Consider the following reaction in which all reactants and products are gases. 1.00 mol of A and 2.00 mol of B are placed in a 5.0-liter container. After equilibrium has been established, 0.50 mol of D is present in the container. Calculate the equilibrium constant, Kc, for the reaction.

The equilibrium constant for this reaction is = 1.25

Explanation:

The equation for this reaction is:

A + B → D

A = 1.0mol ⇒  {A}=1.0 mol/5.00 L = 0.2 M

B = 2.0 mol ⇒ [B] = 2.0 mol/5.00 L= 0.4 M

D = 0.5 mol ⇒ [D] = 0.5 mol/5.00 L = 0.1 M

= =1.25

The equilibrium constant for this reaction is = 1.25

"you start with 15.67 g mgco3-xh2o, when heated and all the water is removed, you are left with 7.58 g mgco3 only.

therefore, you had 15.67 - 7.58 = 8.09g h2o  

moles of each :

7.58g mgco3 = ? moles = 7.58g / 83.4g/mole = 0.09moles  

8 09g h2o = ? moles = 8.09g / 18g/mole = 0.44moles  

molar ratio between the two by dividing both numbers by the smallest number :

0.09 / 0.09 = 1  

0.44 / 0.09 = 4.8  

mgco3-5h2o"

thats how its supposed to be