Dalton law of partial pressure | 1st year chemistry chapter 3 short questions notes | dalton law of partial pressure class 11

 

Dalton law of partial pressure. 1st year chemistry chapter 3 short questions notes. Dalton law of partial pressure class 11 

Q) State Dalton's law of partial pressure. Why is it necessary that no forces of attractions should be there to obey this law? 

Ans. Statement : Total pressure exerted by mixture of gases is equal to sum of individual partial  pressures of gases at given temperature. 

Mathematically:  

P_t = P₁ + P₂ + P₃

_{If forces of attraction present between molecules of gases then total pressure will be less than individual partial pressure of gases. Therefore it is necessary that no forces of attraction should be there to obey this law.}  

_{Q) Define Mole fraction of gas.}

_{Ans. It is the ratio of number of moles of a gas to the total number of moles of gases present in a mixture. Its value always smaller than 1.}

_{Q) What is partial pressure? Give its formula.}

_{Ans. Partial pressure is the pressure which is exerted by a gas in a mixture of gases on wall of container.} 

_{Mathematically:}     P_A = P_t X_A  

Partial pressure of a gas is equal to product of total pressure and mole fraction of that gas. 

Q) What is aqueous tension?

Ans. The pressure exerted by only water vapours at constant temperature is called  aqueous tension.

Q) How do you say that the pressure of the dry gas is equal to the difference of total pressure and aqueous tension of H₂O?

Ans. In laboratory, most gases are collected over water. Water vapours also join with gas. Hence to calculate the partial pressure of only gas, vapour pressure of water (aqueous tension) is subtracted from total pressure.

Q) Why pilots feel uncomfortable breathing at high altitude and divers cannot use normal air?

Ans. Breathing at higher altitudes:

At higher altitude partial pressure of oxygen in cabin less than partial pressure in lungs. Therefore, pilots feel uncomfortable breathing at high altitude.

Breathing in the depth of sea:

At the depth of sea, partial pressure of oxygen higher than as in normal air. Moreover, nitrogen diffuse in blood as the depth of sea increased. Therefore, divers cannot use normal air. 

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