Question

The reaction $2A(g) + B(g) \rightleftharpoons 3C(g) + D(g)$ is began with the concentrations of A and B both at an initial value of 1.00 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
(a) [(0.75)³ (0.25)] $\div$ [(0.75)² (0.25)]
(b) [(0.75)³ (0.25)] $\div$ [(1.00)² (1.00)]
(c) [(0.75)³ (0.25)] $\div$ [(0.50)² (0.75)]
(d) [(0.75)³ (0.25)] $\div$ [(0.50)² (0.25)]

Answer 1

Hello Friend

The answer of u r question is

Option.A

Thank you

Answer 2

${\huge {\mathfrak {Answer :-}}}$

➡️ Option (A)

That's it..