Choose the correct option for graphical representation of Boyle's law, which shows a graph of pressure vs. volume of a gas at different temperatures :

1.

2.

3.

4.

Subtopic:  Gas Laws |
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The correct option for the total pressure (in atm) in a mixture of 4 g O2 and 2 g H2 confined in a total volume of one litre at 0$°$C is :
[Given R=0.082 L atm mol-1 K-1, T=273 K]

1. 25.18

2. 26.02

3. 2.518

3. 2.602

Subtopic:  Ideal Gas Law |
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A mixture of ${\mathrm{N}}_{2}$ and Ar gases in a cylinder contains 7 g of ${\mathrm{N}}_{2}$ and 8 g of Ar. If the total pressure of the mixture of the gases in the cylinder is 27 bar, the partial pressure of ${\mathrm{N}}_{2}$ is:

[Use atomic masses (in g ${\mathrm{mol}}^{-1}$): N=14, Ar=40]

1. 12 bar

2. 15 bar

3. 18 bar

4. 9 bar

Subtopic:  Gas Laws |
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The minimum pressure required to compress 600 dm3 of a gas at 1 bar to 150 dm3 at 40°C is

1. 4.0 bar

2. 0.2 bar

3. 1.0 bar

4. 2.5 bar

Subtopic:  Gas Laws |
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A gas at 350 K and 15 bar has molar volume 20 percent smaller than that for an ideal gas under the same conditions. The correct option about the gas and its compressibility factor (Z) is:

1.  Z<1 and repulsive forces are dominant

2.  Z>1 and attractive forces are dominant

3.  Z>1 and repulsive forces are dominant

4.  Z<1 and attractive forces are dominant

Subtopic:  Compressibility Factor |
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In water-saturated air, the mole fraction of water vapor is 0.02. If the total pressure of the saturated air is 1.2 atm, the partial pressure of dry air is-

1. 1.17 atm

2. 1.76 atm

3. 1.27 atm

4.  0.98 atm

Subtopic:  Dalton's Law |
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The volume occupied by 1.8 g of water vapour at 374 ${}^{\mathrm{o}}\mathrm{C}$ and 1 bar pressure will be -

[Use R=0.083 bar ]

1. 96.66 L

2. 55.87 L

3. 3.10 L

4. 5.31 L

Subtopic:  Ideal Gas Law |
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Which one is not the correct mathematical equation for Dalton's Law of partial pressure? Here p = total pressure of a gaseous mixture
1. $$p_i=\chi_ip^o_i,$$ where $$\chi_i=$$ mole fraction of $$i^\text{th}$$ gas in a gaseous mixture
$$p_{i}^{o}=$$ pressure of $$i^\text{th}$$ gas in a pure state
2. $$\mathrm{p}=\mathrm{p}_{1}+\mathrm{p}_{2}+\mathrm{p}_{3}$$
3. $$\mathrm{p}=\mathrm{n}_{1} \frac{\mathrm{RT}}{\mathrm{V}}+\mathrm{n}_{2} \frac{\mathrm{RT}}{\mathrm{V}}+\mathrm{n}_{3} \frac{\mathrm{RT}}{\mathrm{V}}$$
4. $$\mathrm{p}_{i}=\chi_{i} \mathrm{p}$$, where $$\mathrm{p}_{i}=$$ partial pressure of $$i^\text{th}$$ gas
$$\chi_i=$$ mole fraction of $$i^\text{th}$$ gas in a gaseous mixture
Subtopic:  Dalton's Law |
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A 10.0 L flask contains 64 g of oxygen at 27°C. (Assume $$O_2$$ gas is behaving ideally). The pressure inside the flask in the bar is:
(Given R = 0.0831 L bar K-1 mol-1)
1. 4.9
2. 2.5
3. 498.6
4. 49.8
Subtopic:  Ideal Gas Law |
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Which of the following is not correct about postulates of kinetic molecular theory of gases?

 1 . Pressure of the gas is due to the collision of molecules against the walls of the container. 2. Volume of the gas is due to the large number of molecules of the gas. 3. Average kinetic energy of molecules is directly proportional to the absolute temperature of the gas. 4. The molecules move randomly with different speeds in different directions.

Subtopic:  Kinetic Theory of Gas |
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