<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
If you are given the number of
moles of sodium bicarbonate, use the balanced chemical equation. The molar mass
of the acetic acid is 60 grams per mole. Using stochiometric balance.
Number of moles of acetic acid =
3 moles NaHCO3 (1 mol CH3COOH/1 mol NaHCO3) = 3 moles of acetic acid
Grams of acetic acid = 3 moles
of CH3COOH (60 g CH3COOH/1 mol CH3COOH) = <span>180 grams of acetic acid</span>
D.) the original components retain their individual properties
The boiling point of chloroform is 61.2 C or 142.2 F. Please mark as brainliest if this helped you out :).
I would agree with the second one, not the first. You can't always see the chemical reaction, and it isn't always sudden. But the second claim is true.
