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Q.

The reaction, $2 A (g) + B (g) ⇌ 3 C (g) + D (g)$ is begun with the concentration of A and B both at an initial value of I .00 M. When equilibrium is reached, the
concentration of D is measured and found to be 0.25 M. The value for the equilibrium constant for this reaction is given by the expression:

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a

$[(0 .75)^{3} (0 .25)] \div [(1 .00)^{2} (1 .00)]$

b

$[(0 .75)^{3} (0 .25)] \div [(0 .50)^{2} (0 .75)]$

c

$[(0 .75)^{3} (0 .25)] \div [(0 .50)^{2} (0 .25)]$

d

$[(0 .75)^{3} (0 .25)] \div [(0 .75)^{2} (0 .25)]$

answer is B.

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Detailed Solution

$\begin{array}{lcc} \underset{At Eq .}{\underset{lnitial}{}} \underset{0 .5}{\underset{1 .0}{2 A (g)}} + \underset{0 .75}{\underset{1 .0}{B (g)}} & ⇌ & \underset{0 .75}{\underset{0}{3 C (g)}} + \underset{0 .25}{\underset{0}{D (g)}} \end{array}$
$K_{c} = \frac{(0 .25) \times (0 .75)^{3}}{(0 .5)^{2} \times (0 .75)}$

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The reaction, 2A(g)+B(g)⇌3C(g)+D(g) is begun with the concentration of A and B both at an initial value of I .00 M. When equilibrium is reached, theconcentration of D is measured and found to be 0.25 M. The value for the equilibrium constant for this reaction is given by the expression: