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Question: At 500 K the equilibrium constant for the reaction \(\mathrm { H } _ { 2 ( \mathrm {~g} ) } + \mat...

At 500 K the equilibrium constant for the reaction

H2( g)+I2( g)\mathrm { H } _ { 2 ( \mathrm {~g} ) } + \mathrm { I } _ { 2 ( \mathrm {~g} ) } is 24.824.8 .

If 12\frac { 1 } { 2 }mol/L of HI is present at equilibrium, what are the concentrations of H2\mathrm { H } _ { 2 }and assuming that we started by taking HI and reached the equilibrium at 500 K ?

A

0.068 mol L−10.068 \mathrm {~mol} \mathrm {~L} ^ { - 1 }

B

1.020 mol L−11.020 \mathrm {~mol} \mathrm {~L} ^ { - 1 }

C

0.10 mol L−10.10 \mathrm {~mol} \mathrm {~L} ^ { - 1 }

D

1.20 mol L−11.20 \mathrm {~mol} \mathrm {~L} ^ { - 1 }

Answer

0.10 mol L−10.10 \mathrm {~mol} \mathrm {~L} ^ { - 1 }

Explanation

Solution

: H2( g)+I2( g)\mathrm { H } _ { 2 ( \mathrm {~g} ) } + \mathrm { I } _ { 2 ( \mathrm {~g} ) }

Initial conc. 1 0 0

At equilibrium 0.50.5 x x

or or

X =