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question_answer1) What will happen to the internal energy if work is done by the system?
question_answer2) Change in internal energy is a state function while work is not, why?
question_answer3) Why are changes in heat energy generally enthalpy changes and not internal energy changes?
question_answer4) State the thermodynamic conditions for the process to occur spontaneously?
question_answer5) When an ideal gas expands in vacuum, there is neither absorption nor evolution of heat. Explain.
question_answer6) Although the dissolution of NaCl(s) in water is endothermic but it dissolves. Explain.
question_answer7) When a piece of ice is placed on your hand, you get a cold sensation. Why?
question_answer8) Why is standard heat of formation of diamond not zero although it is an element?
question_answer9) Hess's law is a corollary of the first law of thermodynamics. Comment.
question_answer10) Out of the following reactions, in which case heat evolved will be more? \[{{H}_{2}}(g)+\frac{1}{2}\,{{O}_{2}}(g)\xrightarrow{\,}\,{{H}_{2}}O(g)\] \[{{H}_{2}}(g)+\frac{1}{2}\,{{O}_{2}}(g)\xrightarrow{\,}\,{{H}_{2}}O(l)\]
question_answer11) (i) For a reaction both \[\Delta H\] and \[\Delta S\]are negative. Under what conditions does the reaction occur spontaneously? (ii) For a reaction both \[\Delta H\] and \[\Delta S\] are positive. Under what conditions does the reaction occur spontaneously?
question_answer12) When an ideal gas expands, there is no change in temperature. On the other hand, when a real gas expands, cooling is produced. Explain why.
question_answer13) An exothermic reaction may not be always thermodynamically spontaneous. Justify.
question_answer14) Explain why entropy of a perfectly crystalline substance is less than that of its imperfect crystals.
question_answer15) The entropy of steam is more than that of water at its boiling point. Explain.
question_answer16) To what type of system the following belong? (i) Tree (ii) Pond (iii) Animals (iv) Tea placed in a kettle (v) Tea placed in thermos flask (vi) Tea placed in a cup.
question_answer17) Separate out the following into extensive and intensive: Volume, Temperature, Pressure, Boiling point, Free energy
question_answer18) Can the absolute value of internal energy be determined? Why or why not?
question_answer19) One mole of \[C{{O}_{2}}\] at 300 K and 1 atm pressure is heated in a closed vessel so that temperature is 500 K and pressure is 5 atm. Then it is cooled so that temperature is 300 K and pressure is 1 atm. What is the change in internal energy of the gas?
question_answer20) Show that the product of pressure and volume has the dimensions of energy. Derive the value for 1 litre-atmosphere.
question_answer21) For the same increase in volume, why work done is more if the gas is allowed to expand reversibly at higher temperature?
question_answer22) Water decomposes by absorbing \[286.2\,kJ\] of electrical energy per mole. When \[{{H}_{2}}\] and\[{{O}_{2}}\] combine to form one mole of \[{{H}_{2}}O,\,\,286.\,2kJ\] of heat is produced. Which law is proved? What statement of the law follows from it?
question_answer23) One kg of graphite is burnt in a closed vessel. The same amount of the same sample is burnt in an open vessel. Will the heat evolved in the two cases be same? If not, in which case it would be greater?
question_answer24) Under what condition \[\Delta H\] becomes equal to \[\Delta U\]?
question_answer25) Same mass of diamond and graphite (both being carbon) are burnt in oxygen. Will the heat produced be same or different? Why?
question_answer26) Why standard heat of formation of diamond is not zero though it is an element?
question_answer27) The enthalpy of formation of gaseous iodine is \[62.5\,kJ\,mo{{l}^{-1}}\] at 25°C. What will be the enthalpy of sublimation of iodine at 25°C?
question_answer28) Find out (i) Heat of formation of \[C{{H}_{4}}\] in terms of \[\Delta {{H}_{1}},\,\Delta {{H}_{2}}\] etc. (ii) Heat of sublimation of \[{{C}_{graphite}}\] in terms of \[\Delta {{H}_{1}},\,\Delta {{H}_{2}}\] etc. (iii) Heat of dissociation of \[{{H}_{2}}\] in terms of \[\Delta {{H}_{1}},\,\Delta {{H}_{2}}\] etc.
question_answer29) Given that (i) \[O\,(g)+{{e}^{-}}\xrightarrow{\,}\,{{O}^{-}}(g),\]\[\Delta H=-142\,kJ\,mo{{l}^{-1}}\] (ii)\[O(g)+2\,{{e}^{-}}\xrightarrow{\,}\,{{O}^{2-}}(g),\] \[\,\Delta H=+712\,kJ\,mo{{l}^{-1}}\] Calculate \[\,\Delta H\] for the reaction \[{{O}^{-}}(g)+{{e}^{-}}\xrightarrow{\,}\,{{O}^{2-}}(g)\].
question_answer30) Is the bond energy of all the four C-H bonds in \[C{{H}_{4}}\] molecule equal? If not then why? How is the \[C-H\] bond energy then reported?
question_answer31) Water can be lifted into the water tank at the top of the house with the help of a pump. Then why is not considered to be spontaneous?
question_answer32) Rank the following in the order of increasing entropy: (a) 1 mole of\[{{H}_{2}}O\,\,(l)\] at 25° C and 1 atm. pressure. (b) 2 mole of \[{{H}_{2}}O\,\,(s)\] at 0°C and 1 atm. pressure. (c) 1 mole of \[{{H}_{2}}O\,\,(\upsilon )\] at 100°C and 1 atm. pressure. (d) 1 mole of \[{{H}_{2}}O\,\,(l)\]at 0°C and 1 atm. pressure.
question_answer33) An exothermic reaction \[A\xrightarrow{\,}B\] is spontaneous in the backward direction. What will be the sign of\[\Delta S\] for the forward reaction?
question_answer34) Predict whether following reaction will be exothermic or endothermic. Give reason for your answer \[H-H(g)+Cl-Cl(g)\xrightarrow{{}}\,2\,H-Cl\,(g)\]
question_answer35) We are consuming a lot of electrical energy, solar energy etc. Do you, therefore, conclude that energy of the universe is continuously decreasing? Explain. Which other thermodynamic quantity is continuously increasing or decreasing?
question_answer36) Under what condition, the heat evolved or absorbed in a reaction is equal to its free energy change?
question_answer37) At a certain temperature 'T' the endothermic reaction \[A\xrightarrow{\,}B\] proceeds virtually to the end. Determine (i) sign of \[\Delta S\] for this reaction (ii) sign of \[\Delta G\] for the reaction \[B\xrightarrow{\,}A\] at the temperature T, and (iii) the possibility of reaction \[B\xrightarrow{\,}A\] proceeding at a low temperature.
question_answer38) Why endothermic reactions are favoured at high temperature?
question_answer39) The standard free energy of a reaction is found to be zero. What is its equilibrium constant?
question_answer40) Calculate \[\Delta G\] and \[\Delta {{G}^{o}}\] for the reaction : \[A+B\rightleftharpoons C+D\] at 27°C. Equilibrium constant (K) for this reaction \[={{10}^{2}}\].
question_answer41) Explain why the entropy of a pure crystalline substance is zero at 0K? State the law on which it is based. Give the application of this law?
question_answer42) Comment on the validity of the following statements, giving reasons: (i) Thermodynamically, an exothermic reaction is sometimes not spontaneous. (ii) The entropy of steam is more than that of water at its boiling point (iii) The equilibrium constant for a reaction is one or more if \[{{\Delta }_{r}}G{}^\circ \] for it is less than zero.
question_answer43) Give reasons: (a) Neither \[q\] nor \[w\] is a state function but \[q+w\] is a state function. (b) The dissolution of ammonium chloride in water is endothermic still it dissolves in water. (c) A real crystal has more entropy than an ideal crystal.
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