K= 6.9x10^10 which way does this dominate to right or left? for equilibrium constant? this is a hw problem i just don't understand

can anybody help me with this?

Remember that Keq = (products)/(reactants). For K to be a very large number (6.9 x 10^10 is a huge number), products must be large and reactants must be small so the reaction dominates on the product side, or if we write the equation as

reactants ==> products, we would say the reaction was far to the right. (Note: The only way you can get a large number out of a fraction is for the numerator to be large and/or the denominator to be small. The only way to get a small number out of a fraction is to have the numerator small and/or the denominator large.)
For a very small number, for example, 1.6 x 10^-10, a VERY small number), then products would be small and reactants would be large and we would say the reaction was far to the left (meaning it hardly reacted at all. If this isn't clear, repost a separate question and give specifics about what you don't understand.

To determine whether a reaction is dominated towards the right or the left based on its equilibrium constant (K) value, you need to compare the value of K to 1.

If K > 1, it means that the products are favored at equilibrium, and the reaction is dominated towards the right.

If K < 1, it means that the reactants are favored at equilibrium, and the reaction is dominated towards the left.

In your case, K = 6.9x10^10. Since this value is much greater than 1, it indicates that the products are favored at equilibrium, and the reaction is dominated towards the right.

Therefore, in this particular reaction, the products are the major species at equilibrium compared to the reactants.