CBSE Questions for Class 11 Engineering Chemistry States Of Matter Quiz 8 - MCQExams.com

The boiling point of $$ C_{6}H_{6},CH_{3}OH, C_{6}H_{5}NH_{2} $$ and $$C_{6}H_{5}NO_{2}   $$ are $$ 80^{\circ},\ 65 ^{\circ},\ 184^{\circ}$$ and $$212^{\circ} $$ respectively. Which will show highest vapourr pressure at room temperature?
  • $$ C_{6}H_{6}$$
  • $$ CH_{3}OH$$
  • $$ C_{6}H_{5}NH_{2} $$
  • $$C_{6}H_{5}NO_{2} $$
Kinetic energy of gas depends on:
  • temperature
  • pressure
  • surface area
  • both $$A$$ and $$B$$
At $$127^0C$$ and 1 atm pressure, a mixture of a gas contains 0.3 mole of $$N_2$$ and 0.2 mole of $$O_2$$. The volume of the mixture is?
  • 15 L
  • 18.2 L
  • 16.4 L
  • 22.4 L
Dry ice is solid carbon dioxide. A $$0.05\ g$$ sample of dry ice is placed in an evacuated $$4.6$$L  vessel at $$30^0$$C. Calculate the pressure inside the vessel after all the dry ice has been converted to $$CO_2$$ gas.
  • $$6.14$$ atm
  • $$0.614$$ atm
  • $$0.0614$$ atm
  • $$6.14 \times 10^{-3}$$ atm
A mixture of ethyl alcohol and propyl alcohol has vapour pressure of $$290mm$$ at $$300K$$. The vapour pressure of propyl alcohol is $$200mm$$. If mole fraction of ethyl alcohol is $$0.6$$ its vapour presssure at same temperature will be:-
  • $$360$$
  • $$350$$
  • $$300$$
  • $$700$$
The value of the molar gas constant is:
  • $$8.3145\times 10^3 \ J\ mol^{-1}K^{-1}$$
  • $$1.987 \ cal\ mol^{-1} K^{-1}$$
  • $$0.083145\times 10^3dm^3 bar\ mol^{-1}K^{-1}$$
  • $$0.983145\ dm^3\ bar\ mol^{-1}K^{-1}$$
The amount of solute (mol mass=$$60$$) that must be added to $$180g$$ of water so that the vapour pressure of water is lowered by $$10 \%$$ is?
  • $$30$$g
  • $$60$$g
  • $$120$$g
  • $$12$$g
The vapour pressure of a pure liquid A is 70 torr at 300 K. It forms an ideal solution with another liquid B. The mole fraction of B in the solution is 0.2 and total pressure of solution is 84 torr at 300 K. The vapour pressure of pure liquid B at 27C is ?
  • 0.14 torr
  • 560 torr
  • 140 torr
  • 70 torr
How much pressure will be felt by a gas ballon which at 100 m depth in a sea form sea level?
  • $$1081320$$ Pa
  • $$98$$ Pa
  • $$9.8 \times 10^5$$ Pa
  • $$1.58 \times 10^6$$ Pa
One mole of non volatile solute is dissolved in two moles of water. The vapour pressure of the solution relative to that of water is:
  • $$\dfrac{2}{3}$$
  • $$\dfrac{1}{3}$$
  • $$\dfrac{1}{2}$$
  • $$\dfrac{3}{1}$$
Which is not true in case of an ideal gas?
  • It cannot be converted into a liquid
  • There is no interaction between the molecules
  • All molecules of the gas move with same speed
  • At a given temperature, $$PV$$ is proportional to the amount of the gas
The no. of moles per liter in the equation $$PV=nRT$$ is expressed by:
  • $$\dfrac { P }{ RT } $$
  • $$\dfrac { PV }{ RT } $$
  • $$\dfrac { RT }{ PV } $$
  • none of these
Two liquids, A and B, form an ideal solution. At the specified temperature, the vapour pressure of pure A is 200 mm Hg while that of pure B is 75 mm Hg. If the vapour over the mixture consists of 50 mol percent A, what is the mole percent A in the liquid?
  • 20
  • 76
  • 27
  • 65
The relative decrease in vapour pressure of an aqua solution containing 2 moles of $$4NaCl$$ in 3 moles of $${H}2_{O}$$ is 0.On reaction with $$AgNO_3$$ this solution will form:
  • 1 mol of $$AgCl$$
  • 0.25 mol of $$AgCl$$
  • 2 mol of $$AgCl$$
  • 0.4 mol of $$AgCl$$
A gas volume 100 cc. is kept in a vessel at pressure $$10^4$$ atm maintained at temperature $$24^0C$$. If now the pressure is increased to $$10^5$$ atm, keeping the temperature constant, then the volume of the gas becomes:
  • 10 cc
  • 100 cc
  • 1 cc
  • 1000 cc
The vapour pressure of water is $$12.3k \, Pa$$ at $$300K$$. Calculate the vapour pressure $$1$$ molal solution of a non-volatile solute in it.
  • $$12.08 \ kPa$$
  • $$1.208 \ Ppa$$
  • $$2.4 \ kPa$$
  • $$0.4 kPa$$
A glass tube of volume 112ml containing a gas is partially evacuated till the pressure in it drops to $$3.8\times { 10 }^{ -5 }$$ torr at 0 degree C.The number of molecules of the gas remaining in the tube?
  • $$3\times { 10 }^{ 17 }$$
  • $$1.5\times { 10 }^{ 14 }$$
  • $$112.5\times { 10 }^{ 20}$$
  • Name of the gas is required
A container contains equal mass of $$C{ O }_{ 2 },{ O }_{ 2 },C{ H }_{ 4 },S{ O }_{ 2 }$$ gases at a particular temperature.Which gas will exert the maximum amount of partial pressure?
  • $$C{ O }_{ 2 }$$
  • $${ O }_{ 2 }$$
  • $$C{ H }_{ 4 }$$
  • $$S{ O }_{ 2 }$$
The kinetic energy for 14 grams of nitrogen gas at $$127^0C$$ is nearly (mol. mass of nitrogen = 28 and gas constant = 8.31 $$JK^{-1} mol^{-1}$$)
  • $$1230\ J$$
  • $$4015\ J$$
  • $$2493\ J$$
  • $$990\ J$$
If number of molecules of $$H_{2}$$ are double than that of $$O_{2}$$, then ratio of mean kinetic energy per molecule of hydrogen to that of oxygen at 300 K is:
  • 2:1
  • 1:2
  • 2:3
  • 1:4
Two liquids A and B have $${P}_{A}^{o}$$ and $${P}_{B}^{o}$$ in the ratio $$1:3$$ and the ratio of number of moles of $$A$$ and $$B$$ in liquid phase are $$1:3$$. Then mole fraction of A in vapour phase in equilibrium with the solution is equal to:
  • $$0.1$$
  • $$0.2$$
  • $$0.5$$
  • $$1.0$$
An amount of 1.00 g of a gaseous compound of borbon and hydrogen occupies 0.820 liter at 1.00 atm and at $$3^{0}C$$. The compound is (R=0.0820 liter atm $$mole^{-10}K^{-1};$$ at. wt:H=1.0,B=10.8)
  • $$BH_{3}$$
  • $$B_{4}H_{10}$$
  • $$B_{2}H_{6}$$
  • $$B_{3}H_{12}$$
The gas Z in the above fraction is ?
  • Nitrous oxide
  • Nitric Oxide
  • Dinitrogen tetroxide
  • Nitrogen dioxide
A gas occupies $$600ml$$ at $${27}^{o}C$$ and $$730mm$$ pressure. What would be its volume at STP?
  • $$0.5244$$ lit.
  • $$1.5244$$ lit.
  • $$2.5244$$ lit
  • $$3.5244$$ lit
Two flask $$A$$ and $$B$$ of equal volumes maintained temperature 300 K and 700 K contain equal mass of $$He(g)$$ and $$N_{2}(g)$$ respectively. What is the ratio of total translation kinetic energy of gas in flask $$A$$ to that of flask $$B$$?
  • $$1:3$$
  • $$3:1$$
  • $$3:49$$
  • None of these
Equal mass which of the following substance of occupy maximum volume at room temperature? 
  • Water
  • Sugar
  • Oxygen
  • Graphite
A container contains $$O_{2}$$ and $$N_{2}$$ in equal molar concentration at same temperature, what is the $$CORRECT$$ statement about the average molar kinetic energy of the two gasses?
  • Depends upon volume
  • $$KE_{N2}=KE_{O2}$$
  • $$KE_{N2}> KE_{O2}$$
  • $$KE_{N2}< KE_{O2}$$
Normal boiling point of a liquid is that temperature at which vapour of the liquid pressure of the liquid is equal to:
  • zero
  • 380mm of Hg
  • 760mm of Hg
  • 100mm of Hg
A container of volume $$40$$ liters consist of some gas at a pressure of 2 atm and temperature of $$300 K$$. It is heated to $$400 K$$ such that half of the gas escape and volume changes to 60 liters. The new pressure of the gas at the final condition will be:
  • $$2 atm$$
  • $$1 atm$$
  • $$\dfrac{8}{9}$$ atm
  • $$\dfrac{9}{8}$$ atm
Correct gas equation is :
  • $$\dfrac{V_1T_2}{P_!}=\dfrac{V_2T_1}{P_2}$$
  • $$\dfrac{P_1V_1}{P_2V_2}=\dfrac{T_1}{T_2}$$
  • $$\dfrac{P_1T_2}{V_1}=\dfrac{P_2V_2}{T_2}$$
  • $$\dfrac{V_1V_2}{T_1T_2}=P_1P_2$$
A relation between vapour pressure and the temperature is known as
  • Ideal gas equation
  • Boltzman equation
  • Clausious equation
  • Clausius-Clapeyron equation
Lowering in vapour pressure is highest for:
  • $$0.2m$$ urea
  • $$0.1m $$ glucose
  • $$0.1m \, MgSO_4$$
  • $$0.1m \, BaCl_2$$
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
The total kinetic energy (in joules) of the molecules in $$8 \ g$$ of methane at $$27^oC$$ is:
  • $$374100 \ J$$
  • $$935.3 \ J$$
  • $$1870.65 \ J$$
  • $$700 \ J$$
A mixture contains 16 g of oxygen ,28g of nitrogen and 8g of methane.Total pressure of the mixture is 740mm. What is the partial pressure of nitrogen in mm?
  • 185
  • 370
  • 555
  • 740
if the mass ratio of hydrogen gas is to oxygen gas in a mixture is 1:2 then the ratio of their number of molecules is:
  • 4:1
  • 1:2
  • 8:1
  • 1:4
Mass of a given gas occupies two litre at STP. By keeping the pressure constant, at what temperature the gas will occupy 4 litre?
  • $$ 546\ K $$
  • $$ 273\ K $$
  • $$ 100^oC $$
  • $$ 50^oC $$
When the pressure of 5L of $$N_2$$ is double and its temperature is raised from 300K to 600K, the final volume of the gas would be:
  • 10 L
  • 5 L
  • 15 L
  • 20 L
In an ideal solution of non-volatile solute B in solvent A in 2: 5 molar ratio has vapour pressure 250 mm. If another solution in ratio 3: 4 prepared then vapour pressure above this solution is:
  • 200 mm
  • 250 mm
  • 350 mm
  • 400 mm
The product formed in the reaction of $$SOCl_2$$ with white phosphorus is
  • $$PCl_3$$
  • $$SO_2Cl_2$$
  • $$SCl_2$$
  • $$POCl_3$$
A sample of 16g charcoal was brought into contact with $$  C{  H}_{  4}$$ gas contained in a vessel of 1 litre at $$ 2{ 7 }^{0  }C  $$ . The pressure of gas was found to fall from 760 to 608 torr. The density of charcoal sample is 1.6g/ $$ c{  m}^{ 3 }  $$. What is the volume of the $$  C{  H}_{  4}$$ gas adsorbed per gram of the adsorbent at 608 torr and $$ 2{ 7 }^{0  }C  $$ ?
  • 125 mL/g
  • 16.25 mL/g
  • 26 mL/g
  • None of these
The vapour pressure of a solution containing 5 g of a non electrolyte in 100 g of water at a particular temperature is $$2985 N{m}^{-2}$$. If the vapour pressure of pure water is $$3000 N{m}^{-2}$$, the molecular weight of solute is:
  • $$60$$
  • $$120$$
  • $$180$$
  • $$380$$
The temperature and pressure at which ice, liquid. water and water vapour can exist together are ?
  • $${ 0 }^{ o }C,\quad 1 atm $$
  • $${ 2 }^{ o }C,\quad 4.7atm$$
  • $${ 0 }^{ o }C,\quad 4.7mm$$
  • $${ -2 }^{ o }C,\quad 4.7mm$$
Kinetic theory of gases presumes the collision between the molecules to be perfectly elastic because:
  • the molecules are rigid
  • the temperature remains constant irrespective of collisions
  • collisions will not split the molecules
  • the molecules are tiny
In the gas equation $$PV = nRT$$ , the value of $$R$$ depends upon:
  • Nature of gas
  • The pressure of gas
  • Unit of measurement
  • Temperature of gas
According to the equipartition principle, each degree of freedom contribute following amount to the translational kinetic energy of molecule: (hence k = Boltzmann constant)
  • $$\dfrac{1}{2} kT$$
  • $$kT$$
  • $$\dfrac{3}{2} kT$$
  • $$\dfrac{1}{3} kT$$
The solubility of a specific non-volatile salt is  $$4\mathrm { g }$$  in $$100\mathrm { g }$$  of water at  $$25 ^ { \circ } \mathrm { C } .$$  If  $$2.0 g,$$  $$4.0\mathrm g$$  and  $$6.0 g$$  of the salt added of  $$100 g$$  of water at  $$25 ^ { \circ } \mathrm { C } ,$$  in system  $$X , Y$$  and  $$Z .$$  The vapour pressure would be in the order:
  • $$X < Y < Z$$
  • $$X > Y > Z$$
  • $$Z > X = Y$$
  • $$x > Y = z$$
If volume of $$2$$ moles of a gas at $$27^\circ C$$ is $$8.21 L$$ then pressure of this gas will be.
  • $$0.6$$ atm
  • $$6$$ atm
  • $$60$$ atm
  • $$600$$ atm
If  $$500ml$$  of a gas  $$A$$  at  $$1000$$ torr, and  $$1000ml$$  of gas  $$B$$  at  $$800$$  torr  are placed in  $$2L$$  container the final pressure will be -
  • $$100$$ torr
  • $$650$$ torr
  • $$1800$$ torr
  • $$2400$$ torr
The number of $$H_{3}O^{+}$$ ions present in 10ml of water at $$25^{\circ}C$$ is:
  • $$6.023 \times 10^{-14}$$
  • $$6.023 \times 10^{14}$$
  • $$6.023 \times 10^{-19}$$
  • $$6.023 \times 10^{19}$$
0:0:1


Answered Not Answered Not Visited Correct : 0 Incorrect : 0

Practice Class 11 Engineering Chemistry Quiz Questions and Answers