Question

Can some explain this using ice table?? If `K_c` at this temperature is `0.877`, then in which direction (left or right) will the reaction shift to reach equilibrium?

At high temperatures, dinitrogen tetroxide gas decomposes into nitrogen diioxide gas. At `500^@ "C"`, a sealed vessel initially contained `"8.03 M"` of dinitrogen tetroxide gas and `"3.95 M"` nitrogen dioxide gas?

Answer 1

Don't need an ICE table - just the reaction quotient, `Q`

Explanation:

Since you only need to know the direction of the reaction, all you have to do is use `Q` and calculate the value - then compare to `K`.

`Q = ([NO_2]^2)/([N_2O_4])`

`= 3.95^2/8.03`

`= 1.95`

This value of Q is larger than the value of K, which means that you have too many products in the initial conditions.

As a result, the reaction will proceed to the left in order to produce more reactants and less products...so you can get to the equilibrium value and `Q = K` at that point.