Consider the following equilibrium 4NH_2(g) + 3O_2(g) 2N_2(g) + 6H_2o(l), where

Question

Consider the following equilibrium 4NH_2(g) + 3O_2(g) 2N_2(g) + 6H_2o(l), where delta H = -1530.4 kJ The discussion of ammonia can be reduced by decreasing the temperature of the system. increasing the pressure of the system. decreasing the temperature and decreasing the volume of the system. increasing the temperature and increasing the volume of the system. Look at the following system. PCL_5(g) PCL_3(g) + Cl_2(g) Suppose that the equilibrium constant, K_p, is 490(at 340 degree C). If the partial pressure of PCL_3 is 1.87 atm and the partial pressure of Cl_2 is 0.29 atm, what is the partial pressure of Pcl_5? 1.58 atm 0.0022 atm 0.0011 atm 3.16 times 10^4 atm

Explanation / Answer

I have a little doubt with the first question, so I'm gonna answer the second:

PCl5(g) -------> PCl3(g) + Cl2(g)

Kp = pPCl3 pCl2 / pPCl5

pPCl5 = pPCl3 * pCl2 / Kp

pPCl5 = 1.87 * 0.29 / 490

pPCl5 = 1.11x10-3 or simply 0.00111 atm

Hope this helps. If there's something you need more explanation or something to be fixed tell me in a comment.

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