Answer:
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Answer:
I not understand your questions
Answer:
Total pressure at equilibrium is 0.2798atm.
Explanation:
For the reaction:
H₂S(g) ⇄ H₂(g) + S(g)
Kp is defined as:
![Kp = \frac{P_{H_{2}}*P_S}{P_{H_{2}S}} = 0.834](https://tex.z-dn.net/?f=Kp%20%3D%20%5Cfrac%7BP_%7BH_%7B2%7D%7D%2AP_S%7D%7BP_%7BH_%7B2%7DS%7D%7D%20%3D%200.834)
If initial pressure of H₂S is 0.150 atm, equilibrium pressures are:
H₂S(g): 0.150atm - x
H₂(g): x
S(g): x
Replacing in Kp:
![\frac{X*X}{0.150atm-X} = 0.834](https://tex.z-dn.net/?f=%5Cfrac%7BX%2AX%7D%7B0.150atm-X%7D%20%3D%200.834)
X² = 0.1251 - 0.834X
X² + 0.834X - 0.1251 = 0
Solving for X:
X = -0.964 → False solution: There is no negative pressures
X = 0.1298
Thus, pressures are:
H₂S(g): 0.150atm - 0.1298atm = <em>0.0202atm</em>
H₂(g): <em>0.1298atm</em>
S(g): <em>0.1298atm</em>
Thus, total pressure in the container at equilibrium is:
0.0202atm + 0.1298atm + 0.1298atm = <em>0.2798atm</em>
Answer:
D
Explanation:
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