rustalex6045
24.12.2020 •
Chemistry
A quantity of HI was sealed in a tube, heated to 425°C and held at this temperature until
equilibrium was reached. The concentration of Hl in the tube at equilibrium was found to be
0.0706 mol/L. Calculate the equilibirum concentration of H2 (and 12). For the gas-phase
reaction,
H2 + 2 = 2HIKc = 54.6 at 425°C
O a. 1.17 x 10-3M
O b. 2.34 x 10-3M
c. 9.55 x 10-3M
d. 1.85 x 10-4 M
e. 4.78 x 10 PM
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Ответ:
The gas phase concentration of H2 and I2 is 9.55 x 10-3M.
The equation of the reaction is;
H2 + I2 > 2HI
We also have the information that the equilibrium constant of the process is 54.6.
Now recall that;
Kc = 2HI/[H2] [I2]
We can assume that the concentration of H2 = concentration of I2
Hence; [H2] = [I2] = x
54.6 = [0.0706]^2/x^2
54.6x^2 = [0.0706]^2
x = √ [0.0706]^2/54.6
x = 9.55 x 10-3M
Learn more about equilibrium constant: link?
Ответ:
The equilibrium concentration of H₂ : c. 9.55 x 10⁻³ M
Further explanationGiven
Kc = 54.6 at 425°C
The concentration of Hl = 0.0706 mol/L
Required
The equilibrium concentration of H₂ (and I₂)
Solution
[H₂][I₂]=[H₂]²
Ответ:
bdef
Explanation: