.

**Question 5.22: Critical temperature for carbon dioxide and methane are 31.1 Â°C and â€“81.9 Â°C respectively. Which of these has stronger intermolecular forces and why?**

**Ans:-** Higher is the critical temperature of a gas, easier is its liquefaction. This means that the intermolecular forces of attraction between the molecules of a gas are directly proportional to its critical temperature. Hence, intermolecular forces of attraction are stronger in the case of CO_{2}.**Question 5.23: Explain the physical significance of Van der Waals parameters.****Ans:-** **Physical significance of â€˜aâ€™:**

â€˜aâ€™ is a measure of the magnitude of intermolecular attractive forces within a gas.

**Physical significance of â€˜bâ€™:**

â€˜bâ€™ is a measure of the volume of a gas molecule.

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