Question

2 moles of PCl5 were introduced in a 2L flask and heated at 625K to establish equilibrium when 60% PCl5 dissociated into PCL3 and Cl2.Find the value of Kc(equilibrium constant)​

Answer 1

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Answer 2

Explanation:

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$PCl_5 { \rightleftharpoons} PCl_3 + Cl_2$

$\begin {array}{ | c | c | c | c | } </p><p></p><p>Initially & 2 & 0 & 0 \\ \\</p><p>At \: equilibrium & 2 \times \frac{40}{100} & 2 \times \frac{60}{100} & 2 \times \frac{60}{100} \\ \\ </p><p>Active \: mass & \frac{0.8}{2} & \frac{1.2}{2} & \frac{1.2}{2} </p><p>\end {array}$

$We \: know, \\ \\ \boxed{ K_c = \frac{\left[ PCl_3 \right] \times \left[Cl_2 \right] }{\left[ PCl_5 \right] }}$

$So \: using \: the \: formula..... \\ \\ K_c = \frac{\frac{1.2}{2} \times \frac{1.2}{2}}{\frac{0.8}{2}} \\ \\ K_c = \frac{0.6 \times 0.6}{0.4} \\ \\ \boxed {\boxed{ \bold{K_c = 0.9 }}}$