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In an empty container of $2$ L, kept at $25^oC$, were introduced $0.1$ mol $N_2O_4(g)$ . Let x be the number of moles of $N_2O_4(g)$ which dissociate until equilibrium is established. - Complete the following table, then introduce the molarities into the expression of the equilibrium constant: - Calculate all the molarities at equilibrium. - Calculate the percentage up to which $N_2O_4(g)$ is dissociated.
| $N_2O_{4(g)}$ |  |
$2NO_{2(g)}$ | |
| nb. of moles initially | 0,1 | 0 | |
| variation of mole nb. | -x | ..(1) | |
| nb. of moles at equil. | ..(2) | ..(3) | |
| molarities at equil. ($\frac{mol}{L}$) | ..(4) | ..(5) |
$K_c=0,0058$ à $25^oC$
.......(6)
.......(7)
.......(8)
.......(9)
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