Question

Consider the reaction CO(g) + NH₃(g) ⇌ HCONH₂(g), K = 2.70 at 550 K. If a reaction vessel initially contains only CO and NH₃ at partial pressures of 2.00 bar and 1.80 bar, respectively, what will be the partial pressure of HCONH₂ at equiLiBrium? Express your answer with the appropriate units.

Answer 1

To find the partial pressure of HCONH2 at equilibrium, define x as the change in partial pressure of reactants, set up the equilibrium expression, and solve for x using the initial partial pressures and the quadratic formula or iterative methods.

Step-by-step explanation:

To calculate the partial pressure of HCONH2 at equilibrium for the reaction CO(g) + NH3(g) ⇌ HCONH2(g), we can use the equilibrium constant (K = 2.70) and the initial partial pressures of CO and NH3 (2.00 bar and 1.80 bar, respectively).

Let's define x as the change in partial pressure of CO and NH3 at equilibrium. The change for HCONH2 will be x (since it's a 1:1 ratio).

The equilibrium expression for this reaction is K = P(HCONH2) / (P(CO) × P(NH3))

At equilibrium, the partial pressures will be: P(CO) = 2.00 - x, P(NH3) = 1.80 - x, and P(HCONH2) = x. Plugging these into the equilibrium expression, we get 2.70 = x / ((2.00 - x)(1.80 - x)). Solving for x gives the partial pressure of HCONH2 at equilibrium, which can be found using the quadratic formula or iterative methods.