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Out of the three states of matter, only ...

Out of the three states of matter, only the gases have most of the physical properties common. They neither have definite shapes nor volumes. Upon mixing they form homogeneous mixture irrespective of their nature and can also be compressed on applying pressure. In addition to these, the gases obey different gas laws such as Boyle's Law, Charles's Law, Dalton's Law of partial pressures, Graham's Law of diffusion etc. Based upon these laws, ideal gas equation `PV = nRT` has been derived.
Which pair of gaseous species diffuse through a small jet with the same rate of diffusion at same P and T ?

A

`NO,CO`

B

`NO,CO_(2)`

C

`NH_(3), PH_(3)`

D

`NO, C_(2)H_(6)`

Text Solution

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The correct Answer is:
To determine which pair of gaseous species diffuse through a small jet at the same rate under the same pressure and temperature, we can utilize Graham's Law of Diffusion. According to this law, the rate of diffusion of a gas is inversely proportional to the square root of its molar mass. Therefore, gases with the same molar mass will diffuse at the same rate. ### Step-by-step solution: 1. **Identify the gaseous species in the options**: We need to look at the pairs of gases provided in the question. 2. **Calculate the molar mass of each gas**: - **Option A**: NO and CO - Molar mass of NO: Nitrogen (N) = 14 g/mol + Oxygen (O) = 16 g/mol = 30 g/mol - Molar mass of CO: Carbon (C) = 12 g/mol + Oxygen (O) = 16 g/mol = 28 g/mol - **Option B**: NO and CO2 - Molar mass of CO2: Carbon (C) = 12 g/mol + 2 × Oxygen (O) = 2 × 16 g/mol = 44 g/mol - **Option C**: NH3 and PS3 - Molar mass of NH3: Nitrogen (N) = 14 g/mol + 3 × Hydrogen (H) = 3 × 1 g/mol = 17 g/mol - Molar mass of PS3: Phosphorus (P) = 31 g/mol + 3 × Sulfur (S) = 3 × 32 g/mol = 97 g/mol - **Option D**: NO and C2H6 - Molar mass of C2H6: 2 × Carbon (C) = 2 × 12 g/mol + 6 × Hydrogen (H) = 6 × 1 g/mol = 30 g/mol 3. **Compare the molar masses**: - In **Option A**, NO (30 g/mol) and CO (28 g/mol) have different molar masses. - In **Option B**, NO (30 g/mol) and CO2 (44 g/mol) have different molar masses. - In **Option C**, NH3 (17 g/mol) and PS3 (97 g/mol) have different molar masses. - In **Option D**, NO (30 g/mol) and C2H6 (30 g/mol) have the same molar mass. 4. **Conclusion**: Since only the gases in Option D (NO and C2H6) have the same molar mass, they will diffuse at the same rate under the same conditions of pressure and temperature. ### Final Answer: The pair of gaseous species that diffuse through a small jet with the same rate of diffusion at the same pressure and temperature is **NO and C2H6**.
To determine which pair of gaseous species diffuse through a small jet at the same rate under the same pressure and temperature, we can utilize Graham's Law of Diffusion. According to this law, the rate of diffusion of a gas is inversely proportional to the square root of its molar mass. Therefore, gases with the same molar mass will diffuse at the same rate. ### Step-by-step solution: 1. **Identify the gaseous species in the options**: We need to look at the pairs of gases provided in the question. 2. **Calculate the molar mass of each gas**: - **Option A**: NO and CO ...
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State Graham's law of diffusion.

Boyle.s Law is

Dalton's law of partial pressure are applicable to

What is the use of Dalton's law of partial pressure ?

Dalton's law of partial pressures is not applicable to