The factor of values are important in metallurgy. The $∆ G$ values for the following reactions at 800°C are given as
$\begin{array}{l} S_{2} (s) + 2 O_{2} (g) \to 2 {SO}_{2} (g), ΔG = - 544 kj \\ 2 Zn (s) + S_{2} (s) \to 2 ZnS (s), ΔG = - 293 kj \\ 2 Zn (s) + O_{2} (g) \to 2 ZnO (s), ΔG = - 480 kj \end{array}$
The $∆ G$ for the reaction,
$2 ZnS (s) + 3 O_{2} (g) \to 2 ZnO (s) + 2 {SO}_{2} (g)$
will be

see full answer

Start JEE / NEET / Foundation preparation at rupees 99/day !!

21% of IItians & 23% of AIIMS delhi doctors are from Sri Chaitanya institute !!

An Intiative by Sri Chaitanya

-357 kJ

-731kJ

-673kJ

-229KJ

answer is B.

(Unlock A.I Detailed Solution for FREE)

Ready to Test Your Skills?

Check your Performance Today with our Free Mock Test used by Toppers!

Take Free Test

Detailed Solution

$∆ G$ of formation of different substance are as
2SO₂ = -544 kJ
2Zns = -293 kJ
2ZnO = -480 kJ
For the reaction,
$\begin{array}{l} 2 ZnS + 3 O_{2} (g) \to 2 ZnO (s) + 2 {SO}_{2} (g) \\ ΔG = [{ΔG}_{(products)} - {ΔG}_{(reactan ts)}] \\ = [(- 480) + (- 544) - (- 293)] \\ = - 1024 + 293 = - 731 kJ \end{array}$