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

done Self Evaluation Test - Some Basic Concepts of Chemistry Total Questions - 70

• question_answer1)

  If the true value for an experimental result is 6.23 and the results reported by three students X, Y and Z are:

  X: 6.18 and 6.28

  Y: 6.20 and 6.023

  Z: 6.22 and 6.24

  Which of the following option is correct?
  A)
  X precise, Y accurate, Z precise and accurate. done clear
  B)
  X precise and accurate, Y not precise, Z precise done clear
  C)
  Both X & Z precise & accurate, Y not precise. done clear
  D)
  Both X & Y neither precise nor accurate, Z both precise and accurate. done clear
  View Solution play_arrow

• question_answer2)
  Irrespective of the source, pure sample, of water always yields 88.89% mass of oxygen and 11.11% mass of hydrogen. This is explained by the law of
  A)
  conservation of mass done clear
  B)
  multiple proportions done clear
  C)
  constant composition done clear
  D)
  constant volume done clear
  View Solution play_arrow

• question_answer3)
  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
  A)
  \[1.568\times {{10}^{3}}\]        done clear
  B)
  \[1.568\times {{10}^{4}}\] done clear
  C)
  15.68                            done clear
  D)
  \[3.136\times {{10}^{4}}\] done clear
  View Solution play_arrow

• question_answer4)
  The amount of zinc required to produce 224 mL of \[{{H}_{2}}\] at STP on treatment with dil. \[{{H}_{2}}S{{O}_{4}}\] will be
  A)
  6.5 g         done clear
  B)
  0.65 g done clear
  C)
  65 g                              done clear
  D)
  0.065g done clear
  View Solution play_arrow

• question_answer5)
  Assuming fully decomposed, the volume of \[C{{O}_{2}}\] released at STP on heating 9.85 g of \[BaC{{O}_{3}}\] (Atomic mass, Ba = 137) will be
  A)
  1.12L    done clear
  B)
  2.24L done clear
  C)
  4.06L                done clear
  D)
  0.84L done clear
  View Solution play_arrow

• question_answer6)
  The number of water molecules present in a drop of water (volume 0.0018 mL) density =\[18m{{L}^{-1}}\] at room temperature is
  A)
  \[1.084\times {{10}^{18}}\]                  done clear
  B)
  \[6.023\times {{10}^{19}}\] done clear
  C)
  \[4.84\times {{10}^{17}}\]       done clear
  D)
  \[6.023\times {{10}^{23}}\] done clear
  View Solution play_arrow

• question_answer7)
  1.44 g of titanium (At. mass = 48) reacted with excess of \[{{O}_{2}}\] and produce x g of non-stoichiometric compound \[T{{i}_{1.44}}O\]. The value of x is:
  A)
  2            done clear
  B)
  1.77 done clear
  C)
  1.44                              done clear
  D)
  none of these done clear
  View Solution play_arrow

• question_answer8)
  Silver oxide \[(A{{g}_{2}}O)\] decomposes at temperature \[300{}^\circ C\] yielding metallic silver and oxygen gas.  A 1.60 g sample of impure silver oxide yields 0.104 g of oxygen gas. What is the per cent by mass of the silver oxide in the sample?
  A)
  5.9                    done clear
  B)
  47.125 done clear
  C)
  94.25    done clear
  D)
  88.2 done clear
  View Solution play_arrow

• question_answer9)
  A sample of \[Al{{F}_{3}}\] contains \[3.0\times {{10}^{24}}{{F}^{-}}\] ions. The number of formula unit of this sample are-
  A)
  \[9\times {{10}^{24}}\]            done clear
  B)
  \[3\times {{10}^{24}}\] done clear
  C)
  \[0.75\times {{10}^{24}}\]       done clear
  D)
  \[1.0\times {{10}^{24}}\] done clear
  View Solution play_arrow

• question_answer10)
  Dissolving 120 g of a compound of mol. wt. 60 in 1000 g of water gave a solution of density 1.12 g/mL. The molarity of the solution is:
  A)
  \[1.00 M\]                       done clear
  B)
  \[2.00\text{ }M\] done clear
  C)
  \[2.50\text{ }M\]            done clear
  D)
  \[4.00\text{ }M\] done clear
  View Solution play_arrow

• question_answer11)
  A mixture of \[{{O}_{2}}\] and gas "Y" mol. mass 80 in the mole ratio a : b has a mean molecular mass 40. What would be mean molecular mass, if the gases are mixed in the ratio b : a under, identical conditions? (Assume that gases are non-reacting):    
  A)
  40                     done clear
  B)
  48    done clear
  C)
  62                                 done clear
  D)
  72 done clear
  View Solution play_arrow

• question_answer12)
  If \[3.01\times {{10}^{20}}\]molecules are removed from 98 mg of \[{{H}_{2}}S{{O}_{4}}\] then the number of moles of\[{{H}_{2}}S{{O}_{4}}\] left are
  A)
  \[0.1\times {{10}^{-3}}\]          done clear
  B)
  \[0.5\times {{10}^{-3}}\] done clear
  C)
  \[1.66\times {{10}^{-3}}\]         done clear
  D)
  \[9.95\times {{10}^{-2}}\] done clear
  View Solution play_arrow

• question_answer13)
  The number of molecules in 8.96 litre of a gas at  \[0{}^\circ C\] and 1 atm. pressure is approximately
  A)
  \[6.023\times {{10}^{23}}\]                  done clear
  B)
  \[12.04\times {{10}^{23}}\] done clear
  C)
  \[18.06\times {{10}^{23}}\]                  done clear
  D)
  \[24.08\times {{10}^{22}}\] done clear
  View Solution play_arrow

• question_answer14)
  The density of 3M solution of sodium chloride is \[1.252g\text{ }m{{L}^{-1}}\]. The molality of the solution will be (molar mass,\[NaCl=585gmo{{l}^{-1}}\])
  A)
  2.60 m              done clear
  B)
  2.18 m done clear
  C)
  2.79 m done clear
  D)
  3.00 m done clear
  View Solution play_arrow

• question_answer15)
  Indium (atomic mass = 114.82) has two natural occurring isotopes, the predominant one four has isotopic mass 114.9041 and abundance of 95.72%. Which of the following isotopic mass is the most likely for the other isotope?
  A)
  112.94   done clear
  B)
  115.90 done clear
  C)
  113.90             done clear
  D)
  114.90 done clear
  View Solution play_arrow

• question_answer16)
  A compound contains 54.55 % carbon, 9.09% hydrogen, 36.36% oxygen. The empirical formula of this compound is:
  A)
  \[{{C}_{3}}{{H}_{5}}O\]                     done clear
  B)
  \[{{C}_{4}}{{H}_{8}}{{O}_{2}}\] done clear
  C)
  \[{{C}_{2}}{{H}_{4}}{{O}_{2}}\]                   done clear
  D)
  \[{{C}_{2}}{{H}_{4}}O\] done clear
  View Solution play_arrow

• question_answer17)
  An organic compound whose empirical and molecular formula are same, contains 20% carbon, 6.7% hydrogen, 46.7% nitrogen and the rest oxygen. On heating it yields ammonia, leaving a solid residue. The solid residue gives a violet colour with dilute solution of alkaline copper sulphate. The organic compound is
  A)
  \[N{{H}_{2}}COON{{H}_{4}}\]           done clear
  B)
  \[HCOON{{H}_{4}}\] done clear
  C)
  \[N{{H}_{2}}NHCHO\]    done clear
  D)
    \[N{{H}_{2}}CON{{H}_{2}}\] done clear
  View Solution play_arrow

• question_answer18)
  10 mL of 2 M NaOH solution is added to 200 mL of 0.5 M of NaOH solution. What is the final concentration?
  A)
  0.57 M   done clear
  B)
  5.7 M done clear
  C)
   11.4M              done clear
  D)
  1.14M done clear
  View Solution play_arrow

• question_answer19)

  Arrange the following in the order of increasing mass (atomic mass:\[O=16,\text{ }Cu=63,\text{ }N=14\])

  I. one atom of oxygen

  II.   one atom of nitrogen

  III.   \[1\times {{10}^{-10}}\] mole of oxygen

  IV.   \[1\times {{10}^{-10}}\] mole of copper

  A)
  II<I<III<IV    done clear
  B)
  I<II<III<IV done clear
  C)
  III<II<IV<I                   done clear
  D)
  IV<II<III<I done clear
  View Solution play_arrow

• question_answer20)
  The number of moles of oxygen in one litre of air containing 21% oxygen by volume, under standard conditions are
  A)
  0.0093 mole    done clear
  B)
  0.21 mole done clear
  C)
  2.10 mole          done clear
  D)
  0.186 mole done clear
  View Solution play_arrow

• question_answer21)
  The concentrated sulphuric acid that is peddled commercial is 95% \[{{H}_{2}}S{{O}_{4}}\] by weight. If the density of this commercial acid is \[1.834gc{{m}^{-3}}\], the molarity of this solution is
  A)
  17.8 M   done clear
  B)
  12.0.M done clear
  C)
  10.5 M              done clear
  D)
  15.7 M done clear
  View Solution play_arrow

• question_answer22)

  9 moles of "D" and 14 moles of E are allowed to react in a closed vessel according to given reactions. Calculate number of moles of B formed in the end of reaction, if 4 moles of G are present in reaction vessel. (Percentage yield of reaction is mentioned in the reaction)

  Step-1 \[3D+4E\xrightarrow{80%}~5C+A\]

  Step-2 \[3C+5G\,\xrightarrow{50%}6B+F\]

  A)
  2.4    done clear
  B)
  30    done clear
  C)
  4.8                    done clear
  D)
  1 done clear
  View Solution play_arrow

• question_answer23)
  A mixture of \[N{{H}_{4}}NO{{  }_{3}}\] and \[{{(N{{H}_{4}})}_{2}}HP{{O}_{4}}\] contain 30.40% mass per cent of nitrogen. What is the mass ratio of the two components in the mixture?
  A)
  2 : 1  done clear
  B)
  1 : 2  done clear
  C)
  3 : 4 done clear
  D)
  4 : 1 done clear
  View Solution play_arrow

• question_answer24)
  The mass of \[{{N}_{2}}{{F}_{4}}\] produced by the reaction of 2.0 g of \[N{{H}_{3}}\] and 8.0 g of \[{{F}_{2}}\] is 3.56 g. What is the per cent yield?

  \[2N{{H}_{3}}+5{{F}_{2}}\to {{N}_{2}}{{F}_{4}}+6HF\]

  A)
  79.0                              done clear
  B)
  71.2 done clear
  C)
  84.6                              done clear
  D)
  None of these done clear
  View Solution play_arrow

• question_answer25)
  The ppm level of \[{{F}^{-}}\] in a 500 g sample of a tooth paste containing \[0.2g\text{ }{{F}^{-}}\] is
  A)
  400   done clear
  B)
  1000  done clear
  C)
  250                   done clear
  D)
  200 done clear
  View Solution play_arrow

• question_answer26)
  Two glucose solutions are mixed. One has a volume of 480 mL and a concentration of 1.50 M and the second has a volume of 520 mL and concentration 1.20 M. The molarity of final solution is
  A)
  1.20M               done clear
  B)
  1.50M done clear
  C)
  1.34M       done clear
  D)
  2.70 M done clear
  View Solution play_arrow

• question_answer27)
  What is the volume of \[C{{O}_{2}}\] liberated (in litres) at 1 atmosphere and \[0{}^\circ C\] when 10 g of 100% pure calcium carbonate is treated with excess dilute sulphuric acid?

  (Atomic mass \[Ca:40,\text{ }C:12,O:16\])

  A)
  0.224    done clear
  B)
  2.24   done clear
  C)
  22.4                  done clear
  D)
  224 done clear
  View Solution play_arrow

• question_answer28)
  Complete combustion of \[0.858\text{ }g\] of compound X gives 2.64 g of \[C{{O}_{2}}\] and 1.26g of\[{{H}_{2}}O\]. The lowest molecular mass X can have:
  A)
  43 g                  done clear
  B)
  86 g done clear
  C)
  129 g                 done clear
  D)
  172 g done clear
  View Solution play_arrow

• question_answer29)
  The impure 6 g of NaCl is dissolved in water and then treated with excess of silver nitrate solution. The mass of precipitate of silver chloride is found to be 14 g. The % purity of NaCl solution would be:
  A)
  95%      done clear
  B)
  85% done clear
  C)
  75%                  done clear
  D)
  65% done clear
  View Solution play_arrow

• question_answer30)
  How many of \[0.1N\text{ }HCl\]are required to react completely with 1 g mixture of \[N{{a}_{2}}C{{O}_{3}}\] and \[NaHC{{O}_{3}}\]. containing equimolar amounts of two ?
  A)
  157.7mL        done clear
  B)
  15.77 mL done clear
  C)
  147.7 mL                      done clear
  D)
  14.77 mL done clear
  View Solution play_arrow

• question_answer31)
  5 g of benzene on nitration gave 6.6 g of nitrobenzene. The theoretical yield of the nitrobenzene will be
  A)
  4.5 g                 done clear
  B)
  5.6 g done clear
  C)
  8.09 g done clear
  D)
  6.6 g done clear
  View Solution play_arrow

• question_answer32)
  An aqueous solution of oxalic acid dehydrate contains its 6.3 g in 250 mL. The volume of \[0.1N\] NaOH required to completely neutralize 10 mL of this solution
  A)
  4 mL      done clear
  B)
  20 mL done clear
  C)
  2 mL                  done clear
  D)
  40 mL done clear
  View Solution play_arrow

• question_answer33)
  Choose the incorrect formula out of the four compounds for an element X below:
  A)
  \[{{X}_{2}}{{O}_{3}}\]                       done clear
  B)
  \[{{X}_{2}}C{{l}_{3}}\] done clear
  C)
  \[{{X}_{2}}{{(S{{O}_{4}})}_{3}}\]                 done clear
  D)
  \[XP{{O}_{4}}\] done clear
  View Solution play_arrow

• question_answer34)
  A gaseous compound of nitrogen and hydrogen contains 12.5% (by mass) of hydrogen. The density of the compound relative to hydrogen is 16. The molecular formula of the compound is:
  A)
  \[N{{H}_{2}}\] done clear
  B)
  \[{{N}_{3}}H\] done clear
  C)
  \[N{{H}_{3}}\]             done clear
  D)
  \[{{N}_{2}}{{H}_{4}}\] done clear
  View Solution play_arrow

• question_answer35)
  In an organic compound of molar mass \[108gmo{{l}^{-1}}C\], H and N atoms are present in 9 : 1 : 3.5 by mass. Molecular formula can be:
  A)
  \[{{C}_{6}}{{H}_{8}}{{N}_{2}}\] done clear
  B)
  \[{{C}_{7}}{{H}_{10}}N\] done clear
  C)
  \[{{C}_{5}}{{H}_{6}}{{N}_{3}}\]                   done clear
  D)
  \[{{C}_{4}}{{H}_{18}}{{N}_{3}}\] done clear
  View Solution play_arrow

• question_answer36)
  What is the empirical formula of vanadium oxide, If 2.74 g of the metal oxide contains 1.53 g of metal?
  A)
  \[{{V}_{2}}{{O}_{3}}\]           done clear
  B)
  \[VO\]   done clear
  C)
  \[{{V}_{2}}{{O}_{5}}\] done clear
  D)
  \[{{V}_{2}}{{O}_{7}}\] done clear
  View Solution play_arrow

• question_answer37)
  \[100c{{m}^{3}}\] of \[0.1N\text{ }HCl\] is mixed with \[100c{{m}^{3}}\] of \[0.2N\text{ }NaOH\] solution. The resulting solution is
  A)
  0.1 N and the solution is basic done clear
  B)
  0.1 N and the solution is acidic done clear
  C)
  0.05 N and the solution is basic done clear
  D)
  0.05 N and the solution is acidic done clear
  View Solution play_arrow

• question_answer38)
  On subjecting 10 mL mixture of \[{{N}_{2}}\] and CO to repeated electro spark, 7 mL of \[{{O}_{2}}\] was required for combustion. What was the mole percent of CO in the mixture? (All volumes were measured under identical conditions)
  A)
  60     done clear
  B)
  40     done clear
  C)
  6                                  done clear
  D)
  4 done clear
  View Solution play_arrow

• question_answer39)
  When burnt in air, 14.0 g mixture of carbon and sulphur gives a mixture of\[~C{{O}_{2}}\] and \[S{{O}_{2}}\] in the volume ratio of 2:1, volume being measured at the same conditions of temperature and pressure moles of carbon in the mixture is
  A)
  0.75                  done clear
  B)
  0.5    done clear
  C)
  0.40                  done clear
  D)
  0.25 done clear
  View Solution play_arrow

• question_answer40)
  What is the molarity of \[SO_{4}^{2-}\] ion in aqueous solution that contain 34.2 ppm of \[A{{l}_{2}}{{(S{{O}_{4}})}_{3}}\]? (Assume complete dissociation and density of solution 1 g/mL)  
  A)
  \[3\times {{10}^{-4}}M\]       done clear
  B)
  \[2\times {{10}^{-4}}M\] done clear
  C)
  \[{{10}^{-4}}M\]                     done clear
  D)
  None of these done clear
  View Solution play_arrow

• question_answer41)
  A transition metal M forms a volatile chloride which has a vapour density of 94.8. If it contains 74.75% of chlorine the formula of the metal chloride will be
  A)
  \[MC{{l}_{3}}\] done clear
  B)
  \[MC{{l}_{2}}\] done clear
  C)
  \[MC{{l}_{4}}\] done clear
  D)
  \[MC{{l}_{5}}\] done clear
  View Solution play_arrow

• question_answer42)
  50mL \[10N{{H}_{2}}S{{O}_{4}}\],  25mL \[12NHCl\] and  40ML 5N \[HN{{O}_{3}}\] were mixed together and the volume of the mixture was made 1000 mL by adding water. The normality of the resultant solution will be
  A)
  2N                                done clear
  B)
  1N   done clear
  C)
  3N                                done clear
  D)
  4N done clear
  View Solution play_arrow

• question_answer43)
  250 mL of a sodium carbonate solution contains 2.65 g of \[N{{a}_{2}}C{{O}_{3}}.\] If 10 mL of this solution is diluted to one litre, what is the concentration of the resultant solution? (mol. wt. of\[N{{a}_{2}}C{{O}_{3}}=106\])
  A)
  0.1 M                done clear
  B)
  0.01 M done clear
  C)
  0.001 M     done clear
  D)
  \[{{10}^{-4}}M\] done clear
  View Solution play_arrow

• question_answer44)
  3.92 g of ferrous ammonium sulphate crystals are dissolved in 100 mL of water. 20 mL of this solution requires 18 mL of potassium permaganate during titration for complete oxidation. The weight of \[KMn{{O}_{4}}\] present in one litre of the solution of
  A)
  3.47 g       done clear
  B)
  12.38 g done clear
  C)
  1.23 g                           done clear
  D)
  34.76 g done clear
  View Solution play_arrow

• question_answer45)
  1.12 mL of a gas is produced at S.T.P. by the action of 4.12 mg of alcohol ROH with methyl magnesium Iodide. The molecular mass of alcohol is
  A)
  16.0                  done clear
  B)
  41.2   done clear
  C)
  82.4  done clear
  D)
  156.0 done clear
  View Solution play_arrow

• question_answer46)

  How many moles of \[{{P}_{4}}\] can be produced by reaction of 0.10 moles \[C{{a}_{5}}{{(P{{O}_{4}})}_{3}}\text{F},0.36\] moles \[Si{{O}_{2}}\] and 0.90 moles C according to the following reaction?

  \[4C{{a}_{5}}{{\left( P{{O}_{4}} \right)}_{3}}F+18Si{{O}_{2}}+30C\xrightarrow{{}}\]\[3{{P}_{4}}+2Ca{{F}_{2}}+18CaSi{{O}_{3}}+30CO\]

  A)
  0.060    done clear
  B)
  0.030 done clear
  C)
  0.045                done clear
  D)
  0.075 done clear
  View Solution play_arrow

• question_answer47)
  1 mole of mixture of CO and \[C{{O}_{2}}\] requires exactly \[28g\text{ }KOH\] in solution for complete conversion of all the \[C{{O}_{2}}\] into\[{{K}_{2}}C{{O}_{3}}.\] How much amount more of KOH will be required for conversion into\[{{K}_{2}}C{{O}_{3}}.\] If one mole of mixture is completely oxidized to \[C{{O}_{2}}\]    
  A)
  112g     done clear
  B)
  84g done clear
  C)
  56g                               done clear
  D)
  28g done clear
  View Solution play_arrow

• question_answer48)

  2.0 g of a sample contains mixture of \[Si{{O}_{2}}\]and\[F{{e}_{2}}{{O}_{\text{3}}}\]. On very strong heating, it leaves a residue weighing 1.96 g. The reaction responsible for loss of mass is given below.

  \[F{{e}_{2}}{{O}_{3}}(s)\to F{{e}_{3}}{{O}_{4}}(s)+O(g),\](unbalance equation)

  What is the percentage by mass of \[Si{{O}_{2}}\] in original sample?

  A)
  100%    done clear
  B)
  20% done clear
  C)
  40% done clear
  D)
  60% done clear
  View Solution play_arrow

• question_answer49)
  20 g of \[CaC{{O}_{3}}\]on heating gave 8.8 g of \[C{{O}_{2}}\] and 11.2 g of CaO. This is in accordance with
  A)
  The law of conservation of mass. done clear
  B)
  The law of constant composition. done clear
  C)
  The law of reciprocal proportion. done clear
  D)
  None of these done clear
  View Solution play_arrow

• question_answer50)
  If 224 mL of a triatomic gas has a mass of 1 g at 273K and 1 atmospheric pressure then the mass of one atom is
  A)
  \[8.30\times {{10}^{-23}}g\]     done clear
  B)
  \[2.08\times {{10}^{-23}}g\] done clear
  C)
  \[5.53\times {{10}^{-23}}g\]     done clear
  D)
  \[6.24\times {{10}^{-23}}g\] done clear
  View Solution play_arrow

• question_answer51)

  Specific volume of cylindrical virus particle is \[6.02\times {{10}^{-2}}cc/g.\] whose radius and length are 7 \[\overset{\text{o}}{\mathop{\text{A}}}\,\] & 10 \[\overset{\text{o}}{\mathop{\text{A}}}\,\] respectively.

  If \[{{N}_{A}}=6.02\times {{10}^{23}}mo{{l}^{-1}}\] find molecular weight of virus

  A)
  \[3.08\times {{10}^{3}}kg/mol\] done clear
  B)
  \[3.08\times {{10}^{4}}kg/mol\] done clear
  C)
  \[1.54\times {{10}^{4}}kg/mol\] done clear
  D)
  \[15.4kg/mol\] done clear
  View Solution play_arrow

• question_answer52)
  1.575 g of oxalic acid \[{{(COOH)}_{2}}.x{{H}_{2}}O\] are dissolved in water and the volume made up to 250 mL. On titration 16.68 mL of this solution requires 25 mL of N/15 NaOH solution for complete neutralization, calculate x.
  A)
  3                      done clear
  B)
  2     done clear
  C)
  4                                  done clear
  D)
  5 done clear
  View Solution play_arrow

• question_answer53)
  2g of a mixture of CO and \[C{{O}_{2}}\] on reaction with excess \[{{I}_{2}}{{O}_{5}}\] produced 2.54 g of \[{{I}_{2}}\]. What will be the mass % of \[C{{O}_{2}}\] in the original mixture?
  A)
  35                     done clear
  B)
  70   done clear
  C)
  30         done clear
  D)
  60 done clear
  View Solution play_arrow

• question_answer54)

  Which statement is false for the balanced equation given below?

  \[C{{S}_{2}}+3{{O}_{2}}\xrightarrow{{}}2S{{O}_{2}}+C{{O}_{2}}\]

  A)
  One mole of \[C{{S}_{2}}\]will produce one mole of \[C{{O}_{2}}\] done clear
  B)
  The reaction of 16 g of oxygen produces 7.33g of \[C{{O}_{2}}\] done clear
  C)
  The reaction of one mole of\[{{O}_{2}}\] will produce 2/3 mole of \[C{{S}_{2}}\] done clear
  D)
  Six molecules of oxygen requires three molecules of \[C{{S}_{2}}\] done clear
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• question_answer55)
  Number of moles of \[KMn{{O}_{4}}\] required to oxidize one mole of \[Fe({{C}_{2}}{{O}_{4}})\] in acidic medium is
  A)
  0.167    done clear
  B)
  0.6     done clear
  C)
  0.2                    done clear
  D)
  0.4 done clear
  View Solution play_arrow

• question_answer56)
  Haemoglobin contains 0.33% of iron by weight. The molecular weight of haemoglobin is approximately 67200. The number of iron atoms (at. wt. of Fe =56) present in one molecule of haemoglobin is
  A)
  6          done clear
  B)
  1       done clear
  C)
  2                                  done clear
  D)
  4 done clear
  View Solution play_arrow

• question_answer57)
  A 25.0 mm \[\times \] 40.0 mm piece of gold foil is 0.25 mm thick. The density of gold is \[19.32\,g\text{/}c{{m}^{3}}\]. How many gold atoms are in the sheet? (Atomic weight: Au = 197.0)  
  A)
  \[7.7\times {{10}^{23}}\]        done clear
  B)
  \[~1.5\times {{10}^{23}}\] done clear
  C)
  \[4.3\times {{10}^{21}}\]          done clear
  D)
  \[1.47\times {{10}^{22}}\] done clear
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• question_answer58)
  What volume of oxygen gas \[({{O}_{2}})\] measured at \[0{}^\circ C\] and 1 atm, is needed to burn completely 1L of propane gas\[({{C}_{3}}{{H}_{8}})\] measured under the same conditions?
  A)
  7L                    done clear
  B)
  6L   done clear
  C)
  5L        done clear
  D)
  10L done clear
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• question_answer59)
  25.4 g of \[{{I}_{2}}\] and 14.2 g of \[C{{l}_{2}}\] are made to react completely to yield a mixture of \[ICl\] and \[IC{{l}_{3}}\] Calculate moles of \[ICl\] and\[IC{{l}_{3}}\] formed
  A)
  0.1, 0.1    done clear
  B)
  0.2, 0.2 done clear
  C)
  0.1, 0.2              done clear
  D)
  0.2, 0.1 done clear
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• question_answer60)
  10 moles \[S{{O}_{2}}\] and 15 moles \[{{O}_{2}}\] were allowed to react over a suitable catalyst. 8 moles of \[S{{O}_{3}}\] were formed. The remaining moles of \[S{{O}_{2}}\] and \[{{O}_{2}}\]  respectively are-
  A)
  2 moles, 11 moles done clear
  B)
  2 moles, 8 moles done clear
  C)
  4 moles, 5 moles             done clear
  D)
  8 moles, 2 moles done clear
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• question_answer61)
  In the reaction \[4N{{H}_{3}}\left( g \right)+502\left( g \right)\xrightarrow{{}}4NO\left( g \right)+6H2O\left( l \right)\] when 1 mole of ammonia and 1 mole of \[{{O}_{2}}\] are made to react to completion
  A)
  1.0 mole of \[{{H}_{2}}O\] is produced done clear
  B)
  1.0 mole of NO will be produced done clear
  C)
  all the ammonia will be consumed done clear
  D)
  all the oxygen will be consumed done clear
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• question_answer62)
  An ideal gaseous mixture of ethane \[({{C}_{2}}{{H}_{5}})\] and ethene \[({{C}_{2}}{{H}_{4}})\] occupies 28 litre at 1 atm and 273 K. The mixture reacts completely with 128 g \[{{O}_{2}}\] to produce \[C{{O}_{2}}\] and \[{{H}_{2}}O\]. Mole fraction at \[{{C}_{2}}{{H}_{6}}\] in the mixture is: 
  A)
  0.6     done clear
  B)
  0.4     done clear
  C)
  0.5                    done clear
  D)
  0.8 done clear
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• question_answer63)

  Wood's metal contains 50.0% bismuth, 25.0% lead, 12.5% tin and 12.5% cadmium by mass. What is the mole fraction of tin?

  (Atomic mass: Bi=209, Pb=207, Sn= 199, Cd= 112)

  A)
  0.202                done clear
  B)
  0.158 done clear
  C)
  0.176 done clear
  D)
  0.221 done clear
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• question_answer64)
  The mass of \[BaC{{O}_{3}}\]produced when excess \[C{{O}_{2}}\] is bubbled through a solution of 0.205 mol \[Ba{{\left( OH \right)}_{2}}\]is:
  A)
  81 g                              done clear
  B)
  40.5 g done clear
  C)
  20.25 g              done clear
  D)
  162 g done clear
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• question_answer65)
  Sulfuryl chloride \[(S{{O}_{2}}C{{l}_{2}})\] reacts with water to give a mixture of \[{{H}_{2}}S{{O}_{4}}\] and HCl. How many moles of baryta would be required to neutralize the solution formed by adding 4 mole of \[S{{O}_{2}}C{{l}_{2}}\] to excess of water?
  A)
  1                      done clear
  B)
  2      done clear
  C)
  3                                  done clear
  D)
  4 done clear
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• question_answer66)
  1 g mixture of equal number of mole of \[L{{i}_{2}}C{{O}_{3}}\] and other metal carbonate \[({{M}_{2}}C{{O}_{3}})\] required 21.6 mL of \[0.5\text{ }N\text{ }HCl\] for complete neutralization reaction. What is the approximate atomic mass of the other metal?        
  A)
  25                     done clear
  B)
  23    done clear
  C)
  51                                 done clear
  D)
  118 done clear
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• question_answer67)
  When 2.5 g of a. sample of Mohr's salt reacts N completely with 50 mL of \[\frac{N}{10}KMn{{O}_{4}}\] solution. The % purity of the sample of Mohr's salt is:
  A)
  78.4      done clear
  B)
  70    done clear
  C)
  37                                 done clear
  D)
  40 done clear
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• question_answer68)
  If potassium chlorate is 80% pure, then 48 g of oxygen would be produced from (atomic mass of K=39)
  A)
  153.12 g of \[KCl{{O}_{3}}\]     done clear
  B)
  122.5 g of \[KCl{{O}_{3}}\] done clear
  C)
  245 g of\[KCl{{O}_{3}}\]   done clear
  D)
  98 g of \[KCl{{O}_{3}}\] done clear
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• question_answer69)
  12 g of Mg (atomic mass 24) will react completely with hydrochloric acid to give
  A)
  One mol of \[{{H}_{2}}\] done clear
  B)
  1/2 mol of \[{{H}_{2}}\] done clear
  C)
  2/3 mol of \[{{O}_{2}}\] done clear
  D)
  both 1/2 mol of\[{{H}_{2}}\] and 1/2 mol of \[{{O}_{2}}\] done clear
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• question_answer70)
  2.76 g of silver carbonate (at mass of Ag 108) on being heated strongly yield a residue weighing
  A)
  2.16 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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