Question

Does this reaction favor the products, reactants or neither?

Consider the chemical equation below.
2 NO2(g)⇌ N2O4(g)
The equilibrium constant for this chemical reaction at a certain temperature and pressure is Kc = 85.
Determine if the reaction favors the products, reactants, or neither.

Please explain this answer to me please!

Answer 1

Well, it CLEARLY favours the products....

Explanation:

Why....?

We gots...`2NO_2(g)rightleftharpoonsN_2O_4(g)`

...for which...`K_c=([N_2O_4])/([NO_2(g)]^2)=85`

Now..CLEARLY, given the value of `K_c`, the numerator must be numerically large with respect to the denominator...and so in this scenario....the equilibrium favours the PRODUCTS... Claro? If no, raise an objection, and someone will try to address it..

Answer 2

Alright, Kc being greater than 1 means that the relative product concentration is greater than the relative reactant concentration...therefore the reaction favors the products.

Explanation:

`Kc= [ P. concentration]^x / [R. concentration]^y`

Since the numerator would have to be greater than the denominator in this case to yeild answer greater than 1, therefore the relative product concentration would have to be greater than that of reactants. So therefore, in the state that this equation is the products are favored.