If the value of K= 2.1x10-2 at 720 K which predominate HI or H2 and I2
Added by Andrea R.
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1 \times 10^{-2} \) at 720 K, we can follow these steps: ** Show more…
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In a closed tube, $\mathrm{HI}(\mathrm{g})$ is heated at $440^{\circ} \mathrm{C}$ up to establishment of equilibrium. If it dissociates into $\mathrm{H}_{2}(\mathrm{~g})$ and $\mathrm{I}_{2}(\mathrm{~g})$ up to $22 \%$, the dissociation constant is (a) $0.282$ (b) $0.0796$ (c) $0.0199$ (d) $1.99$
Chemical Equilibrium
Exercises I
At $667 \mathrm{~K}, \mathrm{HI}$ is found to be $11.4 \%$ dissociated into its clements. $$ 2 \mathrm{HI}(\mathrm{g}) \rightleftharpoons \mathrm{H}_{2}(\mathrm{~g})+\mathrm{I}_{2}(\mathrm{~g}) $$ If $1.00 \mathrm{~mol} \mathrm{HI}$ is placed in a $1.00-\mathrm{L}$. container and the container is sealcd and heated to $667 \mathrm{~K}$, calculate (a) the cquilibrium concentration of all three substances and (b) the value of $K$, for this equilibrium at this temperature.
A quantity of HI was sealed in a tube, heated to 425°C and held at this temperature until equilibrium was reached. The concentration of HI at equilibrium was found to be 0.0706 mol/L. Calculate the equilibrium concentration of H2 (and I2) for the gas-phase reaction: H2 + I2 ⇌ 2HI Kc is 54.6 at 425°C.
David C.
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