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  Question 1.  A mixture of carbon monoxide and carbon dioxide is found to have a density of 1.7 g/lit at STP. The mole fraction of carbonmonoxide is : [A]  0.37 [B]  0.40 [C]  0.30 [D]  0.50 Question 2. Consider the reaction, Where gases X and Y are insoluble and inert to water and Z form a basic solution. In an experiment 3 mole each of X and Y areallowed to react in 15 lit flask at 500 K. When the reaction is complete, 5L of water is added to the flask and temperature is reducedto 300 K. The pressure in the flask is : (neglect aqueous tension) [A]  1.64 atm [B]  2.46 atm [C]  4.92 atm [D]  3.28 atm Question 3.  A proton accelerated from rest through a potential difference of 'V' volts has a wavelength associated with it. An alpha particle inorder to have the same wavelength must be accelerated from rest through a potential difference of : [A]  V volt [B]  4V volt [C]  2V volt [D]  volt Question 4.  At 1400 K, for the reaction . A 10.0 L reaction vesselat 1400 K contains 2.00 mole of CH 4 , 3.0 mol of CS 2 , 3.0 mole of H 2  and 4.0 mole of H 2 S. Then : [A]  This reaction is at equilibrium with above concentrations [B]  The reaction will proceed in forward direction to reach equilibrium [C]  The reaction will proceed in backward direction to reach equilibrium [D]  The information is insufficient to decide the direction of progress of reaction Question 5. The value of k p  for the reaction at is '1 atm'. At equilibrium in a closed container partial pressure of BrCl gas is 0.1 atm and at this temperature the vapour pressure of Br  2 is also 0.1 atm. Then what will be minimum moles of Br  2  to be added to 1 mole of Cl 2 , initially, to get above equilibriumsituation : [A]  moles [B]  moles [C]  moles [D]  2 moles Question 6.  An acid-base indicator which is a weak acid has a pK a  value = 5.45. At what concentration ratio of sodium acetate to acetic acidwould be indicator show a colour half-way between those of its acid and conjugate base forms ? pK a  of acetic acid = 4.75. [log 2 =0.3] [A]  4 : 1 [B]  7 : 1 [C]  5 : 1 [D]  2 : 1  Question 7. Equal volume of two solution having pH = 2 and pH = 10 are mixed together at . Then pH of resulting solution is : (Take K w  at ) [A]  2 + log 2 [B][C]  7 [D]  6 Question 8. Which of the following has been arranged in correct order of decreasing freezing point ? [A]  0.05 M KNO 3  > 0.04 M CaCl 2  > 0.140 M sugar > 0.075 M CuSO 4 [B]  0.04 M BaCl 2  > 0.140 M sucrose > 0.075 M CuSO 4  > 0.05 M KNO 3 [C]  0.075 M CuSO 4  > 0.140 M sucrose > 0.04 M BaCl 2  > 0.05 M KNO 3 [D]  0.075 M CuSO 4  > 0.05 M NaNO 3  > 0.140 M sucrose > 0.04 M BaCl 2 Question 9.  An ideal mixture of liquids A and B with 2 moles of A and 2 moles of B has a total vapour pressure of 1 atm at a certain temperature. Another mixture with 1 mole of A and 3 moles of B has a vapour pressure greater than 1 atm. But if 4 moles of C are added to thesecond mixture, the vapour pressure comes down to 1 atm. Vapour pressure of C, . Calculate the vapour pressures of pure A and pure B. [A][B][C][D]Question 10. Identify the true and false statement and answer in given options : I. During electrolysis of 1 M NaCl solution Cl 2  does not form at the anode. II. For a concentration cell with its reaction at equilibrium both and are zero. III.  In a solution of HCN the concentration of ions is given by . [A]  FTF [B]  TTT [C]  FFF [D]  FTT Question 11.  Acetic acid is titrated with NaOH solution. Which of the following statement is correct for this titration? [A]  Conductance increases upto equivalence point, then it decreases [B]  Conductance decreases upto equivalence point, then it increases [C]  First conductance increases slowly upto equivalence point and then increases rapidly [D]  First conductance increases slowly upto equivalence point and then drops rapidly Question 12. What is the value of if and for 0.04 of a CH 3 COOH at : [A]  10.3 [B]  9.2 [C]  4.7 [D]  4.8 Question 13.Statement 1 :  In electrochemical cell, we cannot use KCl in the salt bridge if anodic or cathodic compartment consists of Ag +  or Pb 2+  ion. Statement 2 :  Salt bridge is employed to maintain the electrical neutrality and to minimize the liquid-liquid junction potential. [A]  Statement-1 is True, Statement-2 is True and Statement-2 is a correct explanation for Statement-1 [B]  Statement-1 is True, Statement-2 is True and Statement-2 is NOT a correct explanation for Statement-1  [C]  Statement-1 is True, Statement-2 is False [D]  Statement-1 is False, Statement-2 is True Question 14. Consider the reaction at 300 K If 3 mole of H 2  completely react with 3 mole of Cl 2  to form HCl, of the reaction will be : [A]  Zero [B][C]  555 kJ [D]  None of these Question 15.Statement 1 :  The amount of work done in the isothermal expansion is greater than work done in the adiabatic process for samefinal volume. Statement 2 :  In the adiabatic expansion of a gas temperature and pressure both decrease due to increase in internal energy of the system. [A]  Statement-1 is True, Statement-2 is True and Statement-2 is a correct explanation for Statement-1 [B]  Statement-1 is True, Statement-2 is True and Statement-2 is NOT a correct explanation for Statement-1 [C]  Statement-1 is True, Statement-2 is False [D]  Statement-1 is False, Statement-2 is True Question 16. For which process will and be expected to be most similar. [A][B][C][D]Question 17.  A crystal is made of particle X, Y and Z. X forms FCC packing, Y occupies all octahedral voids of X and Z occupies all tetrahedralvoids of X, if all the particles along one body diagonal are removed then the formula of the crystal would be : [A][B][C][D]Question 18.Statement 1 :  The ratio of Zn 2+  and per unit cell of ZnS and CaF 2  is 1 : 2. Statement 2 :  In ZnS, Zn 2+  ions occupy alternate tetrahedral voids and in CaF 2 , ions occupy all the tehrahedral voids of FCCunit cell. [A]  Statement-1 is True, Statement-2 is True and Statement-2 is a correct explanation for Statement-1 [B]  Statement-1 is True, Statement-2 is True and Statement-2 is NOT a correct explanation for Statement-1 [C]  Statement-1 is True, Statement-2 is False [D]  Statement-1 is False, Statement-2 is True Question 19.  At a certain temperature, the first order rate constant k  1  is found to be smaller than the second order rate constant k  2 . If the energyof activation E 1  of the first order reaction is greater than energy of activation E 2  of the second order reaction, then with increase intemperature. [A]  k  1  will increase faster than k  2 , but always will remain less than k  2 [B]  k  2  will increase faster than k  1 [C]  k  1  will increase faster than k  2 , and becomes equal to k  2 [D]  k  1  will increase faster k  2  and becomes greater than k  2 Question 20.  The activity per ml of a solution of radioactive substance is  x  . How much water be added to 200 ml of this solution so that the activityfalls to x/20 per ml after 4 half-lives ? [A]  100 ml [B]  150 ml [C]  80 ml [D]  50 ml Question 21. What type of crystal defect is indicated in the diagram below ? [A]  Frenkel defect [B]  Schottky defect [C]  Interstitial defect [D]  Frenkel and Schottky defects Question 22.  At , the vapour pressure of pure liquid 'A' is 520 mm Hg and that of pure liquid 'B' is 1000 mm Hg. If a mixture solution of 'A'and 'B' boils at and 1 atm pressure, the amount of 'A' in the mixture is : (1 atm = 760 mm Hg) [A]  52 mole per cent [B]  34 mole per cent [C]  48 mole per cent [D]  50 mole per cent Question 23. If is the degree of dissociation of Na 2 SO 4 , the van't Hoff factor ( i   ) used for calculating the molecular mass is : [A][B][C][D]Question 24. t 1/4  can be taken as the time taken for the concentration of a reactant to drop to 3/4 of its initial value. If the rate constant for a firstorder reaction is k  , the t 1/4  can be written as : [A]  0.75/k [B]  0.69/k [C]  0.29/k [D]  0.10/k Question 25.  A schematic plot of ln K eq  versus inverse of temperature for a reaction is shown below :The reaction must be : [A]  Highly spontaneous at ordinary temperature [B]  One with negligible enthalpy change
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