Fundamentals of Equilibrium Concentration Calculation Constants Periodic Table L

Question

Fundamentals of Equilibrium Concentration Calculation Constants Periodic Table Learning Goal To determine equilibrium concentrations from initial condtions The reversible reaction has a reaction quotient Qc defined as XJIY Because the reaction is reactions will occur simultaneously. The reaction will eventually reach equilibrium, at which point the concentrations do not change, and Qc is equal to a constant known as K reversible, both the forward and reverse Figure 1 of 1 Reaction forms products Reaction forms reactants Equilibrium

Explanation / Answer

As the relation between Kc and Qc is already given in the question.

The value of Kc and the initial concentration of the products and reactants is also given in the table which means that-

We just have to calculate Qc of all the three mixtures(A,B,C). We can easily do this by multiplying the concentrations of [X] and [Y] (reactants), and then dividing it by the concentration of [XY]{products).

So,

For mixture A:-

The value of Qc = 0. (As 0/0.1=0)-which means that the value of Qc is less than Kc(Kc=0.150 as given ). So, the reaction will move forward to attain equilibrium fast

For mixture B:-

The value of Qc =0.02.[As (0.100*0.100)/0.500=0.02]-which is less than the value of Kc(Kc=0.150 as given). So, the reaction will move forward just like the mixture A.

For mixture C:-

The value of Qc=0.45[As (0.3*0.3)/0.2=0.45]- which is more than the value of Kc(Kc=0.150 as given). So. the reaction will move backward or in other words it will get reversed

So, finally mixture A and B will have forward reactions and mixture C will have reversed reaction.

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