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) H2(g)+I2(g). Considering the volume of the container 1L.
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Concentration of HI is 3.2 moles/1litre
=3.2M
degree of dissociation= 20%
degree of dissociation = no of moles of reactants dissociated/no. of moles of reactants present initially
20/100=x/3.2
x=0.64 moles
according to the reaction
2HI(g)=H2(g)+I2(g)
two M of HI gives one M of H2 and I2 each so .64 M of HI would give .32 M of H2 and I2 each
hence equilibrium concentration of HI is 2.56M
Kc=[0.32][0.32]/[2.56]2
=0.0156
=3.2M
degree of dissociation= 20%
degree of dissociation = no of moles of reactants dissociated/no. of moles of reactants present initially
20/100=x/3.2
x=0.64 moles
according to the reaction
2HI(g)=H2(g)+I2(g)
two M of HI gives one M of H2 and I2 each so .64 M of HI would give .32 M of H2 and I2 each
hence equilibrium concentration of HI is 2.56M
Kc=[0.32][0.32]/[2.56]2
=0.0156