Explanation:
Chemical equation for the given reaction is as follows.
[tex]A + 2B \rightarrow C[/tex]
Initial : 0.6 1.30 0.5
Final : (0.6 - x) (1.30 - 2x) (0.5 + x)
It is given that at equilibrium, [A] = 0.410 M.
So, x = (0.600 - 0.410)
= 0.19 M
Hence, [B] will also be calculated as follows.
[B] = [tex]1.30 - (2 \times 0.19)[/tex]
= 0.92
Now, we will calculate the value of equilibrium constant as follows.
[tex]K_{eq} = \frac{[C]}{[A][B]^{2}}[/tex]
= [tex]\frac{0.690}{0.410 \times (0.92)^{2}}[/tex]
= [tex]\frac{0.690}{0.347}[/tex]
= 1.988
Thus, we can conclude that the value of the equilibrium constant, [tex]K_{c}[/tex] is 1.988.
