## General Chemistry: Principles and Modern Applications (10th Edition)

$$P = 12.0 \space atm$$
1. Find the concentration: $$\frac{0.186 \space mol}{2.16 \space L} = 0.0861 \space M$$ 2. The exponent of each concentration is equal to its balance coefficient. $$K_C = \frac{[Products]}{[Reactants]} = \frac{[ NH_3 ][ CO ]}{[ HCONH_2 ]}$$ 3. At equilibrium, these are the concentrations of each compound: $[ HCONH_2 ] = 0.186 \space M - x$ $[ NH_3 ] = 0 \space M + x$ $[ CO ] = 0 \space M + x$ $$4.84 = \frac{( x)( x)}{(0.186 - x)}$$ 4. Solve for x: x = 0.179 $[ HCONH_2 ] = 0.007 \space M$ $[ NH_3 ] = 0.179 \space M$ $[ CO ] = 0.179 \space M$ 5. Find the total amount of moles of gas: $$n_{total} = (0.007 + 0.179 + 0.179) \times 2.16 = 0.788$$ 6. Find the pressure using pv = nrt: $$P = \frac{nRT}{V} = \frac{(0.788)(0.0821)(400)}{2.16} = 12.0 \space atm$$