CBSE Questions for Class 11 Medical Chemistry Some Basic Concepts Of Chemistry Quiz 4 - MCQExams.com

Temporary hardness is due to bicarbonates of $$Mg^{2+}\, and\, Ca^{2+}$$, it is removed by addition of CaO as follows:
$$Ca(HCO_3)_2\,+\, CaO\, \rightarrow\, 2CaCO_3\,+\, H_2O$$
Mass of $$CaO$$ required to precipitate 2 g $$CaCO_3$$ is:
  • $$2 g$$
  • $$0.56 g$$
  • $$0.28 g$$
  • $$1.12 g$$
$$3.01\times 10^{23}$$ molecules of elemental Sulphur will react with 0.5 mole of oxygen gas completely to produce
  • $$6.02\times 10^{23}$$ molecules of $$SO_3$$
  • $$6.02\times 10^{23}$$ molecules of $$SO_2$$
  • $$3.01\times 10^{23}$$ molecules of $$SO_3$$
  • $$3.01\times 10^{23}$$ molecules of $$SO_2$$
The relative atomic mass of naturally occurring chlorine is not a whole number. What is the reason for this ?
  • Chlorine atoms can have different number of neutrons
  • Naturally occurring chlorine cannot be obtained pure
  • Chlorine is unstable
  • The mass of the electrons has been included
A compound was found to contain 5.37% nitrogen. What is the minimum molecular weight of compound ?
  • $$26.07$$
  • $$2.607$$
  • $$260.7$$
  • None of these
Three containers A, B and C of equal volume, contain $$N_2$$, $$NO_2$$ and $$CO_2$$ respectively, at the same temperature and pressure. The ascending order of their masses is:
  • A, C, B
  • C, A, B
  • B, C, A
  • C, B, A
Aluminium reduces manganese dioxide to manganese at high temperature. The amount of aluminium required to reduce one gram mole of manganese dioxide is
  • 1/2 gram mole
  • 1 gram mole
  • 3/4 gram mole
  • 4/3 gram mole
The volume of $$0.5 M$$ aqueous $$NaOH$$ solution required to neutralize $$10 ml$$ of $$2 M$$ aqueous $$HCl$$ solution is
  • $$20 \ ml$$
  • $$40 \ ml$$
  • $$80 \ ml$$
  • $$120 \ ml$$
Number of moles of 1 $$m^3$$ gas, at STP, are:
  • 44.6
  • 40.6
  • 42.6
  • 48.6
Which law stated that 'matter is neither created nor destroyed'?
  • Law of multiple proportion
  • Law of conservation of energy
  • Law of constant composition
  • Law of conservation of mass
A compound was found to contain 5.37% nitrogen. What is the minimum molecular weight of compound?
  • 26.07
  • 2.607
  • 260.7
  • None of these
A chemical equation is balanced in accordance with the law of
  • conservation of mass
  • multiple proportion
  • constant proportion
  • reciprocal proportion
Natural Boron is a mixture of $$_{\text{5}}{{\text{B}}^{{\text{10}}}}\;{\text{and}}{\;_{\text{5}}}{{\text{B}}^{{\text{11}}}}$$ with relative abundance of 20% and 80 %. Find atomic weight of boron.
  • 10
  • 11
  • 10.8
  • 11.2
The law of conservation of mass was given by :
  • Dalton
  • Proust
  • Lavoisier
  • Berzelius
A sample of $$CaCO_3$$ has Ca =40%, C = 12% and O = 48% by mass. If the law of constant proportion is true then the weight of Ca in 16g of $$CaCO_3$$ made from different processes will be -
  • 64 g
  • 0.64g
  • 6.4g
  • 4.6 g
Which atom contains exactly 15 neutrons?
  • $$P^{32}$$ (atomic number $$= 17$$)
  • $$S^{32}$$ (atomic number $$= 16$$)
  • $$O^{15}$$ (atomic number $$= 8$$)
  • $$N^{15}$$ (atomic number $$= 7$$)
A sugar solution contains $$15\%$$ sugar by weight. When the solution is heated, $$40\%$$ sugar is left in the solution. The amount of water which is disappeared is:
  • $$0.0625\;g$$
  • $$62.5\;g$$
  • $$0.625\;g$$
  • $$6.25\;g$$
A sample of $$CaCO_3$$ has $$Ca=40\%,\,C=12\%$$ and $$O=48\%$$. If the law of constant proportion is true then the weight of $$Ca$$ in $$16\;g$$ of $$CaCO_3$$ made from different processes will be
  • $$64\;g$$
  • $$0.64\;g$$
  • $$6.4\;g$$
  • $$4.6\;g$$
In a chemical reaction, when 14 g of sodium carbonate reacted with 10g of acetic acid (ethanoic acid), then it was observed that, 16.67 g of sodium acetate solution in water and 7.33 g of carbon dioxide were produced. Which law does this depicts?
  • Law of definite proportions
  • Law of conservation of mass
  • Law of constant proportions
  • Avogadro's law
Among the following quantities:
(i) mass number
(ii) average mass of a Carbon atom in amu
(iii) the charge of nucleus in amu and
(iv) mass of a Carbon -12 atom in grams
  • only (i) is whole number
  • only (i) and (iii) are whole number
  • only (i) and (iv) are whole numbers
  • only (iii) and (iv) are whole numbers
How much MgO is obtained on heating 5 gm of $$\displaystyle \left ( MgCO_{3} \right )$$ Magnesium carbonate?
  • 2.4 gm
  • 2.38 gm
  • 2.8 gm
  • 3.28 gm
The National Physical Laboratory is situated at:
  • Kolkata
  • New Delhi
  • Bombay
  • None of these
The number of molecules in 1 L of oxygen and 1 L of nitrogen at STP will be:
  • equal
  • greater for $$N_2$$
  • greater for $$O_2$$
  • equal to Avogadro's number
When an inflated tyre bursts, the air escaping out will:
  • get heated up
  • be cooled
  • not undergo any change in its temperature
  • be liquified
Which pair has same percentage of carbon?
  • $$CH_3COOH \: and \: C_6H_{12}O_6$$
  • $$CH_3COOH \: and \: C_{12}H_{22}O_{11}$$
  • $$CH_3COOH \: and \: C_2H_5OH$$
  • $$C_6H_{12}O_6 \: and \: C_{12}H_{22}O_{11}$$
The law which suggests $$n_1 = n_2$$ for two solutions at same temperature and pressure is 
  • van't Haff - avogadro's law
  • van't Hoff Boyle's law
  • van't Hoff's law
  • Henry's law
$$5.6$$ litres of a monoatomic gas at S.T.P contain :
  • $$6.02\times {10}^{23}$$ atoms
  • $$\frac14\times 6.02\times {10}^{23}$$ atoms
  • $$\frac12\times 6.02\times {10}^{23}$$ atoms
  • $$\frac13\times 6.02\times {10}^{23}$$ molecules
The first organic substance ever prepared in the laboratory from the inorganic compound is:
  • urea
  • ethyl alcohol
  • methane
  • ethane
One atomic mass unit is equivalent to
  • $$1.67\times 10^{-27} g$$
  • $$1.66\times 10^{-27} kg$$
  • $$1.67\times 10^{-27} mg$$
  • $$1.6\times 10^{-24} g$$
In chulhas, gaps are left between the logs:
  • to decrease the ignition temperature of the fuel
  • to allow the air to enter and facilitate fuel burning
  • to cut off the supply of air
  • all of these
What is the percentage by weight of sulphuric acid if 13 g of H$$_2$$SO$$_4$$ is dissolved to make 78 g of solution?
  • 13.2%
  • 14.28%
  • 20%
  • 16.6%
Calculate the (w/W)% of 10 g of potassium hydroxide in 40 g of solvent.
  • 25%
  • 20%
  • 30%
  • 40%
What is the percentage by weight of sulphuric acid if 13 g of $$ H_2SO_4$$ is dissolved to make 78 g of solution?
  • 23.4
  • 20
  • 16.6
  • 13.2
The w/W % of 25 g of calcuim hydroxide in 50 g of solvent is_____ %
  • 40
  • 33.33
  • 36.3
  • 30
Mass can neither be created nor destroyed. This is in agreement with which law of chemical combination?
  • Law of definite proportion
  • Law of multiple proportion
  • Law of conservation of mass
  • Law of conservation of momentum
What is the mass of the solvent present in 200 g of 25% (w/W) calcium hydroxide solution?
  • 150 g
  • 125 g
  • 175 g
  • 100 g
1.008 grams of hydrogen combines with 35.453 g of chlorine to form 36.463 g of a pure compound (hydrogen chloride). Dalton's explanation for this experimental fact might be: 
  • One atom of hydrogen combines with 35.453 atoms of chlorine in this reaction
  • Hydrogen and chlorine atoms always combine in a 1:35 ratio.
  • Chlorine accepts hydrogen's electron to form polar covalent hydrogen chloride
  • Hydrogen and chlorine atoms aren't created or destroyed in the process so the reactant mass is the same as the product mass.
The formula for % composition of a compound is:
  • molar mass of a compound/mass due to specific component $$\times$$ 100
  • mass due to specific component $$\times$$ 100
  • mass due to specific component/molar mass of a compound $$\times$$ 100
  • molar mass of a specific component/temperature $$\times$$ 100
What is the atomic mass (u) of chlorine?
  • 34
  • 35.5
  • 33
  • 35
A solution contains 100 g of urea in 400 g of water. Calculate the concentration in terms of mass by mass percentage of the solution.
  • 20
  • 25
  • 10
  • 80
Which is not one of the laws of chemical combinations?
  • Law of multiple proportion
  • Law of conservation of mass
  • Law of conservation of energy
  • Law of definite proportion
Which of these would support the idea that mass is conserved in a reaction that produces gas as a product?
  • Heating the reactants to ensure the reaction occurs in a gaseous state.
  • Subtracting the mass of the gas from the mass of the solid and liquid products.
  • Mixing the reactants and measuring their total mass.
  • Trapping the gas and measuring its mass.
Mass number is denoted by:
  • D
  • S
  • A
  • Z
$$AgNO_3+NaCl\rightarrow AgCl+NaNO_3$$. In this reaction, mass of $$AgNO_3$$ and $$NaCl$$ is equal to the mass of $$AgCl$$ and $$NaNO_3$$. Then this chemical reaction satisfies:
  • Law of constant composition
  • Law of conservation of mass
  • Gay Lussac's law
  • Law of multiple proportion
During any chemical change, the total mass of the products is equal to the total mass of reactants. This is a statement according to:
  • Law of conservation of mass
  • Law of constant composition
  • Law of multiple proportion
  • Law of reciprocal proportion
In a chemical reaction, $$100 g$$ baking soda mixture containing sodium bicarbonate and vinegar on heating gives $$43 g$$ of carbon dioxide gas. What mass of solid residue is left in food?
  • $$54\ g$$
  • $$55\ g$$
  • $$56\ g$$
  • $$57\ g$$
Who laid the foundation of chemical sciences by experimentally establishing laws of chemical combination along with other scientists?
  • Proust
  • Antoine Lavoisier
  • Dalton
  • None of the above
A solution is prepared by dissolving 60 g of sodium chloride in 400 g of water. What is the mass-by-mass percent of sodium chloride in this solution?
  • 18%
  • 13%
  • 0.13%
  • 0.15%
Which scientist proposed the concept of atomic mass?
  • Avogadro
  • Gay Lussac
  • Proust
  • Dalton

Which law was given by Antoine L. Lavoisier?
  • Laws of multiple proportion
  • Law of conservation of mass
  • Both A and B
  • None of the above
If the % composition of a 'x' component is 35%, find the mass of the dried 'x' component in 100g? mixture + beaker = 50 g, mass of beaker = 23 g
  • 15.5 g
  • 9.45 g
  • 35.5 g
  • 13.4 g
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