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CBSE Questions for Class 11 Medical Chemistry Some Basic Concepts Of Chemistry Quiz 13 - MCQExams.com

A sample of a gas at STP contains 3.01×1023 molecules and has a mass of 22.0 grams.
This gas is most likely :
  • CO2
  • O2
  • N2
  • CO
  • NO
0.16 g of an organic compound containing sulphur produces 0.233 g of BaSO4. Percentage of sulphur in the compound is :
  • 20
  • 80
  • 50
  • 10
Maximum percentage of chlorine is in :
  • Chloral
  • Pyrene
  • Ethylidene chloride
  • PVC
Statement I : At STP, 22.4 liters of He will have the same volume as one mole of H2 (assume ideal gases).
Statement II : One mole or 22.4 liters of any gas at STP will have the same mass.
  • true, false
  • false, true
  • true, true, correct explanation
  • true, true, not correct explanation
The system that contains the maximum number of atoms is :
  • 4.25 g of NH3
  • 8 g of O2
  • 2 g of H2
  • 4 g of He
What is the percentage of calcium in calcium carbonate (CaCO3)
  • 30%
  • 40%
  • 50%
  • 60%
What mass of AgI will dissolve in 1.0L of 1.0M NH3? neglect change in conc. of NH3
(Given : Ksp=1.5×1016;Kf[Ag(NH3)+2]; (At.mass Ag=108,I=127)
  • 4.9×105g
  • 0.0056g
  • 0.035g
  • 0.011g
According to Avogadro's law the correct statement are
a) Volume of gas is directly proportional to the no. of moles at constant T and P.
b) The pressure of gas is directly proportional to temp. of the gas under all conditions.
c) Equal volumes of different gases under similar conditions consist of equal no. of molecules.
d) Equal volumes of different gas under same conditions have equal no. of atoms.
  • b,c
  • a,c
  • d,b
  • c,d
Natural abundances of 12C and 13C isotopes of carbon are 99% and 1%, respectively. Assuming they only contribute to the mol. wt. of C2F4, the percentage of C2F4 having a molecular mass of 101 is:
  • 1.00
  • 98
  • 0.198
  • 99
1 g of silver gets distributed between 10 cm3 of molten zinc and 100 cm3 of molten lead at 800oC. The percentage of silver in the zinc layer in approximately:
  • 89%
  • 91%
  • 97%
  • 94%
How do you determine the mass percent of a solute in a solution?
  • Mass percent = mass of solute mass of solution ×100 %
  • Mass percent = mass of solution mass of solute ×100 %
  • Mass percent = moles of solute mass of solution ×100 %
  • Mass percent = mass of solute moles of solution ×100 %
  • Mass percent = moles of solute moles of solution ×100 %
What is the percentage of sulphur in sulphuric acid (H2SO4)?
  • 32%
  • 32.45%
  • 32.65%
  • 32.55%
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): 
  • 1.235NA
  • (135NA)2
  • 1.2(35)2NA
  • 1.2NA
Avogadro's law shows the relationship between which two variables?
  • Volume and number of moles
  • Pressure and number of moles
  • Volume and pressure
  • Temperature and pressure
  • Temperature and number of moles
Percentage purity of a sample of gold is 85%. How many atoms of gold are present in its 1 gram sample? (Atomic mass of gold =197u).
  • 3.0×1021
  • 2.6×1023
  • 2.6×1021
  • 4.5×1026
Calculate the mole percentage of CH3OH and H2O respectively in 60% (by mass) aqueous solution of CH3OH.
  • 45.8,54.2
  • 54.2,45.8
  • 50,50
  • 60,40
The vapour pressure of a solution of a non -volatile electrolyte (A) in a solvent (B) is 95% of the vapour pressure of the solvent at the same temperature. If Mb=0.3MA, where MBand MA are molecular weights of B and A respectively, the weight ratio of the solvent and solute are:
  • 0.15
  • 5.7
  • 0.2
  • 4.0
Two vessels of volumes 16.4 L and 5 L contains two ideal gases of molecular existence at the respective temperature of 27C and 227C and exert 1.5 and 4.1 atm, respectively. The ratio of the number of molecules of the former to that of the later is:
  • 2
  • 1
  • 12
  • 13
  • 3
The mass of one twelfith of the mass of one carbon 12 atoms is 
  • 1.68×1024g
  • 1.008 g
  • -12 g
  • 3.66×1024g
How many hydroxide ions are present in 2.5 mol of Ca(OH)2 ?
(NA=6×1023)
  • 3×1023
  • 6×1023
  • 1.5×1024
  • 3×1024
A 1.85 g sample of an arsenic-containing pesticide was chemically converted to AsO34 (atomic mass of As = 74.9) and titrated with Pb2+ to form Pb3(AsO4)2. If 20 mL of 0.1 M PB2+ is required to reach the equivalence point, the mass percentages of arsenic in the pesticide sample is closest to
  • 8.1
  • 2.3
  • 5.4
  • 3.6
20 ml of H2O2 after acidification with dil H2SO4 required 30 ml of N/2 KMnO4 for complete oxidation .Calculate the % of H2O2 in g/lit.
  • 10.75 g/lit
  • 11.75 g/lit
  • 12.75 g/lit
  • 13.75 g/lit
If  the molar concentration of Pbl2 is then the 1.5×103molL1 concentration of iodide ions in g ion L1 is:
  • 3.0×103
  • 6.0×103
  • 0.3×103
  • 0.6×103
Volume of O_{2} remained after the first combustion?
  • 4\ ml
  • 2\ ml
  • 0
  • 8\ ml
The percentage of Se in peroxidase anhydrous enzyme is 0.5% by weight (atomic weight = 78.4). Then minimum molecular weight of peroxidase anhydrous enzyme is:
  • 1.568\times 10^{4}
  • 1.568\times 10^{3}
  • 15.68
  • 3.136\times 10^{4}
The mass of a mixture containing HCl and H_2SO_4 is 0.1 g. On treatment with an excess of an AgNO_3 solution, reacted with this acid mixture gives 0.1435 g of AgCl. Mass % of the H_2SO_4 mixture is :
  • 30
  • 60
  • 59
  • None of these
During the preparation of H_{2}S_{2}O_{8} (per disulphuric acid) O_{2} gas also releases at anode as by product. When 9.72\ L of H_{2} releases at cathode and 2.35\ L\ O_{2} at anode at STP, the weight of H_{2}S_{2}O_{8} produced in gram is:
  • 87.12
  • 43.56
  • 83.42
  • 51.74
The amonia evolved from 2g of a compound in Kjeldahl's estimation of nitrogen neutralizes 10 mL of 2 M { H }_{ 2 }S{ O }_{ 4 } solution. The weight percentage of nitrogen in the compound is
  • 28
  • 14
  • 56
  • 7
The common isotopes of carbon are ^{ 12 }C and ^{ 13 }C. The average mass of carbon is 12.01115 amu. What is the abundance of ^{ 13 }C isotope ?.
  • 1.115\%
  • 98.885\%
  • 0.480\%
  • 99.52\%
A gas mixture contains 50\% helium and 50\% methane by volume. What is the percentage by mass of methane in the mixture?
  • 20\%
  • 30\%
  • 50\%
  • 80\%
If 224ml of triatomic gas has a mass of 1g at 273K and 1atm pressure, then the mass of one atom is-
  • 8.30\times {10}^{-23}gm
  • 2.08\times {10}^{-23}gm
  • 5.53\times {10}^{-23}gm
  • 6.24\times {10}^{-23}gm
A 5 mL (specific gravity 1.02) of chlorine water is treated with an excess of KI.The liberate iodine required 26 mL of 0.15 \,M-Na_2SO_4 solution.Calculate the percentage of Cl_2 (by weight) the chloride water.Chloride water is a solution of free chlorine in water
  • 0.388 \%
  • 0.301 \%
  • 0.307 \%
  • 3.02 \%
0.3\ g of an oxalate salt was dissolved in 100\ mL solution. The solution required 90\ mL of N/20\ KMnO_4 for complete oxidation.The % of oxalate ion in salt is: 
  • 33\%
  • 66\%
  • 70\%
  • 40\%
5 g of a sample of bleaching powder is treated with excess acetic acid and KI solution. The liberated I_2 required 50 ml of N/10 hypo solution. The % available chlorine in sample is
  • 3.55
  • 7.0
  • 35.5
  • 28.2
A 1.85\ g sample of an arsenic-containing pesticide was chemically converted to AsO_{4}^{3-} (atomic mass of As = 74.9) and titrated with Pb^{2+} to form Pb_{3}(AsO_{4})_{2}. If 20\ mL of 0.1\ M\ Pb^{2+} is required to reach the equivalence point, the mass percentage of arsenic in the pesticide sample is closest to:
  • 8.1
  • 2.3
  • 5.4
  • 3.6
Choose the correct answers from the alternatives given :
Age of fossil may be found out by determining the ratio of two isotopes of carbon. The isotopes are ____________________.
  • C-12 and C-13
  • C-13 and C-14
  • C-12 and C-14
  • C-12 and carbon black
Which one of the following is not required for the formation of photochemical smog?
  • Nitrogen oxide
  • Methane
  • Volatile organic compounds
  • Ozone
4.0 g of a mixture of NaCl and an unknown metal iodide MI_{2} was dissolved in a water to form its aqueous solution. To this aqueous solution, The aqueous solution AgNO_{3} was added gradually so that silver halides are precipitated. The precipitates were weighed at regular interval and the given curve for the mass of precipitate versus volume of AgNO_{3} added was obtained. With the knowledge of the fact that halides are precipitated successively i.e. when one halide is precipitating , the other halide remains in the solution, answer the following questions:
(Molar mass of Ag = 108,\ I = 127,\ Na = 23).
Points P and Q are: P(20, 4.8),\ Q(37, 7.25)
What is the approximate mass percentage of MI_{2}?
  • 25
  • 40
  • 60
  • 75
0.5g sample of a sulphite salt was dissolved in 20ml solution and 20ml of this solution required 10ml of 0.002M acidified permanganate solution. Hence, the \% by mass of sulphite in the sulphite salt is:
  • 2\%
  • 4\%
  • 6\%
  • 8\%
2g of brass containing Cu and Zn only reacts with 3M HNO_3 solution. Following are the reactions taking place.

Cu(s)+HNO_3(aq)\rightarrow Cu^{2+}(aq)+NO_2(g)+H_2O(l)

Zn(s)+H^+(aq)+{NO}^-_3(aq)\rightarrow NH^+_4(aq)+Zn^{2+}(aq)+H_2O(l)

The liberated NO_2(g) was found to be 1.04L at 25^oC and 1 atm [Cu =63.5, Zn=65.4].
How many grams of NH_4NO_3 will be obtained in the reaction?
  • 0.405g
  • 0.0428g
  • 0.2018g
  • 0.358g
When a mixture of NaBr and NaCl is repeatedly digested with sulphuric acid, all the halogens are expelled and Na_{2}SO_{4} is formed quantitatively. With a particular mixture, it was found that the weight of Na_{2}SO_{4} obtained was precisely the same as the weight of NaBr - NaCl mixture taken. Calculate the ratio of the weights of NaCl and NaBr in the mixture.
  • 1:1.454
  • 2:1.31
  • 1.454 : 1.
  • 1.31:2
Calculate the mass percent (w/w) of sulphuric acid in a solution prepared by dissolving 4 g of sulphur trioxide in a 100ml sulphuric acid solution containing 80 mass percent (w/w) of H_2SO_4 and having a density of 1.96\ g/ml(molecular weight of H_2SO_4=98) Take reaction SO_3+H_2O\rightarrow H_2SO_4.
  • 80.8\%
  • 84\%
  • 41.65\%
  • None of these
Mole fraction of ethyl alcohol in aqueous ethyl alcohol (C_2H_5OH) solution is 0.25. Hence percentage of ethyl alcohol by weight is:
  • 54\%
  • 25\%
  • 75\%
  • 46\%
32 g of a sample of FeSO_4.7H_2O were dissolved in dilute sulphuric acid and water and its volume was made up to 1 litre. 25 mL of this solution required 20 mL of 0.02 M KMnO_4 solution for complete oxidation. Calculate the mass % of FeSO_4.7H_2O in the sample.
  • 34.75
  • 69.5
  • 89.5
  • None of these
What is the mass percentage of carbon tetrachloride if 22g of benzene is dissolved in 122g of carbon tetrachloride?
  • 84.72%
  • 15.28%
  • 50%
  • 44%
What is the mass per cent of oxygen in ethanol?
  • 52.14\%
  • 13.13\%
  • 16\%
  • 34.73\%
0.2 g of an organic compound contains C,\ H,\ O on combustion, it yields 0.15 g of CO_2 and 0.12 g H_2O. The percentage of C,\ H and O respectively is:
  • C=15 %, H= 20 %, O=65 %
  • C=10 %, H=8.2 %, O=81.8%
  • C=12.2 %. H=8.8 %, O=79 %
  • C=20 %, H=6.66 %, O=73.34 %
Flask I contains a gaseous mixture of He(g), H_2(g), in the molar ratio of 1:\sqrt{2}. The gas mixture is allowed to effuse through a fine orifice in the flask l and is collected in flask ll. What is the average molar mass of gas mixture initially collected in flask ll?
  • 3.20
  • 2.33
  • 4.00
  • None of these
32g of a sample of { FeSO }_{ 4 }.{ 7H }_{ 2 }O where the dissolved in dilute Sulphuric acid and water and it's volume was made up to 1 litre, 25 mL of this solution required 20 mL of 0.02 M\ KMn{ O }_{ 4 } solution of complete oxidation. Calculate the weight % of FeS{ O }_{ 4 }.{ 7H }_{ 2 }O in the sample. 
  • 34.75
  • 69.5
  • 89.5
  • None of these
Natural water contains about 0.02\% D_2O (heavy water). When it is enriched to 20\% (by volume), calculate the fraction of weight due to neutrons in 1 mole of sample.
  • 0.355
  • 0.444
  • 0.455
  • 0.500
0:0:1


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