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Question

3.2 moles of HI(g) were heated in a sealed bulb at 444oC till the equilibrium reached. Its 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 the equilibrium constant for the reaction 2HI(g)H2(g)+I2(g). Considering the volume of the container 1 L.

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Solution

moles 2HIH2+I2
at t=0 3.2 - -
at eqbm 3.20.2×3.2 0.2×3.22 0.2×3.22
Keq=[nH2][nI2][nHI]2[1V]0
Keq=0.32×0.32[2.56]2=1.56×102
Number of moles at equilibrium,
H20.32 moles
I20.32 moles
HI2.56 moles

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