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 1.60 bar and 2.00 bar, respectively, what will be the partial pressure of HCONH₂ at equiLiBrium?

Answer 1

To find the partial pressure of HCONH₂ at equilibrium, use an ICE table to set up the equilibrium expression and solve for x using the given initial partial pressures of CO and NH₃. Substitute the value of x into the equilibrium expression to find the partial pressure of HCONH₂ at equilibrium.

Step-by-step explanation:

Given the reaction CO(g) + NH₃(g) ⇌ HCONH₂(g) with equilibrium constant K = 2.70, we can determine the partial pressure of HCONH₂ at equilibrium using the given initial partial pressures of CO and NH₃.

Step 1: Construct an ICE table:

CompoundInitial (bar)Change (bar)Equilibrium (bar)CO1.60-x1.60 - xNH₃2.00-x2.00 - xHCONH₂0+xx

Step 2: Write the expression for K in terms of the equilibrium partial pressures:

K = (HCONH₂) / (CO)(NH₃)

Step 3: Substitute the values into the expression:

2.70 = x / ((1.60 - x)(2.00 - x))

Step 4: Solve for x using the quadratic equation or an approximation method.

Step 5: Substitute the value of x into the equilibrium expression to calculate the partial pressure of HCONH₂ at equilibrium.