When sulphur in the form of S8 is heated at 900 K the initial pressure of 1 atm falls by 29% at equilibrium. This is because of conversion of some S8 to S2 . Find the value of equilibrium constant for this reaction.

Question

When sulphur in the form of S8 is heated at 900 K the initial pressure of 1 atm falls by 29% at equilibrium. This is because of conversion of some S8 to S2 . Find the value of equilibrium constant for this reaction. (A) 2.55 atm3 (B) 255 atm3 (C) 25.5 atm3 (D) None

Tardigrade Admin · Accepted Answer

underset underset1 - x1S8 (. g .)leftharpoons underset underset4 x04 S2 (. g .) x=29 %=0.29 Kp=((PS2 )4/(PS8))=(( 4 x2)/(. 1 - x ) ) atm3 =(( 4 × 0.29 4 /1 - 0.29)=2.55 atm3 .

Q. When sulphur in the form of $S_{8}$ is heated at 900 K the initial pressure of 1 atm falls by 29% at equilibrium. This is because of conversion of some $S_{8}$ to $S_{2}$ . Find the value of equilibrium constant for this reaction.

$2.55 a t m^{3}$

$255 a t m^{3}$

$25.5 a t m^{3}$

None

$1 - x 1 S_{8} (g) ⇌ 4 x 0 4 S_{2} (g)$

$x = 29% = 0.29$

$K_{p} = \frac{( P _{S_{2}} ) ^{4}}{( P _{S_{8}} )} = \frac{( 4 x ^{2} )}{( 1 - x )} a t m^{3}$

$= \frac{( 4 \times 0.2 9 ^{4}}{1 - 0.29} = 2.55 a t m^{3}$ .

Q. When sulphur in the form of S8​ is heated at 900 K the initial pressure of 1 atm falls by 29% at equilibrium. This is because of conversion of some S8​ to S2​ . Find the value of equilibrium constant for this reaction.

2.55atm3

255atm3

25.5atm3