CBSE Questions for Class 11 Engineering Chemistry States Of Matter Quiz 11 - MCQExams.com

The density of a liquid is 1.2 g/mL. That are 35 drops in 2 mL. The number of molecules in 1 drop is (molecular weight of liquid = 70): 
  • $$\frac{1.2}{35} N_A$$
  • $$\left (\frac{1}{35} N_A \right )^2$$
  • $$\frac{1.2}{(35)^2} N_A$$
  • $$1.2 N_A$$
The reaction, $$ZnO(s)+CO(g) \rightleftharpoons  Zn(g)+{CO}_{2}(g)$$, has an equilibrium constant of $$1$$ atm at $$1500K$$. The equilibrium partial pressure of zinc vapour in a reaction vessel if an equimolar mixture of $$CO$$ and $${CO}_{2}$$ is brought into contact with solid $$ZnO$$ at $$1500K$$ and the equilibrium is achieved at $$1$$ atm is?
  • $$0.68$$ atm
  • $$0.76$$ atm
  • $$0.24$$ atm
  • $$0.5$$ atm
Dalton's law of partial pressure will not apply to which of the following mixture of gases?
  • $$H_{2}$$ and $$SO_{2}$$
  • $$H_{2}$$ and $$Cl_{2}$$
  • $$H_{2}$$ and $$CO_{2}$$
  • $$CO_{2}$$ and $$Cl_{2}$$
Equal mass of $$H_2$$, $$He$$ and $$CH_4$$ are mixed in empty container at $$300$$K, when total pressure is $$2.6$$ atm. The partial pressure of $$H_2$$ in the mixture is:
  • $$2.1$$ atm.
  • $$1.6$$ atm.
  • $$0.8$$ atm.
  • $$0.2$$ atm.
$$18$$ g glucose ($$C_6H_{12}O_6$$) is added to $$178.2$$ g of water. The vapour pressure of this aqueous solution at $$100^0C$$ in torr is:
  • $$7.60$$
  • $$76.00$$
  • $$752.40$$
  • $$759.00$$
4 g argon (Atomic mass=40) in a bulb is at a temperature of T K has a pressure P atm. When the bulb was placed in hot bath at a temperature $$50^0 C$$ more than the first one, 0.8 g of gas had to be removed to get the original pressure. T is equal to :
  • 510 k
  • 200 k
  • 100 k
  • 73 k
A sample of an ideal gas with initial pressure P and volume V is taken through an isothermal process during which entropy change is found to be $$\Delta$$S. The universal gas constant is R. Then, the work done by the gas is given by:
  • $$\displaystyle\frac{PV\Delta S}{nR}$$
  • $$nR\Delta S$$
  • PV
  • $$\displaystyle\frac{P\Delta S}{nRT}$$
A gaseous mixture contains $$56\ g\ N_{2}. 44\ g\ CO_{2}$$ and $$16\ g\ CH_{4}$$. The total pressure of the mixture is $$720\ mm\ Hg$$. The partial pressure of $$CH_4$$ in mm Hg is:
  • $$620\ mm$$ of $$Hg$$
  • $$180\ mm$$ of $$Hg$$
  • $$160\ mm$$ of $$Hg$$
  • $$200\ mm$$ of $$Hg$$
The vapour pressure of pure benzene at a certain temperature is $$640\ mm\ Hg$$. A non-volatile solute weighing $$2.175\ g$$ is added to $$39.0\ g$$ of benzene. The vapour pressure of solution is $$600\ mm\ Hg$$. What is the molar mass of the solute?
  • $$72.1\ g\ mol^{-1}$$.
  • $$70.6\ g\ mol^{-1}$$.
  • $$69.4\ g\ mol^{-1}$$.
  • $$56.2\ g\ mol^{-1}$$.
The coefficient of thermal expansion, $$\alpha$$, is nearly constant for a liquid $$\alpha =\cfrac { 1 }{ V } { \left( \cfrac { dV }{ dT }  \right)  }_{ P }$$
At $$293K$$ and $$1atm$$ for water $$\alpha =2.1{ K }^{ -1 }$$
What is the approximate work done when 1 mole of liquid is heated from $$288K$$ to $$298K$$ at $$1atm$$ (Molar volume of liquid$$=18ml$$)?
  • $$-78.25kJ$$
  • $$78.15J$$
  • $$-37.8J$$
  • $$-83.14J$$
If $${ PCl }_{ 5 }$$ is 80% dissociated at $$250$$ then its vapour density at room temperature will be:
  • 56.5
  • 104.25
  • 101.2
  • 52.7
The quantity $$\dfrac { PV }{ { k }_{ B }T }$$ represents the:

 $$({ k }_{ B } $$: Boltzmann constant)
  • number of particle of the gas
  • mass of the gas
  • number of the moles of the gas
  • translation energy of the gas
Two containers, X and Y at 300K and 350K with water vapour pressures 22 mm and 40 mm respectively a are connected, initially closed with a valve. If the valves opened.
  • The final pressure in each container is 31 mm
  • The final pressure in each container is 40 mm
  • Mass of $$H_{2}O$$(l) in X increases
  • Mass of $$H_{2}O$$(l) in Y decreases roar.
The vapour pressure of $$C_6H_6$$ and $$C_7H_8$$ mixture at $$50^{\circ}C$$ is given by $$p=179X_B+92$$ where $$X_B$$ is the mole fraction of $$C_6H_6$$.
Calculate (in mm) Vapour pressure of liquid mixture obtained by mixing $$936 \, g\ C_6H_6 \, $$ and $$736\ g$$ toluene is:
  • 300 mm Hg
  • 250 mm Hg
  • 199.4 mm Hg
  • 180.6 mm Hg
Pressure of the gas in column (1) is :
876957_072edef6ea864bf2a035fdce2f1d33b7.JPG
  • 60 cm of Hg
  • 55 cm of Hg
  • 50 cm of Hg
  • 45 cm of Hg
A solution containing 30 g of non-volatile solute exactly in 90 g of water has a vapour  pressure of 2.8 kPa at 298 K. Further 18 g  of water is then added to the solution and the new vapour pressure becomes 2.9 kPa at 298 k Calculate vapour pressure of water at 298K?
  • $$4.53kPa$$
  • $$3.53kPa$$
  • $$5.53kPa$$
  • $$6.53kPa$$
The vapour pressure of two pure liquids A and B which form an ideal solution are 1000 and 1600 torr respectively at 400 K. A liquid solution of A and B for which the mole fraction of A is 0.60 is contained in a cylinder by a piston on which the pressure can be varied. The solution use slowly vapourised at 400 K by decreasing the applied pressure. What is the composition of last droplet of liquid remaining in equilibrium with vapour?
  • $$X_A= 0.30, X_B= 0.70$$
  • $$X_A= 0.40, X_B= 0.60$$
  • $$X_A= 0.70, X_B= 0.30$$
  • $$X_A= 0.50, X_B= 0.50$$
$$P_A \, = \, X_AP_A$$ and $$P_B \, = \, X_BP_B$$
$$P_T \, = \, X_AP_A \, + \, X_BP_B$$
Vapour pressure of mixtures of Benzene $$(C_6H_6)$$ and toluene $$(C_7H_8)$$ at $$50^{\circ}C$$ are given by $$P_M \, = \, 179X_B \, + \, 92$$ where $$X_B$$ is mole fraction of $$C_6H_6$$.
What is the vapour pressure of pure liquids?
  • $$P_B \, = \, 92 mm, \, P_T \, = \, 179 mm$$
  • $$P_B \, = \, 271 mm, \, P_T \, = \, 92 mm$$
  • $$P_B \, = \, 180 mm, \, P_T \, = \, 91 mm$$
  • None of these
A sample of pure $$NO_{2}$$ gas healed lo 1000 K decomposes.

$$NO_{2}(g) \leftrightharpoons 2NO(g) + O_{2}(g)$$

The equillibrium constant $$K_{P}$$ is 100atm. Analysis shows that the partial pressure of $$O_{2}$$ is 0.25 atm at equillibrium. The partial pressure of $$NO_{2}$$ at equillibrium is:
  • 0.03
  • 0.25
  • 0.0245
  • 0.04
The vapour pressure of two pure liquids $$A$$ and $$B$$, that form an ideal solution are $$100$$ and $$900$$ torr respectively at temperature $$T$$. This liquid solution of $$A$$ and $$B$$ is composed of $$1\ mole$$ of $$A$$ and $$1\ mole$$ of $$B$$. What will be the pressure, when $$1$$ mole of mixture has been vapourized?
  • $$800\ torr$$
  • $$500\ torr$$
  • $$300\ torr$$
  • None of these
A nitrogen-hydrogen mixture initially in the molar ratio 1:3 reached equilibrium to form ammonia when 25% of the $$H_{2}$$ and $$N_{2}$$ had reacted. If the total pressure of the system was 21 atm, the partial pressure of ammonia at the equilibrium was: 
  • 4.5 atm
  • 3.0 atm
  • 2.0 atm
  • 1.5 atm
Which of the following is a correct graph?
The vapour pressure of two pure liquids A and B, that form an ideal solution are $$100$$ and $$900$$ torr respectively at temperature T. This liquid solution of A and B is composed of $$1$$ mole of A and $$1$$ mole of B. What will be the pressure, when $$1$$ mole of mixture has been vapourized?
  • $$800$$torr
  • $$500$$torr
  • $$300$$torr
  • None of these
Two moles of pure liquid 'A' $$(P_{A}^{0} =80mm$$ of Hg) and $$3$$ moles of pure liquid 'B' ($$P_{B}^{0} = 120mm$$ of Hg) are mixed. Assuming ideal behaviour?
  • Vapour pressure of the mixture is $$104$$mm of Hg
  • Mole fraction of liquid 'A' in Vapour pressure is $$0.3077$$
  • Mole fraction of 'B' in Vapour pressure is $$0.692$$
  • Mole fraction of 'B' in Vapour pressure is $$0.785$$
Two glass bulbs $$A$$ (of $$100\ mL$$ capacity), and $$B$$ (of $$150\ mL$$ capacity) containing same gas are connected by a small tube of negligible volume. At particular temperature, the pressure in $$A$$ was found to be $$20$$ times more than that in bulb $$B$$. The stopcock is opened without changing the temperature. The pressure in $$A$$ will :
  • Drop by $$75$$%
  • Drop $$57$$%
  • Drop by $$25$$%
  • Will remain same
Vapour pressure of $$CCl_4$$ at $$25^0$$C is $$143$$mm Hg. $$0.5$$ gm of a non-volatile solute (mol.wt.$$65$$) is dissolved in $$100$$ ml of $$CCl_4$$. Find the vapour pressure of the solution. (Density of CCl_4 = $$1.58 gm/cm^3$$)
  • $$141.93$$mm
  • $$94.39$$mm
  • $$199.34$$mm
  • $$143.99$$mm
Two liquids $$X$$ and $$Y$$ are perfectly immiscible. If $$X$$ and $$Y$$ have molecular masses in ration $$1 : 2$$, the total vapour pressure of a mixture of $$X$$ and $$Y$$ prepared in weight ratio $$2 : 3$$ should be:$$(P_{X}^{0} = 400\ torr, P_{Y}^{0} = 200\ torr)$$.
  • $$314\ torr$$
  • $$466.7\ torr$$
  • $$600\ torr$$
  • $$700\ torr$$
A rigid and insulated tank of 3 $$m^3$$ volume is divided into two components. One compartment of volume of 2 $$m^3$$ contains an ideal gas at 0.8314 MPa and 400 K and while the second compartment of volume 1 $$m^3$$ contains the same gas 8.314 MPa and 500 k. If the partition between the two compartments is ruptured, the final temperature of the gas is:
  • 420 K
  • 450 K
  • 480 K
  • None of these
$$100$$ grams of oxygen $$(O_{2})$$ gas and $$100$$ grams of helium $$(He)$$ gas are in separate containers of equal volume at $$100^{\circ}C$$. Which one of the following statement is correct?
  • Both gases would have the same pressure
  • The average kinetic energy of $$O_{2}$$ molecules is greater than that of $$He$$ molecules
  • The pressure of $$He$$ gas would be greater than that of the $$O_{2}$$ gas
  • The average kinetic energy of $$He$$ and $$O_{2}$$ molecules is same
A reaction at 300 K with $$\Delta G^o$$ = -1743 J/mol consists of 3 mole of $$A(g)$$, 6 mole of $$B(g)$$ and 3 mole of $$C(g)$$. If given $$A,\ B$$ and $$C$$ are in equilibrium in 1 litre container then the reaction may be:
[Given : 2 = $$e^{0.7}$$, R = 8.3 J/K - mol]
  • $$A\,+\,B \rightleftharpoons C$$
  • $$A \rightleftharpoons B\,+\,2C$$
  • $$2A \rightleftharpoons B\,+\,C$$
  • $$2C \rightleftharpoons A\,+\,B$$
Two liquids X and Y are perfectly immiscible. If X and Y have molecular masses in ratio 1 : 2, the total vapour pressure of a mixture of X and Y prepared in weight ratio 2 : 3 should be ($$Px^0 = 400 torr, Py^0 = 200 torr$$)
  • 314 torr
  • 466.7 torr
  • 600 torr
  • 700 torr
A mixture (by weight) of hydrogen and helium is enclosed in a two-litre flask at $$27^o C$$. Assuming ideal kept behaviour, the partial pressure of helium is found to be 0.2atm. Then the concentration of hydrogen would be:
  • 0.045
  • 8.26
  • 0.0162
  • 1.62
If $$0.2\ mol$$ of $$H_{2}(g)$$ and $$2\ mol$$ of $$S(s)$$ are mixed in a $$1\ dm^{3}$$ vessel at $$90^{\circ}C$$, the partial pressure of $$H_{2}S(g)$$ formed according to the reaction, $$H_{2}(g) + S(s)\rightleftharpoons H_{2}S, K_{P} = 6.8\times 10^{-2}$$ would be:
  • $$0.19\ atm$$
  • $$0.38\ atm$$
  • $$0.6\ atm$$
  • $$0.072\ atm$$
CuSO$$_4.$$5$$H_2O$$(s) $$\rightleftharpoons$$ CuSO$$_4$$.3H$$_2O$$(s) + 2H$$_2O$$(g); $$k_p$$ = 4 $$10^{4}$$ atm$$^2.$$ If the vapour pressure of water is 38 torr then percentage of relative humidity is : (Assume all data at constant temperature)
  • 4
  • 10
  • 40
  • None of these
Vapour Pressure of a mixture of benzene and toluene is given by $$P= 179X_{B} + 92$$, Where $$X_{B}$$ is mole fraction of benzene.
This condensed liquid again brought to the same temperature then what will be the mole fraction of benzene in vapour phase :
  • 0.007
  • 0.93
  • 0.65
  • 4.5
The pressure of a mixture of equal weights of two gases $$X$$ and $$Y$$ with molecular weight $$4$$ and $$40$$ respectively is $$1.1\ atm$$. The partial pressure of the gas $$X$$ in the mixture is :
  • $$1\ atm$$
  • $$0.1\ atm$$
  • $$0.15\ atm$$
  • $$0.5\ atm$$
A container of $$1\ L$$ capacity contains a mixture of $$4\ g$$ of $$O_{2}$$ and $$2\ g$$ of $$H_{2}$$ at $$0^{\circ}C$$. What will be the total pressure of the mixture?
  • $$50.42\ atm$$
  • $$25.21\ atm$$
  • $$15.2\ atm$$
  • $$12.5\ atm$$
An open flask contains air at $$27^{\circ}C$$. At what temperature should it be heated so that $$1/3rd$$ of air present in it goes out?
  • $$177^{\circ}C$$
  • $$100^{\circ}C$$
  • $$300^{\circ}C$$
  • $$150^{\circ}C$$
The certain volume of a gas exerts on its walls some pressure at a particular temperature. It has been found that by reducing the volume of the gas to half of its original value the pressure becomes twice that of the initial value at a constant temperature. This happens because:
  • mass of the gas increases with pressure
  • speed of the gas molecules decreases
  • more number of gas molecules strikes the surface per second
  • gas molecules attract each other
Value of gas constant $$R$$ in the ideal gas equation $$PV = nRT$$ depends upon:
  • temperature of the gas
  • pressure of the gas
  • units in the $$P, V$$ and $$T$$ are measured
  • nature of the gas

What is a weight of $$CO_2$$ in a $$10L$$ cylinder at $$5atm$$ and $$27^0C$$?
  • $$200\ g$$
  • $$224\ g$$
  • $$44\ g$$
  • $$89.3\ g$$
The main reason for deviation of gases from ideal behaviour is few assumptions of kinetic theory. These are
(i) there is no force of attraction between the molecules of a gas
(ii) volume of the molecules of a gas is negligibly small in comparison to the volume of the gas
(iii) Particles of a gas are always in constant random motion.
  • (i) and (ii)
  • (ii) and (iii)
  • (i), (ii) and (iii)
  • (iii) only
$$X,Y$$ and $$Z$$ in the given graph are?
932582_ab446ecc9fe946d2b73c4b1c74d32a2a.JPG
  • $$X={p}_{1}+{p}_{2},Y=1,Z=0$$
  • $$X={p}_{1}+{p}_{2},Y=0,Z=0$$
  • $$X={p}_{1}\times {p}_{2},Y=0,Z=0$$
  • $$X={p}_{1}-{p}_{2},Y=1,Z=0$$
If $$P_o$$ and $$P_s$$ are the vapour pressure of solvent and its solution respectively. $$x_1$$ and $$x_2$$ are the mole fraction of solvent and solute respectively then:
  • $$P_s = \dfrac{P_o}{x_2}$$
  • $$P_o - P_s = P_ox_2$$
  • $$P_s = P_ox_2$$
  • $$\dfrac{(P_o-P_s)}{P_s} = \dfrac{x_1}{(x_1+x_2)}$$
A plot of volume $$(V)$$ versus temperature $$(T)$$ for a gas at constant pressure is a straight line passing through the origin. The plots at different values of pressure are shown in figure. Which of the following order of pressure is correct for this gas?
936353_aef0d91813a54752b85d7fa8f24e9436.png
  • $$P_1>P_2>P_3>P_4$$
  • $$P_1=P_2=P_3=P_4$$
  • $$P_1 < P_2 < P_3 < P_4$$
  • $$P_1 < P_2 = P_3 < P_4$$
In three beakers labeled as (A), (B) and (C), $$100mL$$ of water, $$100mL$$ of $$1M$$ solution of glucose in water and $$100mL$$ of $$0.5M$$ solution of glucose in water are taken respectively and kept at same temperature.
Which of the following statements is correct?
  • Vapour pressure in all the three beakers is same
  • Vapour pressure of beaker B is highest
  • Vapour pressure of beaker C is highest
  • Vapour pressure of beaker B is lower than that of C and vapour pressure of beaker C is lower than that of A
5 litre of $$N_2$$ under a pressure of 2 atm, 2 litre of $$O_2$$ at 5.5 atm and 3 litre of $$CO_2$$ at 5 atm are mixed. The resultant volume of the mixture is 15 litre. Calculate the total pressure of the mixture and partial pressure of each constituent.
  • 2.06 atm
  • 1.75 atm
  • 3.06 atm
  • 4.50 atm
What is the total pressure exerted by the mixture of 7.0 g of $$N_2$$, 2g of hydrogen and 8.0 g of sulphur dioxide gases in a vessel of 6.1L capacity that has been kept in a reservoir at $$27^oC$$?
  • 2,5 bar
  • 4.5 bar
  • 10 atm
  • 5.7 bar
In a gaseous mixture at $$20^o C$$ the partial pressure of the components are:
$${ H }_{ 2 }$$ : 150 Torr      $${ CH }_{ 4 }$$ : 300 Torr     $${ CO }_{ 2 }$$ : 200 Torr        $${ C }_{ 2 }{ H }_{ 4 }$$ : 100 Torr
The volume % of $${ H }_{ 2 }$$ in mixture:
  • 26.67
  • 73.33
  • 80.00
  • 20
Calculate the change in pressure when $$1.04$$ mole of $$NO$$ and $$20 \,g \,O_2$$ in $$20$$ litre vessel originally at $$27^o C$$ react to produce the maximum quantity of $$NO_2$$ possible according to the equation. $$2NO(g) + O_2(g) \longrightarrow 2NO_2(g)$$
  • 0.2113 atm
  • 1.2321 atm
  • 0.6396 atm
  • 0.5687 atm
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