Just for your interest, the reason that K changes with temperature only (at least for ideal gases in this case) is because of this equation: (known as van't Hoff's differential equation)
∂ln K / ∂T = ΔH / RT²
This basically means that the derivative of ln K with respect to temperature is dependent on enthalpy (whether reaction is endothermic or exothermic) and temperature. R is just a constant.
So for example, if the forward reaction is endothermic then ΔH > 0, so the derivative is positive. (remember that dy/dx > 0 means y is increasing whenever x is increasing)
So this, means that ln K is increasing as T (temperature) is increasing i.e. K is increasing with higher temperature; which makes sense because when you increase temperature, the reaction favours the forward direction (endothermic) more and you get an increase in products which results in an increase in K.
That's a taste of university chemistry for you....
