According to the Dalton’s law of partial pressures, the total pressure of a mixture of ideal gases is equal to the

The highest pressure gas of a mixture has partial pressure p, the partial pressure of other gases decreases by factor of 2n-1, the partial pressure of second gases decreases by a factor of 2, partial pressure of third gas increases by 4, and so on, if the total pressure of gas mixture is 31p/16, how many gases are present in the mixture?

A

3

B

5

C

10

According to Dalton's law of partial pressures, (where pb = Barometric pressure, pa = Partial pressure of dry air and pv = Partial pressure of water vapour)

A

Pb = pa - pv

B

Pb = pa + pv

C

Pb = pa × pv

D

$${\text{Pb}} = \frac{{{\text{pa}}}}{{{\text{pv}}}}$$

Dalton’s law of partial pressure states that the total pressure exerted by a mixture of gas and vapour is the sum of partial pressure of the gas and partial pressure of the vapour at the common temperature.

A

True

B

False

The Henry’s law constant for O2 in water at 25°C is 1.27×10−3M/atm and the mole fraction of O2 in the atmosphere is 0.21. Calculate the solubility of O2 in water at 25°C at an atmospheric pressure of 1.00 atm. Strategy: ▪ Use Dalton’s law of partial pressures to calculate the partial pressure of oxygen. ▪ Use Henry’s law to calculate the solubility, expressed as the concentration of dissolved gas.

A

2.5×10-4 M

B

2.1×10-4 M

C

2.3×10-4 M

D

2.7×10-4M

Which of the following statements about partial pressure are correct? Statement 1: The partial pressure of each gas in a mixture is not proportional to its mole fraction.. Statement 2: The partial pressure of each gas is the product of the total pressure and the mole fraction of that gas.

A

True, False

B

True, True

C

False, True

D

False, False

If u (x, y, z, t) = f(x + iβy - vt) + g(x - iβy - vt), where f and g are arbitrary and twice differentiable functions, is a solution of the wave equation $$\frac{{\partial {u^2}}}{{\partial {x^2}}} = \frac{{{\partial ^2}u}}{{\partial {y^2}}} = \frac{1}{{{c^2}}}\frac{{{\partial ^2}u}}{{\partial {t^2}}}$$ then β is

A

$${\left( {1 - \frac{v}{c}} \right)^{\frac{1}{2}}}$$

B

$$\left( {1 - \frac{v}{c}} \right)$$

C

$${\left( {1 - \frac{{{v^2}}}{{{c^2}}}} \right)^{\frac{1}{2}}}$$

D

$$\left( {1 - \frac{{{v^2}}}{{{c^2}}}} \right)$$

Consider a mixture of three gases a, b and c at equilibrium. If the individual gas components have pressures equal to Pa, Pb and Pc, determine the total pressure P of the mixture of gases. / (Pa + Pb + Pc) d) P = (Pa x Pb / Pc) + (Pb x Pc / P

A

P = Pa + Pb + Pc / (Pa + Pb + Pc) d) P = (Pa x Pb / Pc) + (Pb x Pc / P] + (Pc x Pa / P

B

P = Pa x Pb x Pc /(Pa + Pb + P

C

[ P = [(Pa x Pb) + (Pb x P[ + (Pc x Pa)

D

(Pa x Pb) + (Pb x Pc) + (Pc x Pa)

According to Dalton's law, the total pressure of the mixture of gases is equal to

A

Greater of the partial pressures of all

B

Average of the partial pressures of all

C

Sum of the partial pressures of all

D

Sum of the partial pressures of all divided by average molecular weight

A binary mixture of oxygen and nitrogen with partial pressures in the ratio 0.21 and 0.79 is contained in a vessel at 300 K. If the total pressure of the mixture is 1 * 10 5 N/m2, find the average molecular weight of the mixture

A

28.84

B

29.84

C

30.84

D

31.84

If partial pressure of air and steam be ‘pa’ and ‘ps’ respectively in a condenser, then according to Dalton's law, the pressure in condenser is equal to

A

ps - pa

B

pa - ps

C

pa + ps

D

None of these