For the following reaction, equilibrium constant Kc at 298 K is 1.6×1017 Fe(aq)2++S(aq)2⇔FeS(s) When equal volume of 0.06 MFe2+ and 0.2 Ms−2 solution are mixed, then equilibrium concentration of Fe2+ is found to be Y×10−17M. Y is

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For the following reaction, equilibrium constant {K}_{{{c}}} a

Question

For the following reaction, equilibrium constant $K_{c}$ at 298 K is $1.6 \times 10^{17}$
$F e_{(a q)}^{2 +} + S_{(a q)}^{2} \Leftrightarrow F e S (s)$
When equal volume of 0.06 $M F e^{2 +}$ and 0.2 $M s^{- 2}$ solution are mixed, then equilibrium concentration of $F e^{2 +}$ is found to be $Y \times 10^{- 17} M$ . Y is

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For the following reaction, equilibrium constant

K_{c}

at 298 K is

1.6 \times 10^{17}

F e_{(a q)}^{2 +} + S_{(a q)}^{2} \Leftrightarrow F e S (s)

When equal volume of 0.06

M F e^{2 +}

and 0.2

M s^{- 2}

solution are mixed, then equilibrium concentration of

F e^{2 +}

is found to be

Y \times 10^{- 17} M

. Y is

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