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Question
To study the decomposition of hydrogen iodide, a student fills an evacuated 3 litre flask with 0.3 mol of HI gas and allows the reaction to proceed at 500°C. At equilibrium he found the concentration of HI which is equal to 0.05 M. Calculate Kc and Kp.
Solution
V = 3 L
`["HI"]_"initial" = (0.3 "mol")/(3"L")` 0.1 M
[HI]eq = 0.05 M
\[\ce{2 HI(g) <=> H2(g) + l_2(g)}\]
| HI (g) | H2 (g) | I2 (g) | |
| Initial concentration | 0.1 | - | - |
| Reacted | 0.05 | - | - |
| Equilibrium concentration | 0.05 | 0.025 | 0.025 |
`"K"_"C" =(["H"_2]["I"_2])/(["HI"]^2)`
`= (0.025 xx 0.025)/(0.05 xx 0.05)` = 0.25
Kp = Kc(RT)(∆ng)
∆ng = 2 – 2 = 0
Kp = 0.25(RT)0
Kp = 0.25.
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