[Kaleyrvt]

Consider the equilibrium reaction:
   A (g) 2B (g)  +  C (g)

When 1.00 mol of A is placed in a 4.00 L container at temperature t, the concentration of C at equilibrium is 0.050 mol/L. What is the equilibrium constant for the reaction at temperature t ?

again, having troubles with this equillibrium stuff-If someone could please just point me in the proper direction that would be great. I know the equilibrium constant is:
Ke=[C}c[D]d / [A]ab           but how do I input all of this data?

Sorry guys, I am trying Any hints would be greatly appreciated

[Borek]

First of all - rewrite Ke so that it contains substances and coefficients present in your reaction equation.

Secodd: use reaction stoichiometry to calculate amounts of substances in the equilibrium. How much A was destroyed if there is 0.050 C produced? How much B was produced at the same time?

[Yggdrasil]

Also note that since you are working with gases, you will need to use partial pressures instead of concentrations in calculating K_e.

[xiankai]

the letters in brackets stand for the partial pressure/concentration of that substance.

the letters outside the brackets are the number of moles.

it should have looked more like [A]^a, where a is the power of [A].

also, the products belong to the numerator (at the top), while the reactants belong to the denominator (at the bottom).

[Kaleyrvt]

so then,  Ke= 2+[C]
                              [A]


does [A]=0.25 mol/L   and [C]=0.050 mol/l    is that right?? how do I find B???

[Kaleyrvt]

Anybody have any tips??
 

[Yggdrasil]

From the stoichiometry of the reaction, you know that for every molecule of C formed, two molecules of B are formed.

[Kaleyrvt]

A= 0.25 mol/L
B=0.050 mol/L
C=2 x 0.050 =0.1 mol/L

Ke =    [C]   =     [0.1][0.050]   = 0.02   
                   [A]               [0.25]      

Thus, the equilibrium constant is 0.02 at temperature t.