2. Questions Bank
  3. NEET
  4. Chemistry
  5. Thermodynamics / रासायनिक उष्मागतिकी

NEET Chemistry Thermodynamics / रासायनिक उष्मागतिकी Question Bank Self Evaluation Test - Thermodynamics

  • question_answer
    The molar entropies of HI (g) and I (g) at 298 K are 206.5, 114.6, and \[180.7\text{ }J\text{ }mo{{l}^{-1}}{{K}^{-1}}\] respectively. Using the\[\Delta G{}^\circ \]given Below, calculate the bond energy of HI. \[HI\left( g \right)\xrightarrow{{}}H\left( g \right)+I\left( g \right);\text{ }\Delta G{}^\circ =271.8\text{ }kJ\]

    A) \[282.4\text{ }kJmo{{l}^{-1}}\]            

    B) \[298.3\text{ }kJmo{{l}^{-1}}\]

    C) \[290.1\text{ }kJmo{{l}^{-1}}\]            

    D) \[315.4\text{ }kJmo{{l}^{-1}}\]

    Correct Answer: B

    Solution :

    [b] \[\Delta {{S}^{{}^\circ }}=-206.5+114.6+180.7=88.8\] \[\Delta {{G}^{{}^\circ }}=\Delta {{H}^{{}^\circ }}-T\Delta {{S}^{{}^\circ }}\] \[\Delta {{H}^{{}^\circ }}=271.8+298\times 88.8\times {{10}^{-3}}\] \[\Delta {{H}^{{}^\circ }}=298.3\text{ }kJ\text{ }mo{{l}^{-1}}\]


You need to login to perform this action.
You will be redirected in 3 sec spinner