(Solved): Question 1-4 1. Initially, we place 2mol of A and 4mol of B in a 0.5L flask. At equilibrium, ...

1. Initially, we place $2\mathrm{mol}$ of $A$ and $4\mathrm{mol}$ of $B$ in a $0.5\mathrm{L}$ flask. At equilibrium, the flask contains $0.3\mathrm{mol}$ of $C$. Determine the value of $K$. ${\mathrm{A}}_{(9)}+{\mathrm{B}}_{(9)}\rightleftharpoons 3{\mathrm{C}}_{(9)}+2{\mathrm{C}}_{(9)}$ 2. A system is represented by the following equation: $2{\mathrm{A}}_{(39)}+{\mathrm{B}}_{(39)}\rightleftharpoons 3{\mathrm{C}}_{(30)}$ At equilibrium, $[C]=0.6\mathrm{M}$. Calculate the value of $\mathrm{K}$ if initially $1\mathrm{mol}$ of $A$ and $2\mathrm{mol}$ of $B$ were placed in a $1\mathrm{L}$ flask. 3. In a $500\mathrm{mL}$ flask, we put $6\mathrm{mol}$ of $A,6\mathrm{mol}$ of $B,4$ moles of $C$ and $9\mathrm{mol}$ of $D$. The value of $\mathrm{K}$ is 17.3 . Is the system in equilibrium? If not, in which direction will the reaction proceed to attain equilibrium? ${\mathrm{A}}_{(9)}+2{\mathrm{B}}_{(0)}\rightleftharpoons 2{\mathrm{C}}_{(9)}+{\mathrm{D}}_{(9)}$ 4. $5.6\times 10^{-6}\mathrm{mol}$ of $A$ and $5\times 10^{-5}\mathrm{mol}$ of $B$ are mixed in a $200\mathrm{mL}$ flask. The system is represented by the equation: $2A_{(0)}+B_{(0)}\rightleftharpoons 3C_{(0)}$ At equilibrium, there is $4.8\times 10^{-5}\mathrm{mol}$ of $B$. Calculate the value of the equilibrium constant.