CHEMISTRY-04-06- 11th (PQRS) Space

REVIEW TEST-1 Class : XI Time : 90 min Max. Marks : 75 General Remarks: INSTRUCTIONS 1. The question paper contain two parts. Part-A contains short question and Part-B contains subjective questions. All questions are compulsory. Paper contains 10 questions in Part-A and 9 questions in Part-B. 2. You are advised NOT to spend more than 30 minutes in any case for part-A. 3. Each question should be done only in the space provided for it, otherwise the solution will not be checked. 4. Use of Calculator, Log table and Mobile is not permitted. 5. Legibility and clarity in answering the question will be appreciated. 6. Put a cross ( × ) on the rough work done by you. Name : Roll No. Batch Class : XI Invigilator's Full Name USEFUL DATA Atomic weights: Al = 27, Mg = 24, Cu = 63.5, Mn = 55, Cl = 35.5, O = 16, H = 1, P = 31, Ag = 108, N = 14, Li = 7, I = 127, Cr = 52, K=39, S = 32, Na = 23, C = 12, Br = 80, Fe = 56, Ca = 40, Zn = 65.4, Ti = 48, Ba = 137, R = 0.082 (lt-atm)/(K-mol) For Office Use ……………………………. Total Marks Obtained………………… Part-A Part-B Q.No 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 Marks PART A Q.1 Rearrange the following (I to IV) in the order of increasing masses [3] (I) 0.5 mole of O3 (II) 0.5 gm-molecule of N2 (III) 3.011 × 1023 molecules of O2 (IV) 5.6 litre of CO2 at STP Q.2 Calculate number of neutrons in 17 g of H2O2. [3] Q.3 The hydrated salt Na2CO3.xH2O undergoes 63% loss in mass on heating and becomes anhydrous, calculate the value of x [3] Q.4 The vapour density of a mixture containing NO2 & N2O4 is 27.6. Calculate mole fraction of N2O4 in the mixture. [3] Q.5 Suppose two elements X and Y combine to form two compounds XY2 and X3Y2 when 0.05 mole of XY2 weighs 5 g while 3.011 × 1023 molecules of X3Y2 weighs 90 g. Calculate the atomic masses of X and Y. [3] Q.6 What is the molarity of SO2 ion in aqueous solution that contain 34.2 ppm of Al (SO ) [Assume 4 2 4 3 complete dissociation & density of solution 1 g/ml] [3] Q.7 Concentration of aq. NaOH solution is 3.0 Molal and it's density is 1.1 gm/ml. What is the Molarity of the solution? [3] Q.8 What volume of 90% alcohol by weight (d = 0.80 g/cm3) must be used to prepare 150 cm3 of 30% alcohol by weight (d = 0.90 g/cm3) [3] Q.9 1.44 gram of Titanium (Ti) reacted with excess of O2 and produced x gram of compound Ti1.44O. Find the value of x. [3] PART B Q.10 (i) Find the value of x in Nicotine, C10H14Nx? (Given: mol. mass of Nicotine is 162 amu.) (ii) If an atom of 12C had been assigned a relative value of 24.0 a.m.u., what would be the atomic weight of hydrogen relative to this mass. [2 + 2] Q.11 (i) How many millilitres of a 0.45 M BaCl2 aq. solution contain 15.0 g of BaCl2? (ii) Consider the balanced equation for the formation of 1 mole of Fe2(CO3)3 2Fe(NO3)3 + 3Na2CO3  Fe2(CO3)3 + 6NaNO3 How many oxygen atoms are on each side of the equation? [2 + 2] Q.12 An aq. solution of H2SO4 contain 196 g acid per litre; solution has density 1.24 g/ml. Calculate (i) wt % of H2SO4 in solution (ii) mole % of H2SO4 in solution [4] Q.13(i) In the decomposition of impure KClO3 9.8 g of it gave 1.49 g of KCl and 0.03 mol of O2 gas. Calculate percent purity of KClO3 with the help of law of conservation of mass. (ii) Phosphorus (V) chloride reacts with water to give phosphoric acid and hydrogen chloride according to the following equation (not balanced) PCl5 + H2O  H3PO4 + HCl In an experiment 0.36 mole of PCl5 was reacted to 2.88 mole of water (a) Which reactant was the limiting reagent. (b) Calculate the theoretical yields (in moles) of H3PO4 and HCl. [2+3] Q.14 A mixture of NH4NO3 & (NH4)2HPO4 showed the mass percent of nitrogen to be 30.40%. What is the mass ratio of the two components in the mixture? [5] Q.15 In the preparation of iron from haematite (Fe2O3) by the reaction with carbon Fe2O3 + C  Fe + CO2 (a) Balance the equation (b) How much 80% pure iron could be produced from 120 kg of 90% pure Fe2O3 [5] Q.16(i) The actual mass of the atomic mass unit is 1.66 × 10–24 g using this value, calculate the mass in grams of 10 atoms of 12C. (ii) A gaseous compound is composed of 85.7% by mass carbon and 14.3% by mass hydrogen. It's density is 2.28 g/litre at 300K and 1.0 atm pressure. Determine the molecular formula of the compound. [2+4] M Q.17(i) Calculate volume of water to be added to 300 ml of 5 M 15 . HNO3 solution so that its new strength becomes (ii) It is known that when 1 mole of carbon reacted with 1 mole of oxygen (C + O2  CO2), 1 95 Kcal heat liberated & when 1 mole carbon reacted with 0.5 mole of O2 (C + 2 O2  CO), 24 Kcal heat liberated. When 12.0 g of carbon reacted with oxygen to form CO & CO2, 80.8 Kcal of heat liberated and no carbon remained. Calculate the mass of oxygen which reacted. [2 + 4] Q.18 8KI + 5H2SO4 100%yield 4K2SO4 + 4I2 + H2S + 4H2O H2SO4 + 2NaOH 100%yield  Na2SO4 + 2H2O I2 + 2Na2S2O3 50%yield 2NaI + Na2S4O6 50% yield I2 + 2KCl  2KI + Cl 100 ml of a sample of dilute H2SO4 of specific gravity 1.47 is treated with a 10 g sample of impure KI. The final mixture had to be treated with 20 ml of 4% (w/V) NaOH solution to neutralize left H2SO4. Iodine liberated was trapped and divided into two parts. One part on passing through 20 ml. Na2S2O3 solution yielded 0.3 g of NaI and the other part of I2 sample on treatment with excess KCl yielded 0.497 g of Cl2.Calculate, (i) molarity of Na2S2O3 solution. (ii) % (w/W) of H2SO4 sample (iii) % purity of KI sample [3+3+3] ROUGH WORK

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