For each of the following, write the chemical equation with appropriate equilibrium arrows, as shown in Table 5.

Question

Table 5:
No reaction: <1% ↔
Reactants favoured: <50%↔
Products favoured: >50%↔
Quantitative:>99%↔ or ➡️

a) The Haber process is used to manufacture ammonia fertilizer from hydrogen and nitrogen gases. Under less than desirable conditions, only 1% yield of ammonia is obtained at equilibrium.

Okay so, this is the equation I made:
3H2+N2↔️2NH3

When it says "less desirable conditions", does that mean that the equation I made should be in reverse like: 2NH3↔️3H2+N2 ? Since it's less than desirable, does that mean that it would be <50%↔️? But for the reactants or the products? My workbook says "the larger the K the more products are present at equilibrium, conversely, the smaller K the more reactants are present at equilibrium"... But I don't have any amounts to put into an ICE table. I'm honestly not even sure what it's asking. I'd really appreciate the help!