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Equilibrium constant \( (\mathrm{K}) \) for the reaction
\( \mathrm{Ni}(\mathrm{s})+4 \mathrm{CO}(\mathrm{g}) \rightleftharpoons \mathrm{Ni}(\mathrm{CO})_{4}(\mathrm{~g}) \) can be written in terms of
(1) \( \mathrm{Ni}(\mathrm{s})+2 \mathrm{CO}_{2}(\mathrm{~g})+2 \mathrm{C}(\mathrm{s}) \rightleftharpoons \mathrm{Ni}(\mathrm{CO})_{4}(\mathrm{~g}) \);
equilibrium constant \( =\mathrm{K}_{1} \).
(2) \( \mathrm{CO}_{2}(\mathrm{~g})+\mathrm{C}(\mathrm{s}) \rightleftharpoons 2 \mathrm{CO}(\mathrm{g}) \);
equilibrium constant \( =\mathrm{K}_{2} \).
What is the relation between \( \mathrm{K}, \mathrm{K}_{2} \) and \( \mathrm{K}_{2} \) ?
(a) \( \mathrm{K}=\left(\mathrm{K}_{1}\right) /\left(\mathrm{K}_{2}\right)^{2} \)
(b) \( \mathrm{K}=\left(\mathrm{K}_{1} \cdot \mathrm{K}_{2}\right) \)
(c) \( \mathrm{K}=\left(\mathrm{K}_{1}\right)\left(\mathrm{K}_{2}\right)^{2} \)
(d) \( \mathrm{K}=\mathrm{K}_{1} / \mathrm{K}_{2} \)
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