A quantity of HI was sealed in a tube, heated to 425C, and held at this temperature until
equilibrium is reached. The concentration of HI in the tube at equilibrium was found to be
0.0706 moles/liter. Calculate the equilibrium concentration of H2 (and I2 ). For the reaction H2
(g) + I2 (g) 2HI(g), Kc = 54.6 at 425C.
I don\'t know how to work this without the initial [HI]. Please explain the answer.
Solution
Kc=[2HI]^2/[I2][H2]
BUT [I2]=[H2]
=>54.6=0.0706^2/[h2]^2
[H2]^2=9.128*10^-5
[H2]=[I2]=SQRT9.128*10^-5
=9.55*10^-3MOLES/LITRE.
A quantity of HI was sealed in a tube, heated to 425C, and held at t.pdf
1. A quantity of HI was sealed in a tube, heated to 425C, and held at this temperature until
equilibrium is reached. The concentration of HI in the tube at equilibrium was found to be
0.0706 moles/liter. Calculate the equilibrium concentration of H2 (and I2 ). For the reaction H2
(g) + I2 (g) 2HI(g), Kc = 54.6 at 425C.
I don't know how to work this without the initial [HI]. Please explain the answer.
Solution
Kc=[2HI]^2/[I2][H2]
BUT [I2]=[H2]
=>54.6=0.0706^2/[h2]^2
[H2]^2=9.128*10^-5
[H2]=[I2]=SQRT9.128*10^-5
=9.55*10^-3MOLES/LITRE
![A quantity of HI was sealed in a tube, heated to 425C, and held at this temperature until
equilibrium is reached. The concentration of HI in the tube at equilibrium was found to be
0.0706 moles/liter. Calculate the equilibrium concentration of H2 (and I2 ). For the reaction H2
(g) + I2 (g) 2HI(g), Kc = 54.6 at 425C.
I don't know how to work this without the initial [HI]. Please explain the answer.
Solution
Kc=[2HI]^2/[I2][H2]
BUT [I2]=[H2]
=>54.6=0.0706^2/[h2]^2
[H2]^2=9.128*10^-5
[H2]=[I2]=SQRT9.128*10^-5
=9.55*10^-3MOLES/LITRE](https://image.slidesharecdn.com/aquantityofhiwassealedinatubeheatedto425candheldatt-230708181452-6f15ff32/85/A-quantity-of-HI-was-sealed-in-a-tube-heated-to-425C-and-held-at-t-pdf-1-320.jpg)
