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

  • question_answer
    From given following equations and \[\Delta H{}^\circ \] values, determine the enthalpy of reaction at 298 K for the reaction:
    \[{{C}_{2}}{{H}_{4}}\left( g \right)+6{{F}_{2}}\left( g \right)\xrightarrow{{}}2C{{F}_{4}}\left( g \right)+4HF\left( g \right)\]
    \[{{H}_{2}}(g)+{{F}_{2}}(g)\xrightarrow{{}}2HF(g);\Delta H_{1}^{{}^\circ }=-537kJ\]
    \[C\left( s \right)+2{{F}_{2}}\left( g \right)\xrightarrow{{}}C{{F}_{4}}\left( g \right);\text{ }\Delta H_{2}^{{}^\circ }=-680\text{ }kJ\]
    \[2C\left( s \right)+2{{H}_{2}}\left( g \right)\xrightarrow{{}}{{C}_{2}}{{H}_{4}}\left( g \right);\Delta H_{3}^{{}^\circ }=52kJ\]

    A) \[~-1165\]   

    B) \[-2486\]

    C) \[+1165\]                     

    D) \[+2486\]

    Correct Answer: B

    Solution :

    [b] \[\Delta {{H}^{{}^\circ }}=2\times \Delta H_{1}^{{}^\circ }+2\times \Delta H_{2}^{{}^\circ }-\Delta H_{3}^{{}^\circ }=-2486\,kJ\]


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