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  • Answer please! - Chemical Thermodynamics - NEET

For a given reaction, \DeltaH = 35.5 kJ mol-1 and \DeltaS = 83.6 JK-1 mol-1. The reaction is spontaneous at : (Assume that \DeltaH and \DeltaS do not vary with temperature)

  • Option 1)

    T < 425 K

  • Option 2)

    T > 425 K

  • Option 3)

    all temperatures

  • Option 4)

    T > 298 K

 

Answers (1)

Since, \Delta G=\Delta H-T\Delta S

for spontaneous reaction \Delta G=-ve

i.e. \Delta H< T\Delta S

Therefore, \frac{\Delta H}{\Delta S}< T

T> \frac{35.5\times 10^{3}J}{83.6\:\:\:JK^{-1}}> 425K

\therefore T>425K


Option 1)

T < 425 K

This option is incorrect.

Option 2)

T > 425 K

This option is correct.

Option 3)

all temperatures

This option is incorrect.

Option 4)

T > 298 K

This option is incorrect.

Posted by

Satyajeet kumar

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