Question

Brainliest will be given to correct answer :)

Answer 1

Answer: $\Delta G$ for the reaction   is -90kJ

Explanation:

The balanced chemical reaction is,

$2H_2S(g)+SO_2(g)\rightarrow 3S_{rhombic}(s)+2H_2O(g)$

The expression for Gibbs free energy change is,

$\Delta G=[n\times G_{products}]-[n\times G_{reactants}]$

Putting the values we get :

$\Delta G=[3\times G_f{S,rhombic}+2\times G_f{H_2O}]-[2\times G_f{H_2S}+1\times G_f{SO_2}]$

$\Delta G=[(3\times 0kJ/mol)+(2\times -229kJ/mol)]-[(2\times -34kJ/mol) +(1\times -300kJ/mol)]$

$\Delta G=-90kJ$

Thus $\Delta G$ for the reaction$2H_2S(g)+SO_2(g)\rightarrow 3S_{rhombic}(s)+2H_2O(g)$   is -90kJ