Question

Two 22.4 litre containers A and B contains 8 g of O2 and 8 g of SO2 respectively at 273 K and 1 atm pressure, then
(a) Number of molecules in A and B are same
(b) Number of molecules in B is more than that in A.
(c) The ratio between the number of molecules in A to number of molecules in B is 2:1
(d) Number of molecules in B is three times greater than the number of molecules in A.

Answer 1

Answer ⇒ Option (a). 

As per as the Avogadro's law, equal volumes of all the gases under similar conditions of the temperature and Pressure contains the equal numbers of the molecules. 
Hence, Option (a). is correct. 

Important Note :-

[Although, Numerically, Option (a) cannot be correct as there is slight error in the question. The mass of the SO₂ must be 16 grams.  
If the mass will be 8 grams only, then it will not obey the Avogadro's law. ]


To prove my statement, calculations is done below. 

Given conditions ⇒ 
Mass of the di-Oxygen = 8 g
Mass of the SO₂ = 8 g.

According to the Avogadro's law, equal volumes of all the gases contains the same numbers of the molecules at the same temperature and pressure. 

Option (a). Statement is correct. 

Numerically it is also proved. 

Number of the molecules of Oxygen  = Mass/Molar Mass × Avogadro's number.
 = 8/32 × 6.022 × 10²³
 = 1.5055 × 10²³ molecules.

Number of the molecules of the SO₂ = 64/32 × 6.022 × 10²³
= 8/64 × 6.022 × 10²³ molecules 
= 0.75275 × 10²³

From this we can observes that the ratio of the numbers of the molecules in A to the numbers of the molecules of B is 2 : 1. 

But it cannot be possible because it will not obey the Avogadro's law. 

Hence, Option (a) is Correct. 


Hope it helps.

Answer 2

Answer:

number of molecules in a and b are same