Answer to Question #99506 in General Chemistry for Hailee

Question

A 4.00 L flask was filled with 12.00 mol of SO2 and 2.00 mol of NO2. After equilibrium was reached, it was found that 11.30 mol of NO was present. Calculate the value of all the equilibrium concentrations and calculate the value of Kc.

Answer 1

$$SO_2 + NO_2 \leftrightarrow NO + SO3$$

$c=\frac{n}{V}$

$c_{initial} (SO2) = \frac{12.00}{4.00} = 3.00 \frac{mol}{L}$

$c_{initial}(NO_2) = \frac{12.00}{4.00} = 3.0 \frac{mol}{L}$

$c_{eq}(NO) = \frac{11.30}{4.00}= 2.825\frac{mol}{L}$

$SO_2$ + $NO_2$ $\leftrightarrow$ $NO$ + $SO_3$

I: 3.00 3.00 0 0

C: -2.825 -2.825 +2.825 +2.825

E: 0.175 0.175 2.825 2.825

$$K_c = \frac{[NO][SO_3]}{[SO_2][NO_2]} = \frac{2.825\times2.825}{0.175\times0.175} = 261$$