The equilibrium constant, Kp, for the following reaction is 10.5 at 350 K: 2CH2Cl2(g) CH4(g) CCl4(g) Calculate the equilibrium partial pressures of

The complete question is as follows: The equilibrium constant, Kp, for the following reaction is 10.5 at 350 K: 2CH2Cl2(g) CH4(g) + CCl4(g) Calculate the equilibrium partial pressures of all species when CH2Cl2(g) is introduced into an evacuated flask at a pressure of 0.968 atm at 350 K. PCH2Cl2 = atm PCH4 = atm PCCl4 = atm

The equilibrium partial pressures of all species, that is, , and is 0.420 atm, 0.420 atm and 0.128 atm.

Explanation:

For the given reaction equation, the initial and equilibrium concentration of involved species is as follows.

Initial:                0.968 atm         0               0

Equilibrium:  (0.968 - 2x)           x                x

Now, for this reaction is as follows.

Thus, we can conclude that the equilibrium partial pressures of all species, that is, , and is 0.420 atm, 0.420 atm and 0.128 atm.

conduction is the transfer of thermal energy (heat in transfer) due to collisions between the molecules in the object. collisions between adjacent atoms and molecules transfer kinetic energy from the warmer to the cooler object. the objects must be in physical contact.