Finding K Value

[505671751]

On textbook problem 5I.7, it states , "If Q=1.0 for the reaction N[2](g) + O[2] (g) 2NO (g) @ 25C will the reaction have a tendency to form products or reactants, or will it be at equilibrium?

My question is how would you find the K value in this scenario? (more generally, how do you find the value of K when no concentration values are given)

[Armaan Judge 3L]

You would have to use the formula relating K to the Gibbs Free Energy of the reaction, which is:


I think you'd have to check the appendix for the exact Gibbs Free Energy value for the formation of nitric oxide and then solve for K from there (using the ideal gas constant R and the temperature in Kelvin), but this problem wasn't assigned on the syllabus, so I think we don't need to worry about it for now.