JEE Main & Advanced Chemistry Thermodynamics / रासायनिक उष्मागतिकी Sample Paper

done Topic Test - Thermo Chemistry (Thermodynamics) Total Questions - 35    [Download]

• question_answer1)
  Which of the following is not the extensive property?
  A)
  Gibbs free energy
  done clear
  B)
  Enthalpy
  done clear
  C)
  Entropy
  done clear
  D)
  Viscosity
  done clear
  View Answer play_arrow

• question_answer2)

  If (i) \[\Delta H_{f}^{o}\] (benzene)\[=-358.5\,\,kJ\,\,mo{{l}^{-1}}\].

  (ii) Heat of atomization of graphite\[=716.8\,\,kJ\,mo{{l}^{-1}}\].

  (iii) Bond energy of \[C-H,\,\,C-C,\,\,C=C\] and \[H-H\] bonds are 490, 340, 620 and\[436.9\,\,kJ\,\,mo{{l}^{-1}}\] respectively. The resonance energy (in \[kJ\,\,mo{{l}^{-1}}\]) of \[{{C}_{6}}{{H}_{6}}\] using Kekule formula is

  A)
  - 150
  done clear
  B)
  - 50
  done clear
  C)
  - 250
  done clear
  D)
  +150
  done clear
  View Answer play_arrow

• question_answer3)
  Which of the following parameter is correct regarding adsorption of gases over solid?
  A)
  \[\Delta {{S}_{system}}>0\]
  done clear
  B)
  \[\Delta {{S}_{surronunding}}>0\]
  done clear
  C)
  \[\Delta G>0\]
  done clear
  D)
  \[\Delta H>0\]
  done clear
  View Answer play_arrow

• question_answer4)
  Which of the following defines enthalpy of solution?
  A)
  \[{{H}_{2}}O(l)\xrightarrow[{}]{{}}{{H}^{+}}(aq)+O{{H}^{-}}(aq)\]
  done clear
  B)
  \[N{{H}_{4}}Cl(s)\xrightarrow[{}]{{}}NH_{4}^{+}(aq)+C{{l}^{-}}(aq)\]
  done clear
  C)
  \[CuS{{O}_{4}}\cdot 5{{H}_{2}}O(s)+{{H}_{2}}O\xrightarrow[{}]{{}}CuS{{O}_{4}}(aq)\]
  done clear
  D)
  \[CuS{{O}_{4}}(s)+5{{H}_{2}}O\xrightarrow[{}]{{}}CuS{{O}_{4}}\cdot 5{{H}_{2}}O(s)\]
  done clear
  View Answer play_arrow

• question_answer5)
  The tendency of a reaction to take place spontaneously is greatest when the reaction is
  A)
  Exothermic and randomness increases
  done clear
  B)
  Endothermic & randomness increases
  done clear
  C)
  Exothermic and randomness decreases
  done clear
  D)
  Endothermic & randomness decreases
  done clear
  View Answer play_arrow

• question_answer6)
  Which of the following reactions corresponds to the definition of enthalphy of formation?
  A)
  C (diamond) \[+{{O}_{2}}(g)\to C{{O}_{2}}(g)\]
  done clear
  B)
  C (graphite) \[+{{O}_{2}}(l)\to C{{O}_{2}}(g)\]
  done clear
  C)
  C (graphite) \[+{{O}_{2}}(g)\to C{{O}_{2}}(g)\]
  done clear
  D)
  \[C(g)+{{O}_{2}}(g)\to C{{O}_{2}}(g)\]
  done clear
  View Answer play_arrow

• question_answer7)
  Which of the following combustion reactions would give maximum energy output per unit mass fuel plus oxidant when used to propel a rocket?
  A)
  \[C(s)+{{O}_{2}}\xrightarrow{{}}C{{O}_{2}}(g),\,\,\Delta H=-394\,KJ/mol\]
  done clear
  B)
  \[{{H}_{2}}(g)+\frac{1}{2}{{O}_{2}}\xrightarrow{{}}{{H}_{2}}O(l),\,\Delta H=-285\,kJ/mol\]
  done clear
  C)
  \[\frac{1}{2}{{H}_{2}}+\frac{1}{2}{{F}_{2}}\xrightarrow{{}}2HF(g),\,\Delta H=-271\,kJ/mol\]
  done clear
  D)
  \[C{{H}_{4}}+2{{O}_{2}}\xrightarrow{{}}C{{O}_{2}}(g)+2{{H}_{2}}O(l),\]\[\Delta H=-890\,kJ/mol\]
  done clear
  View Answer play_arrow

• question_answer8)
  A 1 g sample of octane \[{{C}_{8}}{{H}_{18}}\] is burned in excess of oxygen in a bomb calorimeter. The temperature of the calorimeter rises from 294 K to 300 K. If heat capacity of the calorimeter is 8 kJ/K, the enthalpy of combustion of octane is
  A)
  5472 kJ/mol      
  done clear
  B)
  48 kJ/mol
  done clear
  C)
  684 kJ/mol
  done clear
  D)
  4281 kJ/mol
  done clear
  View Answer play_arrow

• question_answer9)
  The polymerization of ethylene to linear polyethylene is represented by the reaction \[nC{{H}_{2}}=C{{H}_{2}}\xrightarrow{\,}\,{{(-C{{H}_{2}}-C{{H}_{2}}-)}_{n}}\] when 'n' has a large integral value. Given that average enthalpies of bond dissociation for \[C=C\] and \[C-C\] at 298 K are + 590 and \[+331\,\,kJ\,\,mo{{l}^{-1}}\] respectively. Then the enthalpy of polymerization/mol of ethylene at298 K is
  A)
  - 132 kJ
  done clear
  B)
  - 72 kJ
  done clear
  C)
  + 80 kJ
  done clear
  D)
  + 162 kJ
  done clear
  View Answer play_arrow

• question_answer10)
  Select the incorrect option about spontaneous exothermic reaction.
  A)
  \[\Delta {{S}_{surr}}=+ve\]
  done clear
  B)
  \[\Delta {{S}_{Overall}}=+ve\]
  done clear
  C)
  \[\Delta {{S}_{System}}may=-ve\]
  done clear
  D)
  \[\Delta {{S}_{System}}=+ve\,\,\text{always}\]
  done clear
  View Answer play_arrow

• question_answer11)
  The standard heat of combustion of Al is \[-\,837.8\,kJ\,mo{{l}^{-1}}\] at \[{{25}^{o}}C\]. If Al reacts with \[{{O}_{2}}\] at \[{{25}^{o}}C,\] which of the following releases 250 kcal of heat?
  A)
  The reaction of 0.624 mole of Al
  done clear
  B)
  The formation of 0.624 mole of \[A{{l}_{2}}{{O}_{3}}\]
  done clear
  C)
  The reaction of 0.312 mole of Al
  done clear
  D)
  The formation of 0.150 mole of \[A{{l}_{2}}{{O}_{3}}\]
  done clear
  View Answer play_arrow

• question_answer12)
  The heat of hydration of solution anhydrous \[CuS{{O}_{4}}\] and hydrated \[CuS{{O}_{4}}\cdot 5{{H}_{2}}O\] are - 66.5 and 11.7 kJ \[mo{{l}^{-1}}\]respectively. Calculate the heat of hydration of \[CuS{{O}_{4}}\] to \[CuS{{O}_{4}}\cdot 5{{H}_{2}}O\]
  A)
  - 78.2 kJ
  done clear
  B)
  - 81.2 kJ
  done clear
  C)
  - 68.2 kJ
  done clear
  D)
  - 60.1 kJ
  done clear
  View Answer play_arrow

• question_answer13)
  State which of the following statements is true?
  A)
  First law of thermodynamics is not adequate in predicting the direction of the process.
  done clear
  B)
  In an exothermic reaction, the total enthalpy of the products is greater than that of reactants.
  done clear
  C)
  The standard enthalpy of diamond is zero at 298K and 1 atm pressure.
  done clear
  D)
  It is possible to calculate the value of \[\Delta H\] for the reaction \[{{H}_{2}}(g)+B{{r}_{2}}(\ell )\to 2HBr(g)\] from the bond enthalpy data.
  done clear
  View Answer play_arrow

• question_answer14)
  In an adiabatic process non-transfer of heat takes place between system and surroundings. Choose the correct option for free expansion of an ideal gas under adiabatic condition from the following.
  A)
  \[q=0,\Delta T,w=0\]
  done clear
  B)
  \[q\ne 0,\Delta T=0,w=0\]
  done clear
  C)
  \[q=0,\Delta T=0,w=0\]
  done clear
  D)
  \[q=0,\Delta t<0,w\ne 0\]
  done clear
  View Answer play_arrow

• question_answer15)

  For a gaseous reaction:

  \[2{{A}_{2}}(g)+5{{B}_{2}}(g)\to 2{{A}_{2}}{{B}_{5}}(g)\] at \[{{27}^{o}}C\]

  the heat change at constant pressure is found to be \[-\,50160\,J\]. Calculate the value of internal energy change \[(\Delta E)\]. Given that R = 8.314 J/K mol.

  A)
  - 34689 J
  done clear
  B)
  - 37689 J
  done clear
  C)
  - 27689 J
  done clear
  D)
  - 38689 J
  done clear
  View Answer play_arrow

• question_answer16)
  The gaseous endothermic reaction :  \[P+Q\to 3R\] at \[327{}^\circ C\] takes place spontaneously, because-
  A)
  \[\Delta H<0;\,\Delta S<0\]
  done clear
  B)
  \[\Delta H>0;\,\Delta S>0\]
  done clear
  C)
  \[\Delta H<0;\,\Delta S>0\]
  done clear
  D)
  \[\Delta H>0;\,\Delta S<0\]
  done clear
  View Answer play_arrow

• question_answer17)
  The difference between the heats of reaction at constant pressure and a constant volume for the reaction \[2{{C}_{6}}{{H}_{6\left( 1 \right)}}+15{{O}_{2(g)}}\xrightarrow{{}}12C{{O}_{2(g)}}+6{{H}_{2}}{{O}_{(I)}}\] in Kj is :
  A)
  - 7.43
  done clear
  B)
  + 3.72
  done clear
  C)
  - 3.72
  done clear
  D)
  + 7.43
  done clear
  View Answer play_arrow

• question_answer18)
  The enthalpy of combustion of \[{{H}_{2}}(g),\] to give\[{{H}_{2}}(g)\] is \[-249\text{ }kJ\text{ }mo{{l}^{-1}}\] and bond enthalpies of \[H-H\] and \[O=O\] are \[433\text{ }kJ\text{ }mo{{l}^{-1}}\] and \[492\text{ }kJ\text{ }mo{{l}^{-1}}\] respectively. The bond enthalpy of \[O-H\] is
  A)
  \[464\text{ }kJ\text{ }mo{{l}^{-1}}\]
  done clear
  B)
  \[-464\text{ }kJ\text{ }mo{{l}^{-1}}\]
  done clear
  C)
  \[232\text{ }kJ\text{ }mo{{l}^{-1}}\]
  done clear
  D)
  \[-232\text{ }kJ\text{ }mo{{l}^{-1}}\]
  done clear
  View Answer play_arrow

• question_answer19)
  Use the bond enthalpies in the table to determine \[\Delta H{}^\circ \] for the formation of hydrazine, \[{{N}_{2}}{{H}_{4}}(g)\] from nitrogen and hydrogen in standard state according to the equation :  \[{{N}_{2}}(g)+2{{H}_{2}}(g)\xrightarrow{{}}{{N}_{2}}{{H}_{4}}(g)\]

  Bond	Bond enthalpies
  \[N-N\]	\[159\text{ }kJ\text{ }mo{{l}^{-1}}\]
  \[N=N\]	\[418\text{ }kJ\text{ }mo{{l}^{-1}}\]
  \[N\equiv N\]	\[941\text{ }kJ\text{ }mo{{l}^{-1}}\]
  \[H-H\]	\[436\text{ }kJ\text{ }mo{{l}^{-1}}\]
  \[H-N\]	\[389\text{ }kJ\text{ }mo{{l}^{-1}}\]

  A)
  \[\Delta H{}^\circ =-425\text{ }kJ\]
  done clear
  B)
  \[\Delta H{}^\circ =-\text{ }98\text{ }kJ\]
  done clear
  C)
  \[\Delta H{}^\circ =+\text{ }98\text{ }kJ\]
  done clear
  D)
  \[\Delta H{}^\circ =+\text{ }711\,kJ\]
  done clear
  View Answer play_arrow

• question_answer20)

  The Solvay process for making \[N{{a}_{2}}C{{O}_{3}}\] involves the reaction

  \[2NaHC{{O}_{3}}N{{a}_{2}}C{{O}_{3}}(s)+{{H}_{2}}O(g)+C{{O}_{2}}(g)\]

  For this reaction \[\Delta {{H}^{o}}=129.2\,kJ/mol,\] \[\Delta {{S}^{o}}=334.2\,J/mol-K\]. From this information, the minimum temperature at which this reaction becomes spontaneous is:

  A)
  \[460{}^\circ C\]
  done clear
  B)
  \[1017{}^\circ C\]
  done clear
  C)
  \[113{}^\circ C\]
  done clear
  D)
  the reaction is spontaneous at all temperatures
  done clear
  View Answer play_arrow

• question_answer21)
  Given the following standard enthalpies of formation, which elements will react exothermically with \[Si{{O}_{2}}(s)\]  to make Si(s)?

  Compounds	\[\Delta H_{f}^{o}kJ/mol\]
  \[Si{{O}_{2}}(s)\]	- 910
  \[MgO(s)\]	- 601
  \[C{{r}_{2}}{{O}_{3}}(s)\]	- 1128
  \[C{{O}_{2}}(g)\]	- 393
  \[L{{i}_{2}}O(s)\]	- 598

  A)
  Cr only
  done clear
  B)
  Mg and Li only
  done clear
  C)
  C, Li and Cr
  done clear
  D)
  Li only
  done clear
  View Answer play_arrow

• question_answer22)
  For an endothermic reaction, where \[\Delta H\] represents the enthalpy of the reaction, the minimum value for the energy of activation will be
  A)
  less than \[\Delta H\]      
  done clear
  B)
  zero
  done clear
  C)
  more than \[\Delta H\]
  done clear
  D)
  equal to \[\Delta H\]
  done clear
  View Answer play_arrow

• question_answer23)
  Consider the following reaction occuring in an automobile engine : \[2{{C}_{8}}{{H}_{18}}(l)+25\,{{O}_{2}}(g)\to 16\,C{{O}_{2}}(g)+18\,{{H}_{2}}O(g)\] of \[\Delta H,\,\Delta S\] and \[\Delta G\] would be:                             
  A)
  - + +
  done clear
  B)
  - - +
  done clear
  C)
  + + -
  done clear
  D)
  - + -
  done clear
  View Answer play_arrow

• question_answer24)
  A coffee cup calorimeter initially contains 125 g of water, at a temperature of \[24.2{}^\circ C\]. 8 g of ammonium nitrate \[(N{{H}_{4}}N{{O}_{3}}),\] also at \[24.2{}^\circ C,\] is added to the water, and the final temperature is \[18.2{}^\circ C\] what is the heat of solution of ammonium nitrate in kJ/mol? The specific heat capacity of the solution is \[4.2\text{ }J/{}^\circ Cg\].
  A)
  33.51 kJ/mol
  done clear
  B)
  39.5 kJ/mol
  done clear
  C)
  32.2 kJ/mol
  done clear
  D)
  37.3 kJ/mol
  done clear
  View Answer play_arrow

• question_answer25)
  Calculate the heat change in the reaction \[4\,N{{H}_{3}}(g)+3{{O}_{2}}(g)\to 2{{N}_{2}}(g)+6{{H}_{2}}O(\ell )\] at 298 K, given that the heats of formation at 298 K  for \[N{{H}_{3}}(g)\] and \[{{H}_{2}}O(\ell )\] are - 46.0 and - 28.60 kJ \[mo{{l}^{-1}}\] respectively.
  A)
  - 1861 kJ
  done clear
  B)
  - 1361 kJ
  done clear
  C)
  - 1261 kJ
  done clear
  D)
  - 1532 kJ
  done clear
  View Answer play_arrow

• question_answer26)

  The in \[{{\Delta }_{f}}H{}^\circ ({{N}_{2}}{{O}_{5}},g)\] kJ/mol on the basis of the following data is -

  \[2NO(g)+{{O}_{2}}(g)\to 2N{{O}_{2}}(g);\]\[{{\Delta }_{r}}H{}^\circ =-114\,kJ/mol\]

  \[4N{{O}_{2}}(g)+{{O}_{2}}(g)\to 2{{N}_{2}}{{O}_{5}}(g);\]\[{{\Delta }_{r}}H{}^\circ =-102.6\,kJ/mol\]

  \[{{\Delta }_{f}}H{}^\circ (NO,g)=90.2kJ/mol\]

  A)
   15.1
  done clear
  B)
  30.2
  done clear
  C)
  - 36.2
  done clear
  D)
  None of these
  done clear
  View Answer play_arrow

• question_answer27)
  Which of the following expressions represents the first law of thermodynamics?
  A)
  \[\Delta E=-q+W\]
  done clear
  B)
  \[\Delta E=q-W\]
  done clear
  C)
  \[\Delta E=q+W\]
  done clear
  D)
  \[\Delta E=-q-W\]
  done clear
  View Answer play_arrow

• question_answer28)
  If heat of dissociation of \[CHC{{l}_{2}}COOH\] is 0.7 kcal/mol, then \[\Delta H\] for the reaction: \[CHC{{l}_{2}}COOH+KOH\to CHC{{l}_{2}}COOK+{{H}_{2}}O\]
  A)
  - 13 kcal
  done clear
  B)
  + 13 kcal    
  done clear
  C)
  - 14.4 kcal 
  done clear
  D)
  - 13.7 kcal
  done clear
  View Answer play_arrow

• question_answer29)
  One gram of an organic liquid X (molecular mass 78) liberates 160 J of heat on solidification. \[\Delta {{H}_{fusion}}\,\,(A)\] is:
  A)
  19.2 kJ/mol
  done clear
  B)
  12.48 kJ/mol      
  done clear
  C)
  124.8 kJ/mol
  done clear
  D)
  None of these
  done clear
  View Answer play_arrow

• question_answer30)
  The \[\Delta H_{F}^{O}\] for \[C{{O}_{2}}(g),\,\,CO(g)\] and  \[{{H}_{2}}O(g)\] are  \[-\,393.5,\,-110.5\] and \[-\,241.8\text{ }kJ\text{ }mol\],  respectively. The standard enthalpy change  (in kJ) for the reaction \[C{{O}_{2(g)}}+{{H}_{2}}_{(g)}\xrightarrow{{}}C{{O}_{(g)}}+{{H}_{2}}{{O}_{(g)}}\] is:
  A)
  + 524.1
  done clear
  B)
  + 41.2  
  done clear
  C)
  - 262.5  
  done clear
  D)
  - 41.2
  done clear
  View Answer play_arrow

• question_answer31)
  The standard heat of combustion of Al is - 837.8 kJ/mol at \[25{}^\circ C\]. Which of the following releases 250 kcal of heat?
  A)
  The reaction of 0.624 mol of Al
  done clear
  B)
  The formation of 0.624 mol of \[A{{l}_{2}}{{O}_{3}}\]
  done clear
  C)
  The reaction of 0.312 mol of \[Al\]
  done clear
  D)
  The formation of 0.150 mol of \[A{{l}_{2}}{{O}_{3}}\]
  done clear
  View Answer play_arrow

• question_answer32)
  A child bought a balloon which became very small in size the next day. Which is correct statement about balloon?
  A)
  It is isolated system
  done clear
  B)
  It is an open system
  done clear
  C)
  It is a closed system
  done clear
  D)
  it exchanges only energy with the surrounding.
  done clear
  View Answer play_arrow

• question_answer33)
  The enthalpies of formation of \[A{{l}_{2}}{{O}_{3}}\] and \[C{{r}_{2}}{{O}_{3}}\] 1596 kJ and - 1134 kJ respectively. \[\Delta H\] for the reaction \[2Al+C{{r}_{2}}{{O}_{3}}\to 2Cr+A{{l}_{2}}{{O}_{3}}\]
  A)
  - 2730 kJ
  done clear
  B)
  - 462 kJ
  done clear
  C)
  - 1365 kJ
  done clear
  D)
  + 2730 kJ      
  done clear
  View Answer play_arrow

• question_answer34)

  Calculate \[\Delta {{H}^{o}}\] for evaporation of \[{{H}_{2}}O(l)\]

  \[{{H}_{2}}+\frac{1}{2}{{O}_{2}}\xrightarrow{\,}\,{{H}_{2}}O(l);\Delta H=285.77\,\,kJ\] ?(i)

  \[{{H}_{2}}+\frac{1}{2}{{O}_{2}}\xrightarrow{\,}\,{{H}_{2}}O(g);\,\Delta H=241.84\,\,kJ\]?(ii)

  A)
  + 43.93 kJ
  done clear
  B)
  - 43.93 kJ       
  done clear
  C)
  527.61 kJ       
  done clear
  D)
  - 527.61 kJ
  done clear
  View Answer play_arrow

• question_answer35)
  The heat of neutralization of four acids A, B, C, D are -13.7, -9.4, - 11.2 and - 12.4 kcal, respectively, when they are neutralized by a common base. The acidic character obeys the order:
  A)
  A > B > C < D
  done clear
  B)
  A > D > C> B
  done clear
  C)
  D > C > B > A
  done clear
  D)
  D > B > C > A
  done clear
  View Answer play_arrow