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memorybuxton
12.12.2019 •
Chemistry
Areaction vessel is charged with hydrogen iodide, which partially decomposes to molecular hydrogen and iodine: 2hi (g) h2(g) + i2(g) when the system comes to equilibrium at 425 °c, phi = 0.708 atm, and ph2 = pi2 the value of kp at this temperature is
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Ответ:
The value of the equilibrium constant:![K_{p} = 0.25](/tpl/images/0414/4415/a3241.png)
Explanation:
Given reaction: 2HI (g) ⇌ H₂(g) + I₂(g)
Number of moles of- HI: n₁ = 2 mole; H₂: n₂ = 1 mole; I₂: n₃ = 1 mole
Total number of moles: n = n₁ + n₂ + n₃ = 2 + 1 + 1 = 4 moles
The equilibrium constant for the given reaction is given as:
Given: Temperature: T = 425 °C = 425 + 273 = 698 K
The partial pressure: pHI = 0.708 atm,
and, pH₂ = pI₂
∵ partial pressure of a given gas: pₐ = Χₐ . P
Here, P is the total pressure
Χₐ is the mole fraction of given gas and is given by the equation
Mole fraction for HI:![\chi_{1} = \frac {n_{1}}{n} = \frac {2}{4} = 0.5](/tpl/images/0414/4415/d2673.png)
Mole fraction for H₂:![\chi_{2} = \frac {n_{2}}{n} = \frac {1}{4} = 0.25](/tpl/images/0414/4415/cec66.png)
Mole fraction for I₂:![\chi_{3} = \frac {n_{3}}{n} = \frac {1}{4} = 0.25](/tpl/images/0414/4415/7ed3f.png)
Thus, Χ₂ = Χ₃ = 0.25
The partial pressure of HI is given by;
pHI = Χ₁ P
0.708 atm = 0.5 × P
⇒ P = 1.416 atm
As the partial pressures: pH₂ = pI₂
∴ pH₂ = pI₂ = Χ₂ P = Χ₃ P = 0.25 × 1.416 atm = 0.354 atm
Therefore, the value of Kp can be calculated as:
Therefore, the value of the equilibrium constant:![K_{p} = 0.25](/tpl/images/0414/4415/a3241.png)
Ответ:
4.46 L
Explanation: By using Charles’s Law, we know that V1/T1=V2/T2. And whenever temperature is involved, you have to convert from Celsius to Kelvin (C° + 273). So, 4.00/ 24 +273 = V2/ 58 + 273. So the answer is, around 4.46 L.