Answer:
pCH₄ = 105.1 - 0.42 = 104.68 torr
pI₂ = 7.96 -0.42 = 7.54 torr
pCH₃I = 0.42 torr
pHI = 0.42 torr
Explanation:
Kp is the equilibrium constant for the partial pressure of the gases in the reaction, and it is calculated for a general equation:
aA(g) + bB(g) ⇄ cC(g) + dD(g)
, where p is the partial pressure in the equilibrium. By the reaction given:
CH₄(g) + I₂(g) ⇄ CH₃I(g) + HI(g)
105.1 torr 7.96 torr 0 0 <em> initial partial pressure</em>
-x -x +x +x <em> react</em>
105.1-x 7.96-x x x <em>equilibrium</em>
Then:
![Kp = \frac{pCH3IxpHI}{pCH4xpI2} = \frac{x^2}{(105.1-x)(7.96-x)}](https://tex.z-dn.net/?f=Kp%20%3D%20%5Cfrac%7BpCH3IxpHI%7D%7BpCH4xpI2%7D%20%3D%20%5Cfrac%7Bx%5E2%7D%7B%28105.1-x%29%287.96-x%29%7D)
![2.26x10^{-4} = \frac{x^2}{836.596 - 113.06x -x^2}](https://tex.z-dn.net/?f=2.26x10%5E%7B-4%7D%20%3D%20%5Cfrac%7Bx%5E2%7D%7B836.596%20-%20113.06x%20-x%5E2%7D)
x² = 0.1891 - 0.0255x -2.26x10⁻⁴x²
0.9997x² + 0.0255x - 0.1891 = 0
Using Bhaskara's rule:
Δ = (0.0255)² - 4x(0.9997)x(-0.1891)
Δ = 0.7568
![x = \frac{-b+/-\sqrt{0.7568} }{2a} = \frac{-0.0255 +/-0.8699}{1.9994}](https://tex.z-dn.net/?f=x%20%3D%20%5Cfrac%7B-b%2B%2F-%5Csqrt%7B0.7568%7D%20%7D%7B2a%7D%20%3D%20%5Cfrac%7B-0.0255%20%2B%2F-0.8699%7D%7B1.9994%7D)
Using only the positive term, x = 0.42 torr.
So,
pCH₄ = 105.1 - 0.42 = 104.68 torr
pI₂ = 7.96 -0.42 = 7.54 torr
pCH₃I = 0.42 torr
pHI = 0.42 torr