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Thermodynamics Test - 5

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Thermodynamics Test - 5
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  • Question 1
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    According to Hess’s Law, if a reaction takes place in several steps then its standard reaction enthalpy is

    Solution

    Hess’s Law states that if a reaction takes place in several steps then its standard reaction enthalpy is the sum of the standard enthalpies of the intermediate reactions into which the overall reaction may be divided at the same temperature.

  • Question 2
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    Spontaneity in the context of chemical thermodynamics means

    Solution

    Spontaneity means a reaction occurring on its own without any help of external agency.

  • Question 3
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    For an adiabatic change

    Solution

    An adiabatic process would not allow exchange of heat between the system and surroundings, hence q=0.

  • Question 4
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    According to the diagram given below, the value of H for conversion of A to B is

  • Question 5
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    Enthalpy of solution of a substance is the enthalpy change

    Solution

    Enthalpy of solution of a substance is the enthalpy change when one mole of it dissolves in a specified amount of solvent.

  • Question 6
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    Directions: The following question has four choices out of which ONLY ONE is correct.

    Dissolution of ammonium chloride in water is an endothermic change. At constant temperature, it is accompanied by
  • Question 7
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    Directions: The following question has four choices out of which ONLY ONE is correct.

    What is the entropy change (in JK-1 mol-1) when one mole of ice is converted into water at 00C? (The enthalpy change for the conversion of ice to liquid water is 6.0 kJ mol-1 at 00C.)
  • Question 8
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    Enthalpy of atomization is enthalpy change on breaking

    Solution

    Enthalpy of atomization is the enthalpy change that take place on breaking one mole of bonds completely of a compound or an element, to obtain atoms in the gas phase.

  • Question 9
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    If the enthalpy of oxidation of methanol to formaldehyde and water is -163 kJ, then what is the enthalpy of the formation of CH3OH? (Given: Enthalpy of formation of HCHO (l) is -116 kJ and enthalpy of formation of H2O (l) is -286 kJ.)
  • Question 10
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    Consider the reaction: 2C + O2  2CO2, H = - 395.5 kJ/mol. Which of the following statements is/are correct for this reaction?
  • Question 11
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    The enthalpy and entropy changes for the reaction Br2(I) + CI2(g) 2 BrCI(g) are 30 kJ mol–1 and 105 JK–1 mol–1, respectively.

    The temperature at which the reaction will be in equilibrium is
  • Question 12
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    In a reversible process, Ssys + Ssurr is 
  • Question 13
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    Standard enthalpy and standard entropy changes for the oxidation of ammonia at 298 K are - 382.64 kJ mol-1 and - 145.6 J K-1 mol-1, respectively. Standard Gibbs energy change for the same reaction at 298 K is
  • Question 14
    1 / -0
    Directions: The following question has four choices out of which ONLY ONE is correct.

    The heat of neutralisation of acetic acid by sodium hydroxide is −50.6 kJ/mol, and the heat of neutralisation of a strong acid by a strong base is −55.9 kJ/mol. What is the value of H for the ionisation of CH3COOH?
  • Question 15
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    Which of the following reactions corresponds to the definition of enthalpy of formation?
  • Question 16
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    When a solid changes into liquid, the entropy
  • Question 17
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    For the reaction 2H2 + O2 2H2O, H = -571 kJ, bond energy of H - H = 435 kJ/mol and that of O - O = 498 kJ/mol. Calculate the average bond energy (in kJ/mol) of O - H bond using this data.
  • Question 18
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    The unit of entropy is
  • Question 19
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    Which one of the following relations is incorrect?
  • Question 20
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    Identify the correct statement for change of Gibbs energy for a system (Gsystem) at constant temperature and pressure.
  • Question 21
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    The lattice enthalpy of an ionic compound is the enthalpy change which occurs when 

    Solution

    The lattice enthalpy of an ionic compound is the enthalpy change which occurs, when one mole of an ionic compound dissociates into its ions in gaseous state.

  • Question 22
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    A thermodynamic state function is a physical quantity whose value 

    Solution

    State function is one which is only dependent on initial and final state of the system and is independent of the path by which that change has occurred.

  • Question 23
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    The amount of heat liberated when 1 mole of a substance is completely burnt in the presence of oxygen is known as
  • Question 24
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    Entropy is a state function and measures

    Solution

    Entropy is a state function and it measures degree of randomness or disorder of a system. It is denoted by 'S'.

  • Question 25
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    Bond energy of hydrogen gas is - 433 kJ. What is the bond dissociation energy of 0.5 mole of hydrogen gas?
  • Question 26
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    Hess's Law deals with
  • Question 27
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    If change in Gibbs energy ΔG is negative (< 0) at constant pressure and temperature

    Solution

    ΔG gives a criteria for spontaneous and non spontaneous process at constant temperature and pressure. ΔG < 0 (negative) means reaction is spontaneous and  ΔG >0 (positive) means reaction is non spontanenous.

  • Question 28
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    If C6H6(I) + 15/2 O2(g)  3H2O(I) + 6CO2(g); = – 3264.6 kJ mol–1, then the energy obtained by burning 3.9 g of benzene in air is 
  • Question 29
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    For the process, dry ice (g), which of the following is true?
  • Question 30
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    By convention, standard enthalpy for formation of an element in reference state is:

    Solution

    By convention, enthalpies of formation of all elements in their most stable state of aggregation (reference state)  at 25oC and 1atm is taken as zero.

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