2.3 grams of a mixture of ${\mathrm{NO}}_{2}$ and ${\mathrm{N}}_{2}{\mathrm{O}}_{4}$ have a pressure of 0.82 atm at temperature, T K and volume, V litres. If $\frac{\mathrm{V}}{\mathrm{T}}=\frac{1}{300}$magnitude, calculate ${{\mathrm{P}}_{\mathrm{NO}}}_{2}.$ Assume that all the ${\mathrm{NO}}_{2}$ was formed ${\mathrm{N}}_{2}{\mathrm{O}}_{4}$.

(A) 0.52 atm

(B) 0.38 atm

(C) 0.19 atm

(D) 0.41 atm

Concept Questions :-

Dalton's Law
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At a certain temperature for which , the density of a gas, in , is , where P is the pressure in atmosphere. The molecular weight of the gas in  is

(A) 25

(B) 50

(C) 75

(D) 10

Concept Questions :-

Ideal Gas Law
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An evacuated glass vessel weighs  when empty,  when filled with a liquid of density  and 50.5 g when filled with an ideal gas at  at . Determine the molar mass or the gas.

(A)

(B)

(C)

(D)

Concept Questions :-

Ideal Gas Law
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The average speed at ${\mathrm{T}}_{1}$ (in kelvin) and the most probable speed at ${\mathrm{T}}_{2}$ (in kelvin) of ${\mathrm{CO}}_{2}$ gas is . Calculate the values of ${\mathrm{T}}_{1}$ and ${\mathrm{T}}_{2}$.

(A) 1682.5 K, 2143.4 K

(B) 1312.5 K, 1243.4 K

(C) 1881.5 K, 2233.4 K

(D) 1712.5 K, 24.13.4 K

Concept Questions :-

Molecular Velocity
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Two flasks of equal volume connected by a narrow tube (of negligible volume) at 27ºC and contain 0.70 mole of ${\mathrm{H}}_{2}$ at 0.5 atm. One of the flasks is then immersed into a hot bath, kept at 127ºC, while the other remains at 27ºC. Calculate the final pressure.

(A) 5.714 atm

(B) 0.5714 atm

(C) 2.5214 atm

(D) 5.5114 atm

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A gas bulb of 1 litre capacity contains  molecules of nitrogen exerting a pressure of . Calculate the root mean square (rms) speed and the temperature of the gas molecules. If the ratio of most probable speed to the root mean square speed is 0.84, calculate the most probable speed for these molecules at this temperature.

(A)

(B)

(C)

(D)

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A mixture of 10 ml  has a vapour density of 11.3. Mixture contains x ml of ${\mathrm{CH}}_{4}$ , y ml of ${\mathrm{C}}_{2}{\mathrm{H}}_{4}$ and z ml of ${\mathrm{C}}_{2}{\mathrm{H}}_{2}$. When 30 ml of oxygen are sparked together over aqueous KOH, the volume contracts to 5.5 ml and then disappears when pyrogallol is introduced. If volumes are measured in the same conditions of pressure, temperature and humidity, value of x, y and z is–

(A) 4, 3, 3

(B) 1, 2, 3

(C) 2, 1, 1,

(D) 3, 4, 2

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The pressure in bulb dropped from 2000 to 1500 mm Hg in 47 mins. when the ${\mathrm{O}}_{2}$ present in the bulb leaked through a small hole. The bulb was then completely evacuated. A mixture of ${\mathrm{O}}_{2}$ and another gas of molecular weight of 79 in the molar ratio 1 : 1 at a total pressure of 400 mm Hg was introduced. Find the mole ratio of two gases remaining in the bulb after a period of 74 mins.

(A) 1 : 1.236

(B) 1 : 2.136

(C) 1 : 3.336

(D) 2 : 1.136

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The average molecular weight of air is . At 20ºC, the pressure of air at a height of 6 km is half of that at the sea level. Assuming that air contains minute quantities of hydrogen, at what height the partial pressure of hydrogen would be one fourth of the partial pressure at the sea level ? The temperature may be assumed to be the same.

(A) 172.8 km

(B) 4.8 km

(C) 86.4 km

(D) 9.6 km

Concept Questions :-

Ideal Gas Law
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Two gases occupy two containers A and B the gas in A, of volume 0.10 ${\mathrm{m}}^{3}$, exerts a pressure of 1.40 MPa and that in B of volume 0.15 ${\mathrm{m}}^{3}$ exerts a pressure 0.7 MPa. The two containers are united by a tube of negligible volume and the gases are allowed to intermingle. Then if the temperature remains constant, the final pressure in the container will be (in MPa)

(A) 0.70

(B) 0.98

(C) 1.40

(D) 210

Concept Questions :-

Ideal Gas Law
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