Chemistry, 07.03.2020 04:48 Mattisback2285
A chemist fills a reaction vessel with 7.92 atm nitrogen (N2) gas, 2.02 atm hydrogen (H2) gas, and 2.11 atm ammonia (NH3) gas at a temperature of 25.0°C
Under these conditions, calculate the reaction free energy ΔG for the following chemical reaction
N2(8) +3H2 2NH3 (g)
Use the thermodynamic information in the ALEKS Data tab. Round your answer to the nearest kilojoule.
Answers: 3
![\Delta G^o_{rxn}=[(2\times \Delta G^o_f_{(NH_3(g))})]-[(1\times \Delta G^o_f_{(N_2(g))})+(3\times \Delta G^o_f_{(H_2(g))})]](/tpl/images/0537/7676/6e73c.png)
![\Delta G^o_{rxn}=[(2\times (-16.45))]-[(1\times (0))+(3\times (0))]\\\\\Delta G^o_{rxn}=-32.9kJ/mol](/tpl/images/0537/7676/8bdb6.png)
= free energy of the reaction
= standard Gibbs free energy = -32.9 kJ/mol = -32900 J/mol (Conversion factor: 1 kJ = 1000 J)![25^oC=[273+25]K=298K](/tpl/images/0537/7676/0e82f.png)
= Ratio of concentration of products and reactants at any time = 
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