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

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 $$Hg$$
$$CuSO_4$$$$\cdot$$$$5H_2O(s)$$$$\rightleftharpoons$$ $$CuSO_4\cdot$$ 3$$H_2O(s)$$ + $$2H_2O(g)$$; $$K_p$$ = 4$$\times10^{-4}$$ $$atm^2$$ if the vapour pressure of water is 38 torr then percentage of relative humidity is: ( Assume all data at constant temperature)
  • $$4$$
  • $$10$$
  • $$40$$
  • $$none\ of\ these$$
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 $$Cl_{2}$$
A gas obeys the equation of state $$P(V-b)=RT$$ (The parameter $$b$$ is a constant). The slope for an isochore will be:
  • negative
  • zero
  • $$R/(V-b)$$
  • $$R/P$$
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.
In a closed vessel, an ideal gas at $$1\ atm$$ is heated from $$27^{\circ}C$$ to $$327^{\circ}C$$. The final pressure of the gas will approximately be :
  • $$3\ atm$$
  • $$0.5\ atm$$
  • $$2\ atm$$
  • $$12\ atm$$
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?
  • $$72.1\ g\ mol^{-1}$$.
  • $$70.6\ g\ mol^{-1}$$.
  • $$69.4\ g\ mol^{-1}$$.
  • $$56.2\ g\ mol^{-1}$$.
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 $$C_6H_6$$ 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
$$P_A \, = \, X_AP_A$$ 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
Vapour pressure of $$CC{l}_{4}$$ at $$25^{O}C$$ is 143mm Hg. 0.5gm of a non-volatile solute (mol. wt. 65) is dissolved in 100ml of $$CC{l}_{4}$$. Find the vapour pressure of the solution.
(Density of $$CC{l}_{4} = 1.58 gm/{cm}^{3}$$)
  • 141.93 mm
  • 94.39 mm
  • 199.34 mm
  • 143.99 mm
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 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 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.
  • Mass of $$H_{2}O$$(l) in X increases
  • 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 Y decreases roar.
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
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?
  • $$X_A= 0.30, X_B= 0.70$$
  • $$X_A= 0.40, X_B= 0.60$$
  • $$X_A= 0.70, X_B= 0.30$$
  • $$X_A= 0.50, X_B= 0.50$$
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
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:$$(P_{X}^{0} = 400\ torr, P_{Y}^{0} = 200\ torr)$$.
  • $$314\ torr$$
  • $$466.7\ torr$$
  • $$600\ torr$$
  • $$700\ torr$$
Which of the following relationships between partial pressure, volume and temperature is correct?
(i) $$P = \dfrac {nRT}{V}$$
(ii) $$P_{total} = p_{1} + p_{2} + p_{3}$$
(iii) $$P_{total} = (n_{1} + n_{2} + n_{3}) \dfrac {RT}{V}$$.
  • (i) and (ii)
  • (i) and (iii)
  • (ii) and (iii)
  • (i), (ii) and (iii)
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
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 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:
  • $$0.19\ atm$$
  • $$0.38\ atm$$
  • $$0.6\ atm$$
  • $$0.072\ atm$$
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 $$0.785$$
The virial equation for 1 mole of a real gas is written as:
PV=RT

[1+$$\frac{A}{V}+\frac{B}{V^2}+\frac{C}{V^3}+$$................to the higher power of n]

Where A, B and C are known as virial coefficients. If Vander Waal's equation is written in virial form, then what will be the value of B?
  • $$a-\cfrac{b}{RT}$$
  • $$b^3$$
  • $$b-\cfrac{a}{RT} $$
  • $$b^2$$
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
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
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?
  • $$50.42\ atm$$
  • $$25.21\ atm$$
  • $$15.2\ atm$$
  • $$12.5\ atm$$
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
A $$2\ L$$ vessel is filled with air at $$50^{\circ}C$$ and a pressure of $$3\ atm$$. The temperature is now raised to $$200^{\circ}C$$. A valve is now opened so that the pressure inside drops to one atm. What will be the fraction of the total number of moles, inside escaped on opening the valve? (Assume no change in the volume of the container).
  • $$7.7$$
  • $$9.9$$
  • $$8.9$$
  • $$0.77$$
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
What is the effect on the pressure of a gas if its temperature is increased at constant volume?
  • The pressure of the gas increases
  • The pressure of the gas decreases
  • The pressure of the gas remains same
  • The pressure of the gas becomes double
$$100$$ 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
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
  • $$P_1>P_2>P_3>P_4$$
  • $$P_1=P_2=P_3=P_4$$
  • $$P_1 < P_2 < P_3 < P_4$$
  • $$P_1 < P_2 = P_3 < P_4$$
A mixture in which the mole ratio of $$H_{2}$$ and $$O_{2}$$ is $$2 : 1$$ is used to prepare water by the reaction,
$$2H_{2(g)} + O_{2(g)} \rightarrow 2H_{2}O_{(g)}$$
The total pressure in the container is $$0.8\ atm$$ at $$20^{\circ}C$$ before the reaction. The final pressure at $$120^{\circ}C$$ after reaction is: (assuming $$80$$% yield of water).
  • $$1.787\ atm$$
  • $$0.878\ atm$$
  • $$0.787\ atm$$
  • $$1.878\ atm$$
On heating a liquid having coefficient of volume expansion $$\gamma$$ in a container having coefficient of linear expansion $$\alpha = \gamma/2$$ (numerically), the level of the liquid in the container would
  • Rise
  • Fall
  • Remains almost stationary
  • Cannot be predicted
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
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
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
When a non volatile solute is added to a pure solvent, the :
  • vapour pressure of the solution becomes lower then that of the pure solvent
  • rate of evaporation of the pure solvent is reduced
  • solute does not effect the rate of condensation
  • rate of the evaporation of the solution is equal to the rate of condensation of the solution at a lower vapour pressure than that in the case of the pure solvent
An inflated balloon has a volume of $$6.0L$$ at sea level ($$P=1atm$$) and is allowed to ascend in altitude until the pressure is $$0.4atm$$. During the rise, the temperature of the gas falls from $${27}^{o}C$$ to $$-{23}^{o}C$$. The volume of balloon at its final altitude is
  • $$12.5L$$
  • $$15L$$
  • $$10L$$
  • $$3L$$
When intermolecular attractive forces are neglected, isobar formed between V and T at constant p is of the type given in the figure.
Pressure at which isobar made is:
1035444_b9ef186e61fa440b89d6055a92aa566d.png
  • 2 atm
  • 0.5 atm
  • 1 atm
  • 4 atm
A glass bulb of volume 400$${ cm }^{ 3 }$$ is connected to another bulb of volume 200$${ cm }^{ 3 }$$ by means of a tube of negligible volume. The bulbs contain dry air and are both at a common temperature and pressure of $${ 20 }^{ 0 }$$C and 1.00 atm. The larger bulb is immersed in steam at $${ 100 }^{ 0 }$$C; the smaller, in melting ice at $${ 0 }^{ 0 }$$. Find the final common pressure.
  • 2.05 atm
  • 1.563 atm
  • 2.36 atm
  • 1.134 atm
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
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