Phosphorous pentachloride decomposes according to the reaction PCl5(g)=PCl3(g)+Cl2(g)

A 12.3 g sample of PCl5 is added to a sealed 1.50 L flask and the reaction is allowed to come to equilibrium at a constant temperature. At equilibrium, 31.8% of the PCl5 remains. What is the equilibrium constant, Kc, for the reaction?

Question is asking for Kc

The equilibrium constant, , for the reaction is 0.061.

Explanation:

Initial concentration of  =  

Equilibrium concentration of =  

The given balanced equilibrium reaction is,

Initial conc.              0.039 M                0 M        0 M

At eqm. conc.     (0.039-x) M              (x) M   (x) M

Given : (0.039-x) = 0.012

x = 0.027

The expression for equilibrium constant for this reaction will be,

Now put all the given values in this expression, we get :

The equilibrium constant, , for the reaction is 0.061.

n2(g) + 3h2-> 2nh3(g)   this is the balanced equation

note the mole ratio between n2, h2 and nh3.   it is 1 : 3 : 2   this will be important.

moles n2 present = 28.0 g n2 x 1 mole n2/28 g = 1 mole n2 present

moles h2 present = 25.0 g h2 x 1 mole h2/2 g = 12.5 moles h2 present

based on mole ratio, n2 is limiting in this situation because there is more than enough h2 but not enough n2.

moles nh3 that can be produced = 1 mole n2 x 2 moles nh3/mole n2 = 2 moles nh3 can be produced

grams of nh3 that can be produced = 2 moles nh3 x 17 g/mole = 34 grams of nh3 can be produced

note:   the key to this problem is recognizing that n2 is limiting, and therefore limits how much nh3 can be produced.

a. they are both space stations

happy to

pls mark as brainliest.