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The quiz is designed for Stoichiometry chapter for JEE Main level.
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Question 1 of 21
1. Question
4 pointsA 10.0 g sample of a mixture of calcium chloride and sodium chloride is treated with Na2CO3 to precipitate the calcium as calcium carbonate. This calcium carbonate is heated to convert all the calcium to calcium oxide and the final mass of calcium oxide is 1.62 gm. The percentage by mass of calcium chloride in the original mixture is
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Question 2 of 21
2. Question
4 pointsA sample of Oleum is labeled 104.5%. The % of free SO3 in the sample is
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Question 3 of 21
3. Question
4 points125 ml of Na2CO3 solution requires 100 ml of 0.1 N HCl to reach end point with Phenolphthalein as indicator. Molarity of resulting solution with respect to HCO3– ion is
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Question 4 of 21
4. Question
4 pointsThe equivalent weight of HCl in the given reaction is
K2Cr2O7 + 14 HCl → 2 KCl + 2 CrCl3 + 3 Cl2 + H2O
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Question 5 of 21
5. Question
4 pointsAn aqueous solution of 6.3g of oxalic acid dihydrate is made upto 250 ml. The volume of 0.1 N NaOH required to completely neutralize 10 ml of this solution is
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Question 6 of 21
6. Question
4 pointsHow many mole of Fe2+ ions are formed, when excess of iron is treated with 50 ml of 4 M HCl under inert atmosphere assuming no change in volume
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Question 7 of 21
7. Question
4 pointsThe molarity of NO3– in the solution after 2 litres of 3M AgNO3 is mixed with 3 litres of 1M BaCl2 is :
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Question 8 of 21
8. Question
4 points1 litre solution of N/2 HCl is heated in a beaker. It was observed that when the volume of solution reduced to 600 ml, 3.25g of HCl is lost. Calculate the normality of the new solution.
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Question 9 of 21
9. Question
4 pointsNormality of 10% (weight / volume) acetic acid would be
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Question 10 of 21
10. Question
4 pointsThe solution A and B are 0.1 and 0.2 molar in a substance. If 100 ml of A are mixed with 25 ml of B and there is no change in volume, then the final molarity of the solution is
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Question 11 of 21
11. Question
4 pointsSO2Cl2 + 2H2O → H2SO4 + 2HCl, If 100 gm SO2Cl2 completely reacts with water then to neutralize this resultant solution how much solid KOH should be added into the solution? [At. Mass of S = 32, K=39]
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Question 12 of 21
12. Question
4 pointsFeS2 + O2 → Fe2O3 + SO2, Equivalent wt. of FeS2 in this reaction is [at. Wt. of Fe = 56]
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Question 13 of 21
13. Question
4 points20 ml 0.1m KI solution is completely oxidized by 0.03 M barium permanganate solution in acidic medium. The volume of permanganate required is
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Question 14 of 21
14. Question
4 pointsThe simplest molecular formula of a metal oxide containing 23% oxygen would be [Atomic weight of the metal is 80.35]
(a) MO2 (b) M2O (c) MO (d) M2O3
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Question 15 of 21
15. Question
4 pointsWhen ferricyanide reacts with H2O2 in alkaline medium then the molar ratio of [Fe(CN)6]-3 and H2O2 is
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Question 16 of 21
16. Question
4 pointsHow many moles of acidified FeSO4 can be completely oxidized by one mole of KMnO4 ?
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Question 17 of 21
17. Question
4 points10 grams of CaCO3 is completely decomposed to X and CaO. X is passed into an aqueous solution containing one mole of sodium carbonate. What is the number of moles of sodium bicarbonate formed (Mol. wt.: CaCO3 = 100, Na2CO3 = 106, NaHCO3 = 84)
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Question 18 of 21
18. Question
4 points2 gram of sulphur is completely burnt in oxygen to form SO2. In this reaction what is the volume of O2 consumed at STP in litres ?
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Question 19 of 21
19. Question
4 pointsIf 0.5 mol of BaCl2 is mixed with 0.2 mol of Na3PO4, then maximum number of moles of Ba3(PO4)2 that can be formed is
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Question 20 of 21
20. Question
4 pointsThe equivalent mass of MnSO4 is half of its molecular mass when it is converted to
(A) Mn2SO3 (B) MnO2
(C) MnO4– (D) MnO42–Correct
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Question 21 of 21
21. Question
4 pointsAssuming full decomposition, the volume of CO2 released at STP on heating 9.85g of BaCO3 (At. mass Ba = 137) will be
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