Question

The reaction, $2 A(g)+B(g) \rightleftharpoons 3 C(g)+D(g)$ 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. $\left[(0.75)^{3}(0.25)\right] \div\left[(1.00)^{2}(1.00)\right]$
• B. $\left[(0.75)^{3}(0.25)\right] \div\left[(0.50)^{2}(0.75)\right]$
• C. $\left[(0.75)^{3}(0.25)\right] \div\left[(0.50)^{2}(0.25)\right]$
• D. $\left[(0.75)^{3}(0.25)\right] \div\left[(0.75)^{2}(0.25)\right]$

Answer 1

Answer: (B)

$\left[(0.75)^{3}(0.25)\right] \div\left[(0.50)^{2}(0.75)\right]$

Answer 2

$K=\frac{(0.75)^{3}(0.25)}{(0.50)^{2}(0.75)}$