JEE Main & Advanced Chemistry Some Basic Concepts of Chemistry / रसायन की कुछ मूलभूत अवधारणाएँ Question Bank

done Topic Test - Some Basic Concepts of Chemistry Total Questions - 35

• question_answer1)
  What is the atomic weight of an element X for which a sample containing \[1.58\times {{10}^{22}}\] atoms weigh 1.05 g?
  A)
  28 g done clear
  B)
  20 g done clear
  C)
  40 g done clear
  D)
  23 g done clear
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• question_answer2)
  When \[Fe{{S}_{2}}\] is burnt in air, it converts into \[F{{e}_{2}}{{O}_{3}}.\] The change in percentage by weight of iron in the process is (Fe = 56)
  A)
  23% increase done clear
  B)
  12% decrease done clear
  C)
  12% increase done clear
  D)
  no change done clear
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• question_answer3)
  An analysis of organic compound gave 74.0% C, 8.65% of H and 17.3% N. What is the empirical formula of compound?
  A)
  \[{{C}_{5}}{{H}_{8}}N\] done clear
  B)
  \[{{C}_{10}}{{H}_{12}}N\] done clear
  C)
  \[{{C}_{5}}{{H}_{7}}N\] done clear
  D)
  \[{{C}_{10}}{{H}_{14}}N\] done clear
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• question_answer4)
  How many grams of \[CaO\] are required to neutralize 852 g of \[{{P}_{4}}{{O}_{10}}\]?
  A)
  1008 g done clear
  B)
  108 g    done clear
  C)
  1800 g done clear
  D)
  3600 g done clear
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• question_answer5)

  Calcium carbonate reacts with aqueous HCl to give \[CaC{{l}_{2}}\] and \[C{{O}_{2}}\] according to the reaction,

  \[CaC{{O}_{3}}(s)+2HCl(aq)\to \]\[CaC{{l}_{2}}(aq)+C{{O}_{2}}(g)+{{H}_{2}}O(l)\]

  In this reaction, 250 mL of 0.76 M HCI reacts with 1000 g of \[CaC{{O}_{3}}.\] Calculate the mass of \[CaC{{l}_{2}}\] formed in the reaction.

  A)
   11.1 g done clear
  B)
  10.54 g  done clear
  C)
  5.25 g done clear
  D)
  2.45 L done clear
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• question_answer6)
  A hydrocarbon contains 10.5 g carbon and 1g hydrogen. Its 2.4 g has 1 L volume as 1 atm and\[{{127}^{o}}C\]. Hydrocarbon is
  A)
  \[{{C}_{6}}{{H}_{7}}\] done clear
  B)
  \[{{C}_{6}}{{H}_{6}}\] done clear
  C)
  \[{{C}_{5}}{{H}_{6}}\] done clear
  D)
  \[{{C}_{6}}{{H}_{6}}\] done clear
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• question_answer7)

  Nitric acid can be produced from \[N{{H}_{3}}\] in three step process

  I. \[4N{{H}_{3}}(g)+5{{O}_{2}}(g)\xrightarrow{{}}4NO(g)+6{{H}_{2}}O(g)\]

  II. \[2NO(g)+{{O}_{2}}(g)\xrightarrow{{}}2N{{O}_{2}}(g)\]

  III. \[3N{{O}_{2}}(g)+{{H}_{2}}O(l)\xrightarrow{{}}2HN{{O}_{3}}(aq)+NO(g)\]

  % yield of Ist, IInd and IIIrd are respectively 40%, 50% and 70% respectively, then what volume of\[N{{H}_{3}}(g)\] sit 1 atm and \[0{}^\circ C\] required to produce 1075 g of \[HN{{O}_{3}}\]?

  A)
  3413 L done clear
  B)
  3500 L done clear
  C)
  6826 L done clear
  D)
  1750 L done clear
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• question_answer8)
  It is known that atoms have proton, neutron, electron and nucleus. If the mass of neutron assumed to be half of its original value whereas that of proton is assumed to be twice the original value, then the atomic mass of \[_{6}{{C}^{14}}\] will be
  A)
  14.3% less than original value done clear
  B)
  14.3% greater than original value done clear
  C)
  28.6% less than original value done clear
  D)
  28.6% greater than original value done clear
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• question_answer9)

  Arrange the following (I to IV) in the order of increasing masses.

  I. 0.5 mole of \[{{O}_{3}}\]

  II. \[3.01\times {{10}^{23}}\] molecules of \[{{O}_{2}}\]

  III. 5.6 L of \[C{{O}_{2}}\] at STP

  IV. 0.5 g atom of \[{{O}_{2}}\]

  A)
  IV < III < II < I done clear
  B)
  II < I < III < IV done clear
  C)
  II = I < III < IV done clear
  D)
  I < III < IV < II done clear
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• question_answer10)
  A 0.70 g sample consisting \[Ca{{C}_{2}}{{O}_{4}}\] and \[Mg{{C}_{2}}{{O}_{4}}\] is heated at \[300{}^\circ C,\] converting the two salts of \[CaC{{O}_{3}}\]  and \[MgC{{O}_{3}}\]. The sample when weighs 0.47 g. If the sample had been heated to \[700{}^\circ C\] where the products are CaO and MgO. What would be the weight of mixture of oxides?
  A)
  0.36 g done clear
  B)
  0.14 g done clear
  C)
  0.28 g done clear
  D)
  1.08 g done clear
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• question_answer11)
  23.2 g of an organic compound having molecular formula \[{{C}_{n}}{{H}_{2n+2}}\] is burnt in excess of \[{{O}_{2}}(g)\]initially taken in a 44.82 L steel vessel. Before reaction the gaseous mixture w at 273 K with pressure of 2 aim. After complete combustion and loss of considerable amount of heat the mixture of product and excess of had a temperature of 546 K and 4.6 atm pressure. The formula of compound is
  A)
  \[{{C}_{5}}{{H}_{12}}\] done clear
  B)
  \[{{C}_{6}}{{H}_{10}}\] done clear
  C)
  \[{{C}_{3}}{{H}_{8}}\] done clear
  D)
  \[{{C}_{4}}{{H}_{10}}\] done clear
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• question_answer12)
  How many moles of electron weigh one kilogram?
  A)
  \[6.023\times {{10}^{23}}\] done clear
  B)
  \[\frac{1}{9.108}\times {{10}^{31}}\] done clear
  C)
  \[\frac{6.023}{9.108}\times {{10}^{54}}\]                     done clear
  D)
  \[\frac{1}{9.108\times 6.023}\times 108\] done clear
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• question_answer13)
  The volume of concentrated sulphuric acid which is 98% by mass (density \[=1.84\,g\,c{{m}^{-3}}\]) required to prepare \[5\,d{{m}^{3}}\] of \[0.5\text{ }mol\text{ }d{{m}^{-3}}\] solution of sulphuric acid is
  A)
  272 mL done clear
  B)
  68 mL    done clear
  C)
  136 mL  done clear
  D)
  204 mL done clear
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• question_answer14)
  2.76 g of silver carbonate on being strongly heated yields a residue weighing
  A)
  2.15 g done clear
  B)
  2.48 g    done clear
  C)
  2.32 g done clear
  D)
  2.64 g done clear
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• question_answer15)
  Two elements X and Y have atomic weights of 14 and 16. They form a series of compounds A, B, C, D and E in which the same amount of element X, Y is present in the ratio 1 : 2 : 3 : 4 : 5. If the compound A has 28 parts by weight of X and 16 parts by weight of Y, then the compound of C will have 28 parts weight of X and
  A)
  32 parts by weight of Y done clear
  B)
  48 parts by weight of Y done clear
  C)
  64 parts by weight of Y done clear
  D)
  80 parts by weight of Y done clear
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• question_answer16)
  What weight of \[{{H}_{2}}{{C}_{2}}{{O}_{4}}\,\,2{{H}_{2}}O\,\,(\text{mol}\text{.}\,\text{wt}\text{.}\,=126)\] should be dissolved to prepare 250 ml of cent normal to be used as a reducing agent?
  A)
  0.63 gm done clear
  B)
  0.1575 gm done clear
  C)
  0.126 gm done clear
  D)
  0.875 gm done clear
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• question_answer17)
  Apatite is a mineral that is found in tooth enamel. When fluoride toothpastes are used, this mineral is converted to fluoroapatite, which is more resistant to tooth decay. The formula of apatite is \[C{{a}_{5}}{{(P{{O}_{4}})}_{x}}F\]. What is the value of \[x\] if the compound contains 18.45% by weight of phosphorus? (Atomic weight of \[P=31,\,\,Ca=40,\]\[F=19\] and \[O=16\])
  A)
  2 done clear
  B)
  4            done clear
  C)
        5 done clear
  D)
  3 done clear
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• question_answer18)
  Calculate the weight of lime (CaO) obtained by heating 200 kg of 95% pure lime stone \[(CaC{{O}_{3}}).\]
  A)
  104.4 kg done clear
  B)
  105.4 kg done clear
  C)
  212.8 kg done clear
  D)
  106.4 kg done clear
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• question_answer19)
  The chloride of a metal has the formula \[MC{{l}_{4}}\]. The formula of its phosphate will be-
  A)
  \[{{M}_{2}}P{{O}_{4}}\] done clear
  B)
  \[MP{{O}_{4}}\] done clear
  C)
  \[{{M}_{3}}P{{O}_{4}}\] done clear
  D)
  \[M{{(P{{O}_{4}})}_{2}}\] done clear
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• question_answer20)
  A silver coin weighing 11.34 g was dissolved in nitric acid. When sodium chloride was added to the solution all the silver (present as \[AgN{{O}_{3}}\]) was precipitated as silver chloride. The weight of the precipitated silver chloride was 14.35 g. Calculate the percentage of silver in the coin - 
  A)
  4.8% done clear
  B)
  95.2% done clear
  C)
  90%      done clear
  D)
  80% done clear
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• question_answer21)

  A self-contained breathing apparatus used \[K{{O}_{2}}\] to convert \[C{{O}_{2}}\] and \[{{H}_{2}}O\] in exhaled air into oxygen and \[KHC{{O}_{3}}\] as shown in the equation \[K{{O}_{2}}+{{H}_{2}}O+C{{O}_{2}}\xrightarrow{\,}\,KHC{{O}_{3}}+{{O}_{2}}\].

  How many molecules of \[{{O}_{2(g)}}\] will be produced from the 0.044 g of \[C{{O}_{2(g)}}\] that is exhaled in a typical breath?

  A)
  \[6\times {{10}^{20}}\] done clear
  B)
  \[4.5\times {{10}^{20}}\] done clear
  C)
  \[2.25\times {{10}^{21}}\] done clear
  D)
  \[4.5\times {{10}^{22}}\] done clear
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• question_answer22)
  The empirical formula of a compound composed of 38.4% potassium, 36.3% oxygen, 23.7% carbon and 1.66% hydrogen is determined to be
  A)
  \[~K{{C}_{2}}{{H}_{5}}{{O}_{4}}\] done clear
  B)
  \[{{K}_{3}}{{C}_{6}}{{H}_{5}}{{O}_{7}}\] done clear
  C)
  \[{{K}_{2}}CH{{O}_{3}}\] done clear
  D)
  \[{{K}_{6}}{{C}_{4}}{{H}_{5}}{{O}_{7}}\] done clear
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• question_answer23)
  How many years it would take to spend Avogadro's number of rupees at the rate of 1 million rupees in one second?
  A)
  \[19.098\times {{10}^{19}}\] years        done clear
  B)
  \[19.098\] years done clear
  C)
  \[19.098\times {{10}^{9}}\] years   done clear
  D)
              None of these done clear
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• question_answer24)
  15 grams of methyl alcohol is dissolved grams of water. What is the mass percent methyl alcohol in solution?
  A)
  30% done clear
  B)
  50% done clear
  C)
  70% done clear
  D)
  75% done clear
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• question_answer25)
  Three isotopes of an element have mass numbers M, (M + 1) and (M + 2). The mean atomic mass is (M + 0.5). Then which of the following ratio maybe accepted for M, (M + 1), (M + 2) respectively
  A)
  1 : 1 : 1 done clear
  B)
  4 : 1 : 1 done clear
  C)
  3 : 2 : 1 done clear
  D)
  2 : 1 : 1 done clear
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• question_answer26)
  A gaseous compound is composed of 85.7% by mass of carbon and 14.3% by mass of hydrogen. Its density is 22.8 g/L at 350 K and 1.0 atm pressure. Calculate the molecular formula of compound.
  A)
  \[{{C}_{5}}{{H}_{10}}\] done clear
  B)
  \[{{C}_{6}}{{H}_{12}}\] done clear
  C)
  \[{{C}_{4}}{{H}_{8}}\] done clear
  D)
  \[{{C}_{8}}{{H}_{18}}\] done clear
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• question_answer27)
  If 3 moles of \[{{H}_{2}}\] and 1 mole of \[{{N}_{2}}\] are completely converted into \[N{{H}_{3}},\] the ratio of initial and final volume at the same temp. and pressure will be:
  A)
  1 done clear
  B)
  3 done clear
  C)
  2 done clear
  D)
  4.20 done clear
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• question_answer28)
  1 mol of a gaseous aliphahatic compound\[{{C}_{n}}{{H}_{3n}}{{O}_{m}}\] is completely burnt in an excess of oxygen. The contraction in volume is (assume water get condensed out)
  A)
  \[\left( 1+\frac{1}{2}n-\frac{3}{4}m \right)\] done clear
  B)
  \[\left( 1+\frac{3}{4}n-\frac{1}{4}m \right)\] done clear
  C)
  \[\left( 1-\frac{1}{2}n-\frac{3}{4}m \right)\] done clear
  D)
              \[\left( 1+\frac{3}{4}n-\frac{1}{2}m \right)\] done clear
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• question_answer29)
  X and Y are two elements which form \[{{X}_{2}}{{Y}_{3}}\] and \[{{X}_{3}}{{Y}_{4}}\]. If 0.20 mol of \[{{X}_{2}}{{Y}_{2}},\] weighs 32.0 g and 0.4 mol of \[{{X}_{3}}{{Y}_{4}}\] weighs 92.8 g, the atomic weights of X and Y are respectively
  A)
  16.0 and 56.0 done clear
  B)
  8.0 and 28.0        done clear
  C)
  56.0 and 16.0 done clear
  D)
  28.0 and 8.0 done clear
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• question_answer30)
  How many H-atoms are present in 0.046 got ethanol?
  A)
  \[6\times {{10}^{20}}\] done clear
  B)
  \[1.2\times {{10}^{21}}\] done clear
  C)
  \[3\times {{10}^{21}}\] done clear
  D)
  \[3.6\times {{10}^{21}}\] done clear
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• question_answer31)
  Chlorophyll, the green colouring matter of plants responsible for photosynthesis, contains 2.68% of magnesium by mass. Calculate the number of magnesium atoms in 2.00g of chlorophyll.
  A)
  \[1.345\times {{10}^{21}}\] done clear
  B)
  \[1.345\times {{10}^{20}}\] done clear
  C)
  \[13.45\times {{10}^{21}}\]      done clear
  D)
  \[1.345\times {{10}^{23}}\] done clear
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• question_answer32)
  Minimum amount of \[A{{g}_{2}}C{{O}_{3}}(s)\] required to produce sufficient oxygen for the complete combustion of C, H, which produces 11.2 ltr. of \[C{{O}_{2}}\] at S.T.P after combustion is: [Ag = 108] \[A{{g}_{2}}C{{O}_{3}}(s)\to 2Ag(s)+C{{O}_{2}}(g)+1/2{{O}_{2}}(g)\]\[{{C}_{2}}{{H}_{2}}+5/2{{O}_{2}}\to 2C{{O}_{2}}+{{H}_{2}}O\]
  A)
  276 g done clear
  B)
  345 g  done clear
  C)
  690 g done clear
  D)
  1380 g done clear
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• question_answer33)
  In the reaction \[4A+2B+3C\xrightarrow{{}}{{A}_{4}}{{B}_{2}}{{C}_{3}}\] what will be the number of moles of product formed. Starting from 2 moles of A, 1.2 moles of B & 1.44 moles of C:
  A)
  0.5 done clear
  B)
  0. 6 done clear
  C)
  0.48 done clear
  D)
              4.64 done clear
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• question_answer34)
  About \[6\times {{10}^{-3}}\] mol \[{{K}_{2}}C{{r}_{2}}{{O}_{7}}\] reacts completely with \[9\times {{10}^{-3}}\] mol \[{{X}^{n+}}\] to give \[X{{O}^{-}}_{3}\] and \[C{{r}^{3+}}\]. The value of \[n\] is:
  A)
  1 done clear
  B)
  2            done clear
  C)
  3 done clear
  D)
  none of these done clear
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• question_answer35)
  About 0.5 g of hydrocarbon gave 0.9 g water on combustion. The percentage of carbon in hydrocarbon is:
  A)
  75.8 done clear
  B)
  80.0          done clear
  C)
  56.6 done clear
  D)
  28.6 done clear
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