<u>Answer:</u> The Gibbs free energy of the given reaction is -40 kJ
<u>Explanation:</u>
The given chemical equation follows:
The equation for the standard Gibbs free change of the above reaction is:
![\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))})]](https://tex.z-dn.net/?f=%5CDelta%20G%5Eo_%7Brxn%7D%3D%5B%282%5Ctimes%20%5CDelta%20G%5Eo_f_%7B%28NH_3%28g%29%29%7D%29%5D-%5B%281%5Ctimes%20%5CDelta%20G%5Eo_f_%7B%28N_2%28g%29%29%7D%29%2B%283%5Ctimes%20%5CDelta%20G%5Eo_f_%7B%28H_2%28g%29%29%7D%29%5D)
We are given:
Putting values in above equation, we get:
![\Delta G^o_{rxn}=[(2\times (-16.45))]-[(1\times (0))+(3\times (0))]\\\\\Delta G^o_{rxn}=-32.9kJ/mol](https://tex.z-dn.net/?f=%5CDelta%20G%5Eo_%7Brxn%7D%3D%5B%282%5Ctimes%20%28-16.45%29%29%5D-%5B%281%5Ctimes%20%280%29%29%2B%283%5Ctimes%20%280%29%29%5D%5C%5C%5C%5C%5CDelta%20G%5Eo_%7Brxn%7D%3D-32.9kJ%2Fmol)
The equation used to Gibbs free energy of the reaction follows:
where,
= free energy of the reaction
= standard Gibbs free energy = -32.9 kJ/mol = -32900 J/mol (Conversion factor: 1 kJ = 1000 J)
R = Gas constant = 8.314J/K mol
T = Temperature = ![25^oC=[273+25]K=298K](https://tex.z-dn.net/?f=25%5EoC%3D%5B273%2B25%5DK%3D298K)
= Ratio of concentration of products and reactants at any time = 
Putting values in above equation, we get:
Hence, the Gibbs free energy of the given reaction is -40 kJ
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It is important to test only one variable, because 2 or more may cause changes in the original variable that weren't supposed to occur
Answer:
The reverse of answer B
Explanation:
In a heterogeneous mixture the phases are clearly seen distinguished but a uniform single phase is seen in a homogeneous mixture
