A mixture containing 8.07 moles of hydrogen and 9.08 moles of iodine was heated at 448° C till equilibrium was attained when 13.38 moles of hydrogen iodide was obtained. Find the degree of disassociation.
Answers
Answer:
3.2 moles of HI(g) were heated in a sealed bulb at 444°C till the equilibrium was reached. It's degree of dissociation was found to be 20%. Calculate the number of moles of hydrogen iodide, hydrogen and iodine present at the equilibrium point and determine the value of equilibrium constant for the reaction
2HI (g) (g). Considering the volume of the container 1 L.2(g) + I2
Answer:
Explanation:
At a given temperature, the product of concentration of the reaction products raised to the respective stoichiometric coefficient in the balanced chemical equation divided by the product of concentration of the reactants raised to their individual stoichiometric coefficients has a constant value.
- wherein
aA+bB\rightleftharpoons cC+dD
K_{c}=\frac{[C]^{c\:[D]^{d}}}{[A]^{a}\:[B]^{b}}
[A],\:[B],\:[C]\:[D]
are equilibrium concentration
The reaction undergoes as follows:
2HI\:\rightleftharpoons \:H_{2}+I_{2}
At t=0 3.2 0 0
At equilibrium 3.2(1-\propto ) 3.2\propto 3.2\propto
\propto\:=\:0.22\:(given)