CBSE Questions for Class 11 Medical Chemistry Some Basic Concepts Of Chemistry Quiz 12 - MCQExams.com

When 100 ml of a $$O_{2} - O_{3}$$ mixture was passed through turpentine, there was the reduction of volume by 20 ml. If 100ml of such a mixture is heated, what will be the increase in volume?
  • $$10\ ml$$
  • $$20\ ml$$
  • $$30\ ml$$
  • $$25\ ml$$
The average atomic mass of a mixture containing 79 mole percent of  $$\displaystyle ^{24}\textrm{Mg}$$ and remaining 21 mole percent of $$\displaystyle ^{25}\textrm{Mg}$$ and $$\displaystyle ^{26}\textrm{Mg}$$, is 24.Mole percent of $$\displaystyle ^{26}\textrm{Mg}$$ is :
  • 5
  • 20
  • 10
  • 15
$$15\; g$$ of methyl alcohol is present in $$100$$ ml of solution. If density of solution is $$0.90$$ g/ml. Calculate the mass percentage of methyl alcohol in solution.
  • $$16.67\:\%$$
  • $$16.97\:\%$$
  • $$17.67\:\%$$
  • $$17.97\:\%$$
Calculate percentage change in $$M_{avg}$$ of the mixture, if $$PCl_{5} $$ undergo $$50\%$$ decomposition is a closed vessel.
  • $$50\%$$
  • $$66.66\%$$
  • $$33.65\%$$
  • $$Zero$$
$$300$$ g of an aqueous solution of a particular solute (containing $$30$$% solute by mass) is mixed with $$400$$ g of another aqueous solution of the same solute (containing $$40$$% solute by mass). In the final solution, mass $$\%$$ of solute is :
[Given, Molecular mass of solute $$\displaystyle = 50$$]
  • $$40.09\%$$
  • $$39.87\%$$
  • $$34.05\%$$
  • $$35.71\%$$
The mole fraction of solute in aqueous urea solution is $$0.2$$. The mass percent of solute is:
  • $$45.45\%$$
  • $$43.34\%$$
  • $$34.23\%$$
  • $$35.67\%$$
Which of the following statements is correct about the reaction given below?
$$\displaystyle 4Fe\left ( s \right )+3O_{2}\left ( g \right )\rightarrow 2Fe_{2}O_{3}\left ( g \right )$$
  • The total mass of reactants $$=$$ Total mass of the products. It follows the law of conservation of mass.
  • The total mass of reactants $$=$$ Total mass of the products. Therefore, the law of multiple proportions is followed.
  • Amount of $$Fe_{2}O_{3}$$ can be increased by taking any one of the reactants (iron or oxygen) in excess.
  • Amount of $$Fe_{2}O_{3}$$ produced will decrease if the amount of any one of the reactants (iron or oxygen) is taken in excess.
10 ml mixture of $$CO, CH_{4}$$ and $$N_{2}$$, exploded with an excess of oxygen, gave a contraction of 6.5 ml. There was a further contraction of 7ml when the residual gas was treated with $$KOH$$. Volume of $$CO, CH_{4}$$ and $$N_{2}$$ respectively, is :
  • 5ml, 2ml, 3ml
  • 2ml, 6ml, 4ml
  • 1ml, 8ml, 9ml
  • 4ml, 3ml, 5ml
60ml of a mixture of nitrous oxide and nitric oxide was exploded with excess of hydrogen. If 38ml of $$N_{2}$$ was formed, calculate the volume of each gas in the mixture.
  • $$\displaystyle \:NO= 44ml; N_{2}O= 16ml$$
  • $$\displaystyle \:NO= 45ml; N_{2}O= 20ml$$
  • $$\displaystyle \:NO= 34ml; N_{2}O= 22ml$$
  • $$\displaystyle \:NO= 20ml; N_{2}O= 26ml$$
How many moles of $$Na^{+}$$ ions are present in $$20$$ mL of $$0.40$$ M $$Na_3PO_4$$?
  • $$0.0080$$
  • $$0.024$$
  • $$0.050$$
  • $$0.20$$
Two gases A and B which react according to the equation $$\displaystyle \:aA_{(g)}+bB_{(g)}\rightarrow cC_{(g)}+dD_{(g)}$$ to give two gases C and D are taken (amount not known) in an Eudiometer tube (operating at a constant pressure and temperature) to cause the above. If on causing the reaction there is no volume change observed then which of the following statement are correct :
  • $$\displaystyle \:\left ( a+b \right)= \left ( c+d \right )$$
  • Average molecular mass may increase or decrease if either of A or B is present in limited amount.
  • Vapour Density of the mixture will remain same throughout the course of reaction.
  • Total moles of all the component of mixture will change.
10 ml of CO is mixed with 25 ml air having  20 per cent $$O_{2}$$ by volume. What would be the final volume if none of CO and $$\displaystyle\: O_{2}$$ is left after the reaction?
  • 30 ml
  • 40 ml
  • 43 ml
  • 49 ml
When a certain quantity of oxygen was ozonised in suitable apparatus, the volume decreased by $$4\ ml$$. On addition of turpentine the volume further decreased by $$8\ ml$$. All volumes were measured at the same temperature and pressure. From these data, establish the formula of ozone.
  • $$\displaystyle \:O_{3}$$
  • $$\displaystyle \:O_{4}$$
  • $$\displaystyle \:O_{5}$$
  • $$\displaystyle \:O_{6.5}$$
$$40\: g\: Ba(MnO_{4} )_{2}$$ (mol. wt. $$= 375$$ g/mol) sample containing some inert impurities in acidic medium is completely reacted with $$125$$ mL of $$33.6\: V$$ of $$H_{2}O_{2}$$. What is the percentage purity of the sample?
  • $$28.12 \%$$
  • $$70.31 \%$$
  • $$85 \%$$
  • None of the above
20 ml of a mixture of $$C_{2}H_{2}$$ and CO was exploded with 30ml of oxygen. The gases after the reaction had a volume of 34ml. On treatement with $$KOH$$, 8ml of oxygen remained. Calculate the composition of the mixture.
  • $$C_{2}H_{2}= 6 ml, CO= 14 ml$$
  • $$C_{2}H_{2}= 4 ml, CO= 28 ml$$
  • $$C_{2}H_{2}= 8 ml, CO= 30 ml$$
  • $$C_{2}H_{2}= 10 ml, CO= 19 ml$$
Calculate the volume of $$CO_{2}$$ evolved by the combustion of $$50$$ ml of a mixture containing $$40$$ per $$C_{2}H_{4}$$ and $$60$$ per $$CH_{4}$$ (by volume).
  • $$70$$ ml
  • $$75$$ ml
  • $$80$$ ml
  • $$82$$ ml
A mixture of $$NH_{4}NO_{3}$$ and $$(NH_{4})_{2}HPO_{4}$$ contains $$30.40 \%$$ mass percent of nitrogen. What is the mass ratio of the two components in the mixture?
  • $$2:1$$
  • $$1:2$$
  • $$3:4$$
  • $$4:1$$
10 ml of a mixture of $$CH_{4}, C_{2}H_{4}$$ and $$CO_{2}$$ were exploded with excess of air. After explosion, there was contraction on cooling of 17 ml and after treatment with KOH, there was further reduction of 14 ml. What is the composition of the mixture?
  • $$CH_{4}= 4.5 ml, CO_{2}= 1.5 ml$$
  • $$CH_{4}= 3.6 ml, CO_{2}= 2.5 ml$$
  • $$CH_{4}= 4.8 ml, CO_{2}= 1.8 ml$$
  • $$CH_{4}= 5.1 ml, CO_{2}= 2.8 ml$$
40 ml of mixture of $$C_{2}H_{2}$$ and CO is mixed with 100 ml of $$O_{2}$$ gas and the mixture is exploded. The residual gases occupied 104 ml and when these are passed through KOH solution, the volume becomes 48ml. All the volume are at same the temperature and pressure. Determine the composition of the original mixture.
  • $$\displaystyle\:C_{2}H_{2}= 16 ml, CO= 24 ml$$
  • $$\displaystyle\:C_{2}H_{2}= 23 ml, CO= 14 ml$$
  • $$\displaystyle\:C_{2}H_{2}= 30 ml, CO= 26 ml$$
  • $$\displaystyle\:C_{2}H_{2}= 33 ml, CO= 28 ml$$
A $$0.60$$ g nitrogen containing compound was boiled with $$NaOH$$, and $$NH_3$$ thus formed, required $$100$$ mL of $$0.2$$ N $$H_2SO_4$$ for neutralisation. The percentage of nitrogen in the compound is:
  • $$46.67\%$$
  • $$23.34\%$$
  • $$60.00\%$$
  • $$20.00\%$$
Number of $$K^+$$ ions and number of moles of $$K^+$$ ions present in $$1\:L$$ of $$\displaystyle\frac{N}{5}\:KMnO_4$$ solution respectively, in acidic medium are :
  • $$0.04$$ and $$2.4\times{10}^{22}$$
  • $$2.4\times{10}^{22}$$ and $$0.04$$
  • $$200$$ and $$6.023\times{10}^{23}$$
  • $$6.023\times{10}^{23}$$ and $$200$$
Which of the following have equal mass of $$Cl^-$$ ions in $$1.0$$ L of each of the following solutions?
  • $$5\%\ NaCl$$ (density $$= 1.07$$ g/mL)
  • $$5\%\ KCl$$ (density $$=1.06$$ g/mL)
  • $$58.5$$ g of $$NaCl$$
  • $$55.5$$ g of $$BaCl_2$$
The $$\%$$ loss in weight after heating a pure sample of potassium chlorate (Molecular weight $$= 122.5$$ g/mol) will be:
  • $$12.25$$
  • $$24.5$$
  • $$39.2$$
  • $$19.6$$
The number of $${Ag}^{+}$$ ion in one drop of silver nitrate solution is:
  • $$2.12\times {10}^{20}$$
  • $$7.2\times {10}^{20}$$
  • $$7.2\times {10}^{21}$$
  • $$7.2\times {10}^{19}$$
If the percentage of water of crystallization in $$MgSO_4.xH_2O$$ is $$13\%$$, then what is the value of $$x$$?
  • $$1$$
  • $$4$$
  • $$5$$
  • $$7$$
The percentage of $${P}_{2}{O}_{5}$$ in diammonium hydrogen phosphate $$[{(N{H}_{4})}_{2}HP{O}_{4}]$$ is : 
  • $$23.48 \%$$
  • $$53.78 \%$$
  • $$46.96 \%$$
  • $$71.0 \%$$
Mole fraction of ethanol in ethanol-water mixture is $$0.25$$. Hence, the percentage concentration of ethanol by weight of the mixture is:
  • $$25\%$$
  • $$75\%$$
  • $$46\%$$
  • $$54\%$$
A mineral consists of an equimolar mixture of the carbonates of two bivalent metals. One metal is present to the extent of $$15.0\%$$ by weight. $$3.0$$ g of the mineral on heating lost $$1.10$$ g of $$CO_2$$. The percent by weight of other metal is :
  • $$65$$
  • $$25$$
  • $$75$$
  • $$35$$
A hydrate of $$Na_2SO_3$$ has $$50\%$$ water by mass. It is :
  • $$Na_2SO_3\cdot 4H_2O$$
  • $$Na_2SO_3\cdot 6H_2O$$
  • $$Na_2SO_3\cdot 7H_2O$$
  • $$Na_2SO_3\cdot 2H_2O$$
An aqueous solution of $$NaOH$$ having density $$1.1$$ $$kg/{dm}^{3}$$ contains $$0.02$$ mole fraction of $$NaOH$$. The $$\%$$ by mass of $$NaOH$$ in the solution is :
  • $$4.34$$
  • $$2.17$$
  • $$5.28$$
  • $$8.34$$
A $$1000$$ g sample of $$NaOH$$ contains $$3$$ moles of $$O$$ atom, what is the purity of $$NaOH$$?
  • $$14\%$$
  • $$100\%$$
  • $$12\%$$
  • $$24\%$$
The molality of $$1$$ L solution with $$x\%$$ $$H_2SO_4$$ is $$9$$. The weight of the solvent present in the solution is $$910$$ g. The value of $$x$$ is:
  • $$90$$
  • $$49$$
  • $$30$$
  • $$47$$
$$Na_2SO_\:xH_2O$$ has $$50\%$$ $$H_2O$$. Hence, $$x$$ is :
  • $$4$$
  • $$5$$
  • $$6$$
  • $$8$$
Cortisone is a molecular substance containing $$21$$ atoms of carbon per molecule. The mass percentage of carbon in cortisone is $$69.98$$%. Its molar mass is:
  • $$176.5$$
  • $$252.2$$
  • $$287.6$$
  • $$360.1$$
The sodium salt of methyl orange has $$7\%$$ sodium. What is the minimum molecular weight of the compound?
  • $$420$$
  • $$375$$
  • $$329$$
  • $$295$$
Mole fraction of ethanol and water mixture is $$0.25$$. Hence, percentage concentration of ethanol by weight of mixture is:
  • $$25\%$$
  • $$75\%$$
  • $$46\%$$
  • $$54\%$$
The simplest formula of a compound containing $$50$$% of element $$X$$ (Atomic mass $$=$$ $$10$$) and $$50$$% of the element $$Y$$ (Atomic mass $$=$$ $$20$$) by weight is: 
  • $$XY$$
  • $$X_2Y$$
  • $$XY_2$$
  • $$X_2Y_3$$
A spherical ball of radius $$7$$ cm contains $$56\%$$ iron. If density is $$1.4$$ g/cc, the number of moles of $$Fe$$ present approximately is :
  • $$10$$
  • $$15$$
  • $$20$$
  • $$25$$
Which of the following is a suitable example for illustrating the law of conservation of mass?
 (Atomic mass of O = 16 g/mol, H = 1 g/mole)
  • $$18$$ g of water is formed by the combination of $$16$$ g oxygen with $$2$$ g of hydrogen.
  • $$18$$ g of water in liquid state is obtained by heating $$18$$ g of ice.
  • $$18$$ g of water is completely converted into vapour state on heating.
  • $$18$$ g of water freezes at $$4^oC$$ to give same mass of ice.
A mixture of $$CuSO_4.5H_2O$$ and $$MgSO_4.7H_2O$$ was heated until all the water was driven off. If $$5.0$$ g of mixture gave $$3$$ g of anhydrous salt, what was the percentage by mass of $$CuSO_4.5H_2O$$ in the original mixture?
  • $$74.4$$
  • $$70$$
  • $$80$$
  • $$90$$
Two beakers $$A$$ and $$B$$ present in a closed vessel. Beaker $$A$$ contains $$152.4\:g$$ aqueous solution of urea, containing  $$12\:g$$ of urea. Beaker $$B$$ contains $$196.2\:g$$ glucose solution, containing $$18\:g$$ of glucose. Both the solutions allowed to attain the equilibrium. Determine weight $$\%$$ of glucose in its solution is at equilibrium.
  • $$\;25\%$$
  • $$\;10\%$$
  • $$\;18\%$$
  • $$\;15.5\%$$
A salt is formed due to the reaction between an oxy acid containing chlorine and a base containing a monovalent metal of atomic mass $$x$$. The number of oxygen atoms in one molecule of the acid is more than the corresponding 'ic' acid. Calculate the molecular mass of the salt.
  • $$\displaystyle 83.5 + \frac{x}{4}$$
  • 99.5 + $$x$$
  • 83.5 + $$x$$
  • $$\displaystyle 99.5 + \frac{x}{2}$$
If 40 g of ethyl alcohol is dissolved in 50 ml of water, then calculate the weight/volume percentage of ethyl alcohol present in the solution? [Density of ethyl alcohol = 0.8 g/ml].
  • 40%
  • 30%
  • 25%
  • 35%
$$\displaystyle n_{1}$$ g of substance X reacts with $$\displaystyle n_{2}$$ g of substance Y to form $$\displaystyle m_{1}$$ g of substance R and $$\displaystyle m_{2}$$ g of substance of S. This reaction can be represented as $$X + Y \rightarrow R + S$$. The relation which can be established in the amounts of the reactants and the products will be :
  • $$\displaystyle n_{1}-n_{2}=m_{1}-m_{2}$$
  • $$\displaystyle n_{1}+n_{2}=m_{1}+m_{2}$$
  • $$\displaystyle n_{1}=n_{2}$$
  • $$\displaystyle m_{1}=m_{2}$$
A certain compound has the molecular formula, $$\displaystyle X_{4}O_{6}$$. If $$10$$ g of compound contains $$5.62$$ g of X, the atomic mass of X is approximately :
  • 32 amu
  • 30.8 amu
  • 42 amu
  • 48 amu
The number of electrons required to deposit $$1$$ g atom of Al (atomic wt. $$=27$$) from a solution of $$AlCl_3$$ is:
  • $$1N_A$$
  • $$2N_A$$
  • $$3N_A$$
  • $$4N_A$$
The hydrated salt, $$\displaystyle Na_{2}SO_{4}.nH_{2}O$$ undergoes 56% loss in weight on heating and becomes anhydrous. The value of n (approx.) will be :
  • 5
  • 3
  • 7
  • 10
For 7 molal $$NaOH$$ solution. Select the correct statement
  • %$$\left(\displaystyle\frac{w}{w}\right) = 28$$
  • %$$\left(\displaystyle\frac{w}{w}\right) = 72$$
  • $${ X }_{ { H }_{ 2 }O }= \displaystyle\frac { 7 }{ 47 } $$
  • $${ X }_{ NaOH }= \displaystyle\frac { 7 }{ 47 } $$
"All gases have the same number of moles in the same volume at constant temperature and pressure:. This statments belongs to :
  • Boyle's law
  • Charles's law
  • Avogadro's principle
  • ideal gas law
  • Dalton's law
Statement 1: At the same temperature and pressure, 1 L of hydrogen gas and  1 L of neon gas have the same mass.
Statement 2: Equal volumes of ideal gases at the same temperature and pressure contain the same number of moles.

  • Both statement 1 and statement 2 are correct and statement 2 is the correct explanation of statement 1

  • Both statement 1 and statement 2 are correct but Statement 2 is not the correct explanation of Statement 1

  • Statement 1 is correct but statement 2 is incorrect

  • Statement 1 is incorrect but statement 2 is correct

  • Both the statement 1 and statement 2 are incorrect

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