CBSE Questions for Class 11 Medical Chemistry States Of Matter Gases And Liquids Quiz 13 - MCQExams.com

The vapour pressure of pure water at $$25^{\circ}C$$ is $$30\ mm$$. The vapour pressure of $$10\%\ (W/W)$$ glucose  solution at $$25^{\circ}C$$ is :
  • $$31.5\ mm$$
  • $$30.6\ mm$$
  • $$29.67\ mm$$
  • $$26.56\ mm$$
 For the adiabatic expansion of an ideal gas
  • PV $$^{\gamma}$$= constant
  • TV $$^{\gamma-1}$$ = constant
  • T $$^{\gamma}$$P $$^{1-\gamma}$$ =constant
  • All of these
A reaction follows the given concentration (M)- time graph. The rate for the reaction at 20 seconds will be
1182476_9ec368e9033747469f0e8f612103d38c.jpg
  • 410 MS
  • 810 MS
  • 210 MS
  • 710 MS
5.40 gm of an unknown gas at $${\text{2}}{{\text{7}}^{\text{o}}}{\text{C}}\,\,$$ occupies the same volume as 0.14 gm of hydrogen at $$1{{\text{7}}^{\text{o}}}{\text{C}}$$ and same pressure. The molecular weight of unknown gas is 
  • 79.8
  • 81
  • 79.2
  • 83
At point P and Q,the real gas deviation with respect to ideal gas is respectively 
1199324_e20da8cd0975400eaf2bedf5ba3abc23.PNG
  • Positive,negative
  • Positive, positive
  • Negative,Positive
  • Negative,Negative
The vapour pressure of pure benzene at a certain temperature is 200 mm Hg. At the same temperature the vapour pressure of a solution containing 2 g of non volatile non electrolyte solid in 78 g of benzene is 195 mm Hg. What is the molecular mass of solid?
  • 50
  • 70
  • 85
  • 80
One atmosphere is numerically equal to approximately?
  • $${ 10 }^{ 6 }{ dyne\quad cm }^{ -2 }$$
  • $${ 10 }^{ 2 }{ dyne\quad cm }^{ -2 }$$
  • $${ 10 }^{ 4 }{ dyne\quad cm }^{ -2 }$$
  • $${ 10 }^{ 8 }{ dyne\quad cm }^{ -2 }$$
Consider a binary mixture of volatile liquids. If at $$X_A=0.4$$ the vapour pressure of solution is $$580\ torr$$ then the mixture could be $$(p_{A}^{0}=300\ torr, p_{B}^{0}=800\ torr)$$
  • $$CHCl_3-CH_3COCH_3$$
  • $$C_6H_5Cl-C_6H_5Br$$
  • $$C_6H_6-C_6H_5CH_3$$
  • $$nC_6H_{14}-nC_7H_{16}$$
The ratio of densities of a gas at two conditions of temperature and pressure is given by:
  • $$\dfrac{\rho_2}{\rho_1} = \left(\dfrac{p_2}{p_1} \right) \left(\dfrac{T_2}{T_1} \right)$$
  • $$\dfrac{\rho_2}{\rho_1} = \left(\dfrac{p_2}{p_1} \right) \left(\dfrac{T_1}{T_2} \right)$$
  • $$\dfrac{\rho_2}{\rho_1} = \left(\dfrac{p_1}{p_2} \right) \left(\dfrac{T_1}{T_2} \right)$$
  • $$\dfrac{\rho_2}{\rho_1} = \left(\dfrac{p_1}{p_2} \right) \left(\dfrac{T_2}{T_1} \right)$$
$$200\ ml$$ of $$He$$ at $$0.66\ atm$$ pressure and $$400\ ml$$ of $${ O }_{ 2 }$$ at $$0.52\ atm$$ pressure are mixed in a $$400\ ml$$ vessel at $${ 25 }^{ \circ  }C$$. The partial pressure of $$He$$ and  $${ O }_{ 2 }$$ will be:
  • $$0.33\ and\ 0.56$$
  • $$0.33\ and\ 0.52$$
  • $$0.38\ and\ 0.56$$
  • $$0.25\ and\ 0.45$$
Calculate solubility (in moles / litre) of a saturated aqueous solution of $$Ag_3PO_4$$ if the vapour pressure of the solution becomes 750 torr at 373 K
(Assume molality=molarity).
  • $$2/15$$
  • $$1/30$$
  • $$10/54$$
  • $$20/27$$
18 g of glucose $${ (C }_{ 6 }{ H }_{ 12 }{ O }_{ 6 })$$ is added to 178.2 g of water. The vapour pressure of water for this aqueous solution at $${ 100 }^{ \circ  }C$$ is ?
  • 7.60 Torr
  • 76.00 Torr
  • 752.40 Torr
  • 759.00 Torr
Which of the following attraction is strongest? 
Liquids $$A$$ and $$B$$ form an ideal solution. At $$30^o$$ C, the total vapour pressure of a solution containing $$1$$ mol of $$A$$ and $$2$$ mols of $$B$$ is $$250$$ mm $$Hg$$. The total vapour pressure becomes $$300$$ mm $$Hg$$ when $$1$$ more mol of A is added to the first solution. The vapour pressures of pure $$A$$ and $$B$$ at the same temperature are 
  • $$450, 150$$ mm $$Hg$$
  • $$150, 450$$ mm $$Hg$$
  • $$250, 300$$ mm $$Hg$$
  • $$125, 150$$ mm $$Hg$$
The equilibrium constant for the following equilibrium is given at $$0^0C$$:

$$Na_2HPO_4.12H_2O(s)\rightarrow Na_2HPO_4.7H_2O(s)+5H_2O(g); K_p=31.25 \times 10^{-13}$$. 

The vapor pressure of water is:
  • $$2 \times 10^{-4}\,atm$$
  • $$5 \times 10^{-4}\,atm$$
  • $$5 \times 10^{-2}\,atm$$
  • $$5 \times 10^{-3}\,atm$$
$$n$$ moles of Helium gas are placed in a vessel of volume $$V$$ Litre. At T K, if $$V_{1}$$ is free volume of Helium then diameter of He atom is 
  • $$\left[\dfrac{3}{2}\dfrac{V_{1}}{\pi N_{A}n}\right]^{1/3}$$
  • $$\left[\dfrac{3}{2}\dfrac{(V-V_{1})}{\pi N_{A}n}\right]^{1/3}$$
  • $$\left[\dfrac{6(V-V_{1})}{\pi N_{A}n}\right]^{1/3}$$
  • $$\left[\dfrac{6V_{1}}{\pi N_{A}n}\right]^{1/3}$$
An ideal gas is compressed in a closed container its U?
  • Increases
  • Decreases
  • Remains same
  • Both $$(1)$$ & $$(2)$$
45.4 L of dinitrogen reacted with 22.7 L of dioxygen and 45.4 L of nitrous oxide was formed. The reaction is given below : 
$$2N_{2(g)}+O_{2(g)}.  \rightarrow .    2N_2O_(g)$$
Which law is being obeyed in this experiment?
  • Gay Lussac's law
  • Law of definite proportion
  • Law of multiple proportion
  • Avogadro's law
Gay Lussac's law is not valid for which chemical reaction?
  • $$2NO(g)+O_2(g)\longrightarrow 2NO_2(g)$$
  • $$2HI(g)\longrightarrow H_2(g)+I_2(g)$$
  • $$4B(s)+3O_2(g)\longrightarrow 2B_2O_3(s)$$
  • $$2SO_2(g)+O_2(g)\longrightarrow 2SO_3(g)$$
A mixture of 50.ml of $$N{H_3}$$ and 60.0 ml of $${O_2}$$ gas react as
$$4N{H_3}(g) + 5{O_2}(g)\xrightarrow{{}}4NO + 6{H_2}O(g)$$
If all the gases are at the same temperature and the reaction continues until one of the gases is completely consumed, what volume of water vapour is produced?
  • 48 mL
  • 60.0mL
  • 72 mL
  • 75.0 mL
Calculate the mass of a non - volatile solute (molar  mass $$40\,\,g mol^{-1}$$) which should be dissolved in $$114g$$ octane to reduce its vapour pressure to $$80\%$$
  • $$2g$$
  • $$4g$$
  • $$8g$$
  • $$10g$$
Consider the followimg Vapour Pressure - Mole fraction graph. SP (Total vapour pressure of the resultant solution) is equal to
1301464_35fd1e25e047480a9b506d47311a4ba6.png
  • PQ+RS
  • PQ+QR+RS
  • SR+SQ
  • PQ+QR
Which of the following solutions will have the lowest vapour pressure?
  • $$0.1 M\  Glucose$$
  • $$0.1 M\  NaCl$$
  • $$0.1 M\  BaCl_2$$
  • $$0.1 M Al_2 (SO_4)_3$$
At $${40^ \circ }C$$ the vapour pressure ( in torr ) of a mixture of methyl alcohol and ethyl alcohol is represented by $$P = 199x + 135$$
(where $$x$$ is the mole fraction of methyl alcohol) 
What are the vapour pressures of pure methyl alcohol and pure ethyl alcohol at $${40^ \circ }C$$ ?
  • $$135$$ and $$254$$ torr
  • $$119$$ and $$135$$ tor
  • $$119$$ and $$254$$ torr
  • $$334$$ and $$135$$ torr
Vapour Pressure of methyl alcohol and ethyl alcohol solution is represented by $$P=115{ x }_{ A}+140$$. Where $${ x }_{ A }$$ is the mole fraction of methyl alcohol. The value of $$\lim _{ { x }_{ A }\rightarrow 0 }{ \frac { { P }_{ B }^{ 0 } }{ { x }_{ B } }  } \\  $$
  • 255
  • 115
  • 140
  • 135
A rigid vessel of volume 0.50 $$m^3$$ containing $$H_2$$ at $$20.5^0 C$$ and a pressure of $${ 611\times 10 }^{ 3 }$$ Pa is connected to a second rigid vessel of volume 0.75$$m^3$$ containing Ar at $$31.2^0 C$$ at a pressure of $${ 611\times 10 }^{ 3 }$$ Pa and temperature of $$14.5^0 C$$. What is the final pressure of the vessels?
  • $${ 2\times 10 }^{ 5 }$$
  • $${ 3.22\times 10 }^{ 5 }$$ Pa
  • 4840 Pa
  • $${ 4.84\times 10 }^{ 5 }$$ Pa
Calculate the vapour pressure of aqueous 0.1 m glucose solution at 300 K temperature, the vapour pressure of water is 0.03 bar at 300 K temperature.
  • 0.5 bar
  • 0.29 bar
  • 0.3 bar
  • 0.03 bar
$$5.0\ L$$ water placed in a closed room of volume $$2.5\times 10^{4}L$$ having temperature $$300\ K$$. If vapour pressure of water is $$27.0\ mm$$ and density is $$0.990\ g/cm^{3}$$ at this temperature, how much water is left in liquid state?  
  • $$3.444\ L$$
  • $$4.344\ L$$
  • $$4.798\ L$$
  • $$1.212\ L$$
Two liquids A and B have $${P_A}^0:{P_B}^0$$ = 1:3 at a certain temperature. If the mole fraction ratio  $${x_A}:{x_B} = $$ 1:3, the mole fraction of A in vapour in equilibrium with the solution at the given temperature is -        
  • 0.1
  • 0.2
  • 0.5
  • 1.0
How much pressure will be felt by a gas balloon which at $$100m$$ depth in a sea from sea level.
[Pressure at ground level=$$10^5Pa,g=9.8m/s^2$$]
  • $$100Pa$$
  • $$98 Pa$$
  • $$9.8\times 10^5Pa$$
  • $$1.08\times 10^6Pa$$
The vapour pressure of the solution of $$5\,g$$ on non-electrolyte in $$100\,g$$ of water at a particular temperature is $$2950\,N/{m^2}$$. The vapour pressure of water is $$3000\,N/{m^2}$$. The mocular mass of the solute is ?
  • $$54$$
  • $$124$$
  • $$180$$
  • $$340$$
$$300ml$$ of a gas at $$27^o$$C is cooled to $$7^oC$$ at constant pressure, the final volume is 
  • $$540ml$$
  • $$135ml$$
  • $$280ml$$
  • $$350ml$$
The mass of a non-volatile non-electrolyte solute (molar mass$$=50\ g\ mol^ {-1}$$) needed to be dissolved in $$114\ g$$ octane to reduce its vapour pressure to $$75\%$$ is:
  • $$37.5\ g$$
  • $$75\ g$$
  • $$150\ g$$
  • $$50\ g$$
At a certain temperature, the vapour pressure of water is $$50\ mm.$$ The relative lowering of vapour pressure of a solution containing $$36\ g$$ of glucose in $$900\ g$$ of water is
  • $$0.1$$
  • $$0.5$$
  • $$0.004$$
  • $$3.75$$
The vapour pressure of $$1$$ molal glucose solution at $$100^{o}C$$ will be 
  • $$760\ mmHg$$
  • $$76.0\ mmHg$$
  • $$1\ atm$$
  • $$746.32\ mmHg$$
$$0.5$$ moles of gas $$A$$ and $$x$$ moles of gas $$B$$ exert a pressure of $$200$$ Pa in a a container of volume $$10 m^3$$ at $$1000$$ K. Given $$R$$ is the gas constant in $$JK^{-1}$$ mol$$^{_1}$$, $$x$$ is:
  • $$\dfrac{2R}{4+ 12}$$
  • $$\dfrac{2R}{4- 12}$$
  • $$\dfrac{4-R}{2R} $$
  • $$\dfrac{4+R}{2R} $$
At a certain temperature pure liquid A and liquid B have vapour pressures 10 torr and 37 torr respectively. For a certain ideal solution of A and B, the vapour in equilibrium with the liquid has the components A and B in the partial pressure ratio $$P_A : P_B=1 : 7 $$. What is the mole fraction of A in the solution? 
  • 0.346
  • 0.654
  • 0.5
  • None of these
35 ml sample of hydrogen peroxide gives of 500ml of $$O_2$$ at $$27^oC$$ and 1 atm pressure. Volume strength of $$H_2O_2$$ sample will be:-
  • 10 volume
  • 13 volume
  • 11 volume
  • 12 volume
An ideal solution formed by mixing two liquids  'A' and 'B' find the pressure at which $${X_A} = {Y_B}\ ({P_A}^0 = 400\ torr,{P_B}^0 = 100\,torr)$$ 

$$({X_A}$$ and $${Y_B}$$ are mole fraction of A and B in liquid and vapour forms respectively at equilibrium.)
  • 250 torr
  • 200 torr
  • 150 torr
  • 125 torr
At $${35}^{o}C$$, the vapour pressure of $$CS_2$$ is $$512mm$$ $$Hg$$, and acetone is $$344mm$$ $$Hg$$. A solution of $$CS_2$$ and acetone in, which the mol fraction of $$CS_2$$ is $$0.25$$, has a total vapour pressure of $$600mm$$ $$Hg$$. Which of the following statements is/are correct:
  • A mixture of $$100mL$$ of acetone and $$100mL$$ $$CS_2$$ of has a volume is $$200mL$$
  • When acetone and $$CS_2$$ are mixed at $${35}^{o}C$$, heat must be absorbed in order to produce a solution at $${35}^{o}C$$
  • When acetone and $$CS_2$$ are mixed at $${35}^{o}C$$, heat is released
  • There is negative deviation from Raoult's law
Vapour pressure increase with increase in : 
  • Concentration of solution containing non-volatile soulute
  • Temperature up to boiling point
  • Temperature upto triple point
  • Altitude of the concerned place of boiling
Vapour pressure of pure 'A' is 70 mm of Hg at $$25^0C$$ it forms an ideal solution is with 'B' in which mole fraction of A is 0.If the vapour pressure of the solution is 84 mm is Hg at $$25^0C$$, the vapour pressure of pure 'B' at $$25^0C$$ is :
  • 56 mm Hg
  • 70 mm Hg
  • 140 mm Hg
  • 28 mm Hg
A solution is prepared by mixing $${\text{8}}{\text{.5}}\,{\text{g}}$$ of $${\text{C}}{{\text{H}}_{\text{2}}}{\text{C}}{{\text{l}}_2}$$ and $$11.95\,{\text{g}}$$ of $${\text{CHC}}{{\text{l}}_{\text{3}}}$$. If vapour pressure of $${\text{C}}{{\text{H}}_{\text{2}}}{\text{C}}{{\text{l}}_{\text{2}}}$$ and $${\text{CHC}}{{\text{l}}_3}$$ at $${\text{298}}\,{\text{K}}$$ are $$415$$ and $$200\,{\text{mm}}$$ Hg respecetively, then mole fraction of $${\text{CHC}}{{\text{l}}_{\text{3}}}$$ in vapour form is:
  • $$0.162$$
  • $$0.675$$
  • $$0.325$$
  • $$0.486$$
When a solution containing non-volatile solute is diluted with water,
  • its vapour pressure increases
  • its osmotic pressure increases
  • its boiling point increases
  • its freezing point increases
Gaseous mixture contains $$56 g$$ of $$N_{2},44 g$$ of $$CO_{2}$$ and $$16g$$ of $$CH_{4}$$. The total pressure of mixture is $$720mm$$ of Hg. The partial pressure of methane is 
  • $$75 atm$$
  • $$160 atm$$
  • $$180 atm$$
  • $$215 atm$$
The kinetic energy of $$1\ mole$$ of gas is equal to-
  • $$\dfrac {3}{2}RT$$
  • $$\dfrac {3}{2}KT$$
  • $$\dfrac {RT}{2}$$
  • $$\dfrac {2R}{3}$$
Henry's law constant K of $$CO_{2}$$ in water at $$20^{\circ}C$$ is $$3.0\times 10^{-2}molL^{-1}atm^{-1}$$. Calculate the mass of $$CO_{2}$$ present in 100 L of soft drink bottled with a partial pressure of $$CO_{2}$$ of 4 atm at the same temperature
  • 5.28 g
  • 12.0 g
  • 428 g
  • 528 g

Two liquids A and B form ideal solution.At 300K,the vapour pressure of solution containing 1 mol of A and 3 mol of B is 550mm Hg.At the same temperature,if one more mole of B is added to this solution,the vapour pressure of the solution increases by 10mm Hg.Determine the vapour pressures of A and B in their pure states.
  • $$563$$ and $$469$$
  • $$500$$ adn $$1250$$
  • $$513$$ and $$494$$
  • $$400$$ and $$600$$
Pressure remaining constant, the volume of a given sample of gas at $${127}^{o}C$$ will be doubled at
  • $${254}^{o}C$$
  • $${527}^{o}C$$
  • $$600K$$
  • $${800}^{o}C$$

Two flasks of equal volume, connected by a narrow tube of negligible volume, contain $$2$$ moles of $$H_2$$ gas at $$1$$ atm pressure and $$300$$ K. Now, one of the flasks are heated to $$400$$ K and the other is maintained at $$300 K$$, then find final pressure: 
  • $$\cfrac {8}{5}$$ atm
  • $$\cfrac {5}{3}$$ atm
  • $$\cfrac {7}{5}$$ atm
  • $$\cfrac {8}{7}$$ atm
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