1. Tardigrade
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  3. Chemistry
  4. 10 moles of A2 , 15 moles of B2 and 5 moles of AB are placed in a 2 litre vessel and allowed the come to equilibrium. The final concentration of AB is 10.5 M , mathrmA2( mathrm~g)+ mathrmB2( mathrm~g) leftharpoons 2 mathrmAB( mathrmg) Determine the value of equilibrium constant (KC) for the reaction.

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Q. $10$ moles of $A_{2}$ , $15$ moles of $B_{2}$ and $5$ moles of $AB$ are placed in a $2$ litre vessel and allowed the come to equilibrium. The final concentration of $AB$ is $10.5 \, M$ ,

$\mathrm{A}_2(\mathrm{~g})+\mathrm{B}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{AB}(\mathrm{g})$

Determine the value of equilibrium constant $\left(K_{C}\right)$ for the reaction.

NTA AbhyasNTA Abhyas 2020Equilibrium

Solution:

Solution

$\frac{5 + 2 x}{2}=10.5$ $; \text{x} = 8$

$K_{C}=\frac{\left(\left[\right. A B \left]\right.\right)^{2}}{\left[A_{2}\right] \left[B_{2}\right]}=\frac{\left(\frac{5 + 2 x}{2}\right)^{2}}{\left(\frac{10 - x}{2}\right) \left(\frac{15 - x}{2}\right)}=\frac{\left(\right. 21 \left.\right)^{2}}{2 \times 7}=31.5$