Chemistry: 5) 0.028 g of (NH4)2SO4 = ? moles N

5) 0.028 g of (NH4)2SO4 = ? moles N - id5002842411032410, jphelps19992019

trodgers0202

03.10.2022

$\Delta G^{0}$ = 168.12 kJ

Explanation: Gibbs Free Energy, at any time, is defined as the enthalpy of the system minus product of temperature and entropy of the reaction, i.e.:

$\Delta G^{0} = \Delta H^{0} - T.\Delta S^{0}$

Enthalpy is defined as internal heat existent in the system. It is calculated as:

$\Delta H^{0} = \Sigma H^{0}_{product} - \Sigma H^{0}_{reagent}$

Using Enthalpy Formation Table:

$\Delta H^{0} = [3*(-299.9)+(-524.7)] - (-1277)$

$\Delta H^{0} = 62,6 kJ$

Entropy is the degree of disorder in the system. It is found by:

$\Delta S^{0} = \Sigma S^{0}_{products} - \Sigma S^{0}_{reagents}$

Calculating:

$\Delta S^{0} = (-321.7) + 3(-10.8) - 0$

$\Delta S^{0} = -354.1J$

And so, Gibbs Free energy will be:

$\Delta G^{0} = \Delta H^{0} - T.\Delta S^{0}$

$\Delta G^{0} = 62600 - [298.(-354.1)]$

$\Delta G^{0} = 168121.8 J$

Rounding to the nearest kJ:

$\Delta G^{0}$ = 168.12 kJ

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