`K_c` for the reaction :
`2H_2S(g) hArr 2H_2(g) + S_2(g)` is `1xx10^(-6)` at 100 K.
What is the dissociation of `H_2S` is 1 mole of `H_2S` is introduced in a 1.1 L of flask at 1000 K?

Explanation

To solve the problem, we need to determine the dissociation of \( H_2S \) when 1 mole is introduced into a 1.1 L flask at 1000 K, given that the equilibrium constant \( K_c \) for the reaction

\[ 2H_2S(g) \rightleftharpoons 2H_2(g) + S_2(g) \]

is \( 1 \times 10^{-6} \).

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