please help

its important
https://imgur.com/0dtxWae

am giving the data of number of moles of the respective species at equilibrium N204=7.3 and NO2=5.4 so clearly N204 has more moles than NO2 but if you increase pressure you will expect the equilibrium to shift to left thats according to mole ratio which says there are fewer moles on reactant side so equilibrium must shift to left but the actual moles of reactant is greater than the product so how is this valid? here is the link to the sample material paper--https://qualifications.pearson.com/content/dam/pdf/International%20Advanced%20Level/Chemistry/2018/Specification-and-Sample-Assessment/International-A-Level-Chemistry-SAMs.pdf

When working out which direction an equilibrium will shift when you change the pressure, you consider the number of mol of particles in the balanced equation (in this case it is a 1:2 ratio), rather than the the number of mol of chemicals present in the equilibrium mixture.

but why is that the case why not consider the actual moles at equilibrium?