Final answer:
To calculate P [NO]eq, a balanced chemical equation is required, followed by an expression of changes in partial pressure (x) due to the reaction's progress. The equilibrium constant Kp is then used to find the value of x, allowing for the determination of P [NO]eq.
Step-by-step explanation:
To calculate the partial pressure of NO (P [NO]eq), given the equilibrium partial pressures of NOCl (P [NOCl]eq) and Cl2 (P [Cl2]eq), along with the equilibrium constant (Kp), we must first write the balanced chemical equation for the reaction:2 NOCl(g) <=> 2 NO(g) + Cl2(g)Assuming that the reaction starts with NOCl dissociating into NO and Cl2, and that the change in NOCl's partial pressure (x) is the same as the change in NO's partial pressure (since they dissociate in a 1:1 ratio), we can express the equilibrium partial pressures as follows:
- P [NOCl]eq = initial P [NOCl] - x
- P [NO]eq = initial P [NO] + x (since NO is forming, and we start with none)
- P [Cl2]eq = initial P [Cl2] + x/2 (since Cl2 forms at half the rate of NO from NOCl)
Given that P [NOCl]eq = 0.33 atm and P [Cl2]eq = 0.50 atm, we express the equilibrium expression for Kp as:Kp = (P [NO]^2 * P [Cl2]) / P [NOCl]^2Substituting the known values and solving for x, we get:Kp = (0.33 - x)^2 / (0.50 + x/2)^2 = 1.9 x 10^-2After solving the quadratic equation we find the value of x, and consequently, P [NO]eq = initial P [NO] + x.