The reaction,$2A_{(g)} + B_{(g)} \rightleftharpoons 3C_{(g)} + D_{(g)}$ is begun 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
  $[(0.75)^3(0.25)] \div [(1.00)^2(1.00)]$
• 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
  $[(0.75)^3(0.25)] \div [(0.75)^2(0.25)]$