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Question

At a certain temperature the equilibrium constant (K)(K) for the following reaction is 9.00×1029.00 \times 10^2.

2H2(g)+S2(g)2H2 S(g)2 \mathrm{H}_2(g)+\mathrm{S}_2(g) \rightleftharpoons 2 \mathrm{H}_2 \mathrm{~S}(g)

It is found that [H2]=0.010 M\left[\mathrm{H}_2\right]=0.010~M and [H2 S]=0.15 M\left[\mathrm{H}_2 \mathrm{~S}\right]=0.15~M. Calculate [S2]\left[\mathrm{S}_2\right].

Solution

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Answered 2 years ago
Answered 2 years ago
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The reaction system below has already reached the state of equilibrium:

2 H2 (g) + S2 (g)  2 H2S (g)\begin{aligned} \text{2 H$_2$ (g) + S$_2$ (g) $\rightleftharpoons$ 2 H$_2$S (g)} \end{aligned}

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