For reactions in solution, molar concentrations are usually used in equilibrium constant
expressions (designated by K or Kc). In gases, partial pressures can also be used (designated
by Kp). Equilibrium partial pressures of NOCl, NO and Cl2 in a container at 300 K are 1.2
atm, 0.050 atm and 0.30 atm, respectively. Calculate a value for the equilibrium constant Kp
for the following reaction.
2 2NO (g) + Cl (g) � 2NOCl (g)
I found K =1920
my question is whether the temperature is being used at all and if it is why?
My calculator is broken so I can't check your calculation; however, no the temperature is not being used EXCEPT that the value for Kp calculated is at 300 K and no other temperature. Kp and Kc change with T.
To calculate the equilibrium constant Kp for the given reaction, we need to first write the balanced chemical equation:
2NO (g) + Cl2 (g) → 2NOCl (g)
The equilibrium constant expression for this reaction in terms of partial pressures is:
Kp = (PNOCl)^2 / (PNO)^2 * (PCl2)
Where PNOCl, PNO, and PCl2 represent the equilibrium partial pressures of NOCl, NO, and Cl2, respectively.
Given that the equilibrium partial pressures of NOCl, NO, and Cl2 are 1.2 atm, 0.050 atm, and 0.30 atm respectively, we can substitute these values into the equation to calculate Kp.
Kp = (1.2)^2 / (0.050)^2 * (0.30)
Simplifying the calculation:
Kp = 36 / 0.0025 * 0.30
Kp = 36 * 120
Kp = 4320
Therefore, the equilibrium constant Kp for the given reaction is 4320.