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In an empty container of $5$ L, kept at $250^oC$, were introduced $1.8$ mol $PCl_5$. Let x be the number of moles of this substance which dissociate until equilibrium is established. - Complete the following table, then introduce the molarities into the expression of the equilibrium constant: - Find x by solving the equation found by that method. - Calculate $[PCl_3]$ at equilibrium.
| $PCl_5$ |  |
$PCl_3$ | + | $Cl_2$ | |
| nb. of moles initially | 1.8 | 0 | 0 | ||
| variation of mole number | -x | ..(1) | ..(2) | ||
| nb. of moles at equil. | ..(3) | ..(4) | ..(5) | ||
| molarities at equil. ($\frac{mol}{L}$) | ..(6) | ..(7) | ..(8) |
$K_c=0.042$ à $250^oC$
.......(9)
.......(10)
.......(11)
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