You should verify the relationship by checking one of the previous examples. In the HCl reaction (298) = -45.54 kcal per 2 moles of HCl. Then,

= 10 = 2.5 x 10

This tallies with the value of quoted previously, which is necessarily so since this is how the value was obtained originally. For many reactions with extremely large or small equilibrium constants, it is easier and more accurate to measure the free energy change of the reaction and use the equations given above, than to try to obtain from concentration measurements at equilibrium.
At temperatures other than 298K, the 1.364 factor cannot be used. For the ammonia reaction at 1000K:






This was the value of quoted previously. Note that (1000) was expressed in calories instead of kilocalories because R is in calories per degree per mole.