JEE Main & Advanced Chemistry Thermodynamics / रासायनिक उष्मागतिकी Question Bank

done Numerical Value Type Question - Chemical Energetic Total Questions - 16

• question_answer1)
  What is the heat of formation of \[HCl\,\left( g \right)\] from reaction   \[{{H}_{2}}\,\left( g \right)\,\,+\,\,C{{l}_{2}}\left( g \right)\,\,\to \,\,2HCl\,\left( g \right).\,\,\Delta H\,\,=\,\,44\,\,kcal.\]
  View Solution play_arrow

• question_answer2)
  When 10 gm of hydrogen gas at 1 aim pressure and \[30{}^\circ C\]  is brought to a reduced pressure of \[\frac{1}{2}\]  atm also at \[30{}^\circ C,\]  calculate entropy change involved.
  View Solution play_arrow

• question_answer3)
  You are given Avogadro's number of "X" atoms. If half of the atoms of X transfer one electron to other half of 'X' atoms, 409 KJ must be added. If these \[{{X}^{-}}\] ions are subsequently converted to \[{{X}^{+}}\] , an addition 733 KJ must be added. Calculate IP of X in eV. Use \[(1eV=1.602\times {{10}^{-19}}\,J\,\,and\,\,{{N}_{A}}=6.023\times {{10}^{23}})\]
  View Solution play_arrow

• question_answer4)
  The heat evolved on combustion of 1 gm starch \[{{\left( {{C}_{6}}{{H}_{10}}{{O}_{5}} \right)}_{n}}\]  into \[C{{O}_{2}}\]  and \[{{H}_{2}}O\,\left( \ell  \right)\]  is \[17.49\,\,kJ\,\,g{{m}^{-1}}.\]  Compute the enthalpy of formation of 1 gm starch. Given \[\Delta {{H}_{f}}\,\,of\,\,{{H}_{2}}O\,\,\left( \ell  \right)\,\,=\,\,-\,285.85\,\,kJ\,\,mo{{l}^{-1}},\] \[\Delta {{H}_{f}}\,\,of\,\,C{{O}_{2}}\,\,=\,\,-293.7\,\,kJ\,\,mol{{e}^{-1}}\]
  View Solution play_arrow

• question_answer5)
    The heat of formation of \[C{{O}_{2}}\,\left( g \right)\]  and \[{{H}_{2}}O\,\left( l \right)\] are - 94.3 kcal and - 68.4 kcal respectively. Calculate heat of combustion of \[{{C}_{6}}{{H}_{6}}\] if heat of formation of \[{{C}_{6}}{{H}_{6}}\]  is +11.72 kcal.
  View Solution play_arrow

• question_answer6)
  Calculate the heat of combustion of glucose from the following data -

  (i) \[{{C}_{\left( graphite \right)}}\,\,+\,\,{{O}_{2}}\,\,\left( g \right)\,\,\xrightarrow{{}}\,\,C{{O}_{2}}\,\left( g \right),\,\,\Delta H\,\,=\,\,-395.0\,\,kJ\]

  (ii) \[{{H}_{2}}\,\,\left( g \right)\,\,+\,\,{}^{1}/{}_{2}{{O}_{2}}\,\,\xrightarrow{{}}\,\,{{H}_{2}}O\,\left( l \right),\,\,\Delta H\,\,=\,\,-269.5\,\,kJ\]

  (iii) \[6{{C}_{\left( graphite \right)}}\,\,+\,\,6{{H}_{2}}\,\left( g \right)\,\,+\,\,3{{O}_{2}}\,\left( g \right)\,\,\xrightarrow{{}}\,\,{{C}_{6}}{{H}_{12}}{{O}_{6}}\,\,\left( s \right),\]\[\Delta H\,\,=\,\,-1170\,\,kJ\]

  View Solution play_arrow

• question_answer7)
  Standard heat of combustion of \[{{C}_{2}}{{H}_{2}}\,\left( g \right)\] and \[{{C}_{2}}{{H}_{4}}\,\,\left( g \right)\] are - 310.6 kcal and - 337.2 kcal per mole respectively. Heat of formation of water is\[-\,68.3\text{ }kcal\text{ }mo{{l}^{-\,1}}\]. Calculate heat of hydrogenation of \[{{C}_{2}}{{H}_{2\text{ }}}\,\left( g \right)\,\,to\,\,{{C}_{2}}{{H}_{4}}\,\left( g \right).\]  
  View Solution play_arrow

• question_answer8)
  Calculate the heat evolved in the formation of 2.5 litre of CO at STP from its elements. Given that \[C\,\,+\,\,{{O}_{2}}\,\,\xrightarrow{{}}\,\,C{{O}_{2}}\] \[\Delta H\,\,=\,\,-94.5\,\,kcal\] \[2CO\,\,+\,\,{{O}_{2}}\,\,\xrightarrow{{}}\,\,2C{{O}_{2}}\]      \[\Delta H\,\,=\,\,-136.0\,\,kcal\]
  View Solution play_arrow

• question_answer9)
  The enthalpy for the following reactions \[\left( \Delta H{}^\circ  \right)\] at \[25{}^\circ C\]are given as : \[1/2{{H}_{2}}\,\left( g \right)\,\,+\,\,1/2\,{{O}_{2}}\,\left( g \right)\,\,\xrightarrow{{}}\,\,OH\,\left( g \right)\,:\,\Delta H\,\,=\,\,10.06\,\,kcals\]\[{{H}_{2}}\,\,\left( g \right)\,\,\xrightarrow{{}}\,\,2H\,\,\left( g \right)\,\,:\,\,\Delta H\,\,=\,\,104.18\,\,kcals\] \[{{O}_{2}}\,\,\left( g \right)\,\,\xrightarrow{{}}\,\,2O\,\,\left( g \right)\,\,:\,\,\Delta H\,\,=\,\,118.32\,\,kcals\] Calculate the \[O-H\] bond energy in the hydroxyl radical.
  View Solution play_arrow

• question_answer10)
  Calculate the enthalpy of the reaction. \[C{{H}_{2}}\,\,=\,\,C{{H}_{2}}\,\,\left( g \right)\,\,+\,\,{{H}_{2}}\,\,\left( g \right)\,\,\xrightarrow{{}}\,\,C{{H}_{3}}\,\,-\,\,C{{H}_{3\text{ }}}\,\,\left( g \right).\]Bond energies of \[C\,-\,H,\,\,C\,-\,C,\,\,C\,=\,C\]and \[H\,-\,H\]are 99, 83, 147 and 104 kcal respectively.
  View Solution play_arrow

• question_answer11)
  Bond energies of \[{{F}_{2}}\] and \[C{{l}_{2}}\] are 153.0 and \[242.4\,\,kJ\,/\,mol\] respectively. The heat liberated in the reaction is 111.0 kJ. Find out the bond energy of \[F\,-\,Cl.\] \[1/2\,{{F}_{2}}\,\,+\,\,1/2\,C{{l}_{2}}\,\,\xrightarrow{{}}\,\,FCl\]
  View Solution play_arrow

• question_answer12)
  Calculate the free energy change when 1 mole of \[NaCl\] is dissolved in water at \[25{}^\circ C.\] Lattice energy of \[NaCl\,\,=\,\,777.8\,\,kJ\,\,mo{{l}^{-1}}\,;\] \[\Delta S\,\,for\,\,dissolution\,\,=\,\,0.043\,\,kJ\,\,mo{{l}^{-1}}\,\,;\]and hydration energy of \[NaCI\,\,=\,\,-774.\,\,1\,kJ\,\,mo{{l}^{-1}}.\]
  View Solution play_arrow

• question_answer13)
  Calculate the standard free energy change for the reaction, \[{{N}_{2(g)}}+3{{H}_{2(g)}}\xrightarrow{{}}2N{{H}_{3(g)}}\]at\,\,298\,\,K.\] Given \[\Delta H{}^\circ \,\,=\,\,-\,92.4kJ\text{ }and\] \[\Delta S{}^\circ \,\,=\,\,-\,198.3\,\,J{{K}^{-1}}.\]
  View Solution play_arrow

• question_answer14)
  10 moles of an ideal gas expands isothermally and reversibly from a pressure of 10 aim to 2 aim at 300K. What is the largest mass which can be lifted through a height of 1 meter in this expansion?
  View Solution play_arrow

• question_answer15)
  Diborane is a potential rocket fuel which undergoes combustion according to the reaction. \[{{B}_{2}}{{H}_{6}}\,\left( g \right)\,\,+\,\,3{{O}_{2}}\,\left( g \right)\,\,\xrightarrow{{}}\,\,{{B}_{2}}{{O}_{3}}\,\left( s \right)\,\,+\,\,3{{H}_{2}}O\,\left( g \right)\] From the following data, calculate the enthalpy change for the combustion of diborane. \[2B\,\left( s \right)\,\,+\,\,\left( 3/2 \right){{O}_{2}}\,\,\left( g \right)\,\,\xrightarrow{{}}\,\,{{B}_{2}}{{O}_{3}}\,\,\left( s \right)\] \[\Delta H\,\,=\,\,-\,\,1273\,\,kJ\,\,mo{{l}^{-1}}\] \[{{H}_{2}}\,\,\left( g \right)\,\,+\,\,\left( 1/2 \right)\,{{O}_{2}}\,\,\left( g \right)\,\,\xrightarrow{{}}\,\,{{H}_{2}}O\,\,\left( l \right)\] \[\Delta H\,\,=\,\,-286\,\,kJ\,\,mo{{l}^{-1}}\] \[{{H}_{2}}O\,\left( l \right)\,\,\xrightarrow{{}}\,\,{{H}_{2}}O\,\left( g \right)\] \[\Delta H\,\,=\,\,44\,\,kJ\,\,mo{{l}^{-1}}\] \[2B\,\left( s \right)\,\,+\,\,3{{H}_{2}}\,\left( g \right)\,\,\xrightarrow{{}}\,\,{{B}_{2}}{{H}_{6}}\,\left( g \right)\] \[\Delta H\,\,=\,\,36\,\,kJ\,\,mo{{l}^{-1}}\]
  View Solution play_arrow

• question_answer16)
  A sample of argon gas at 1 aim pressure and  expands reversibly and adiabatically from  to  Calculate the enthalpy change in this process Cv.m for Argon is  
  View Solution play_arrow