Answer:
Kc = 32.3
Explanation:
To calculate the Kc, it's the ratio of products over reactants (each raised to their respective stoichiometric coefficient). In this case:
[tex]K_c = \frac{{[H_2]}^8[S_8]}{{[H_2S]}^8}\\K_c = \frac{0.4^8 \times 0.75}{0.25^8}\\K_c = \frac{4.91 \times 10^{-4}}{1.52 \times 10^{-5}}\\K_c = 32.3[/tex]
The equilibrium constant for the reaction is 32.2
The equilibrium constant (K꜀) for a given reaction is simply defined as the ratio of the concentration of the products raised to their coefficients to the concentration of the reactants raised to their coefficients
With the above information, we can obtain the equilibrium constant for the reaction given above as follow:
8H₂S(g) <=> 8H₂(g) + S₈(g)
Concentration of Hydrogen sulphide [H₂S] = 0.250 M
Concentration of Hydrogen [H₂] = 0.400 M
Concentration of sulphur [S₈] = 0.750 M
[tex]K_{C} = \frac{[H_{2}]^8[S_{8}]}{[H_{2}S]^{8}} \\\\K_{C} = \frac{0.4^{8} * 0.750}{0.25^{8}}\\\\[/tex]
Therefore, the equilibrium constant for the reaction is 32.2
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