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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
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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
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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
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B)
\[1.568\times {{10}^{4}}\] done
clear
C)
15.68 done
clear
D)
\[3.136\times {{10}^{4}}\] done
clear
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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
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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
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B)
2.24L done
clear
C)
4.06L done
clear
D)
0.84L done
clear
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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
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B)
\[6.023\times {{10}^{19}}\] done
clear
C)
\[4.84\times {{10}^{17}}\] done
clear
D)
\[6.023\times {{10}^{23}}\] done
clear
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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
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B)
1.77 done
clear
C)
1.44 done
clear
D)
none of these done
clear
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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
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B)
47.125 done
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C)
94.25 done
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D)
88.2 done
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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
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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
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B)
\[2.00\text{ }M\] done
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C)
\[2.50\text{ }M\] done
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D)
\[4.00\text{ }M\] done
clear
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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
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B)
48 done
clear
C)
62 done
clear
D)
72 done
clear
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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
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B)
\[0.5\times {{10}^{-3}}\] done
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C)
\[1.66\times {{10}^{-3}}\] done
clear
D)
\[9.95\times {{10}^{-2}}\] done
clear
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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
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B)
\[12.04\times {{10}^{23}}\] done
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C)
\[18.06\times {{10}^{23}}\] done
clear
D)
\[24.08\times {{10}^{22}}\] done
clear
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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
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C)
2.79 m done
clear
D)
3.00 m done
clear
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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
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C)
113.90 done
clear
D)
114.90 done
clear
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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
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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
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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
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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
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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
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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
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B)
0.21 mole done
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C)
2.10 mole done
clear
D)
0.186 mole done
clear
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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
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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
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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
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B)
1 : 2 done
clear
C)
3 : 4 done
clear
D)
4 : 1 done
clear
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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
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C)
84.6 done
clear
D)
None of these done
clear
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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
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B)
1000 done
clear
C)
250 done
clear
D)
200 done
clear
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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
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B)
1.50M done
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C)
1.34M done
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D)
2.70 M done
clear
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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
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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
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B)
86 g done
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C)
129 g done
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D)
172 g done
clear
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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
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B)
85% done
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C)
75% done
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D)
65% done
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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
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C)
147.7 mL done
clear
D)
14.77 mL done
clear
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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
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B)
5.6 g done
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C)
8.09 g done
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D)
6.6 g done
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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
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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
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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
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B)
\[{{N}_{3}}H\] done
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C)
\[N{{H}_{3}}\] done
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D)
\[{{N}_{2}}{{H}_{4}}\] done
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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
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B)
\[{{C}_{7}}{{H}_{10}}N\] done
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C)
\[{{C}_{5}}{{H}_{6}}{{N}_{3}}\] done
clear
D)
\[{{C}_{4}}{{H}_{18}}{{N}_{3}}\] done
clear
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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
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B)
\[VO\] done
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C)
\[{{V}_{2}}{{O}_{5}}\] done
clear
D)
\[{{V}_{2}}{{O}_{7}}\] done
clear
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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
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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
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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
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B)
0.5 done
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C)
0.40 done
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D)
0.25 done
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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
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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
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B)
\[MC{{l}_{2}}\] done
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C)
\[MC{{l}_{4}}\] done
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D)
\[MC{{l}_{5}}\] done
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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
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B)
1N done
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C)
3N done
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D)
4N done
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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
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C)
0.001 M done
clear
D)
\[{{10}^{-4}}M\] done
clear
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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
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B)
12.38 g done
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C)
1.23 g done
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D)
34.76 g done
clear
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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
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B)
41.2 done
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C)
82.4 done
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D)
156.0 done
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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
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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
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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
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B)
20% done
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C)
40% done
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D)
60% done
clear
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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
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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
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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
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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
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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
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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
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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
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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
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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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