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The following equilibrium constants have been determined for hydrosulfuric acid at 25ºC:
H2S(aq) ⇌ H+(aq) + HS–(aq) K′c = 9.5 × 10^–8
HS–(aq) ⇌ H+(aq) + S2–(aq) K″c = 1.0 × 10^–19
Calculate the equilibrium constant for the following reaction at the same temperature: H2S(aq) ⇌ 2H+(aq) + S2–(aq).

Answer :

Willchemistry

hey there!:

H2S(aq) <=> H⁺(aq) + HS⁻(aq)

K'c = [H⁺][HS⁻]/[H₂S] = 9.5*10⁻⁸

HS⁻(aq) <=> H⁺(aq) + S²⁻(aq)

K"c = [H⁺][S²⁻]/[HS⁻] = 1.0*10⁻¹⁹

H₂S(aq) <=> 2 H⁺(aq) + S²⁻(aq)

Kc = [H⁺]²[S²⁻] / [H₂S]

= [H+][HS⁻] / [H₂S] * [H⁺][S²⁻]/[HS⁻]

= K'c *K"c

= ( 9.5*10⁻⁸ ) * ( 1.0 x 10⁻¹⁹ )

= 9.5*10⁻²⁷

Hope this helps!

mahima6824soni

The equilibrium constants the following reaction at the same temperature is 9.5*10⁻²⁷.

What is equilibrium?

Equilibrium is the state that is in control, a balance state in which no changes occur.

The calculation of equilibrium constants is

[tex]H_2S(aq) < = > H^+(aq) + HS^-(aq)[/tex]

K'c = [H⁺] [HS⁻] / [H₂S] = 9.5 * 10⁻⁸

HS⁻ (aq) <=> H⁺(aq) + S²⁻(aq)

K"c = [H⁺] [S²⁻]/[HS⁻] = 1.0 * 10⁻¹⁹

H₂S (aq) <=> 2 H⁺(aq) + S²⁻(aq)

Kc = [H⁺]²[S²⁻] / [H₂S]

= [H+] [HS⁻] / [H₂S] * [H⁺] [S²⁻] / [HS⁻]

= K'c *K"c

= ( 9.5*10⁻⁸ ) * ( 1.0 x 10⁻¹⁹ )

= 9.5*10⁻²⁷

Thus, the equilibrium constants of the following reaction at the same temperature is 9.5*10⁻²⁷.

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