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

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!

The initial equation you provided, 3H2 + N2 ↔ 2NH3, is correct for the Haber process. However, the information that only a 1% yield of ammonia is obtained at equilibrium indicates that the reaction heavily favors the reactants, hydrogen and nitrogen gases.

In the context of chemical equilibrium, the equilibrium arrows indicate the relative concentrations of reactants and products at equilibrium. The symbols < and > represent the direction in which the equilibrium is shifted, while the percentage values indicate the extent to which the chemical species are present. Reactants favored (<50% ↔) means that the reactants are in higher concentration, and products favored (>50% ↔) means that the products are more abundant at equilibrium.

Considering that the yield of ammonia is only 1%, the reaction heavily favors the reactants. Therefore, the correct chemical equation with appropriate equilibrium arrows for the Haber process under these less favorable conditions is:

2NH3 ↔ 3H2 + N2

This represents a reactant-favored equilibrium since the reactants are present in significantly higher amounts.

The Haber process equation you provided, 3H2 + N2 ↔ 2NH3, is correct. In this equation, hydrogen and nitrogen gases react to form ammonia.

When it says "less desirable conditions," it means that the reaction does not proceed efficiently, resulting in a lower yield of ammonia at equilibrium. In this case, only 1% yield of ammonia is obtained.

To determine the direction of the equilibrium reaction and whether reactants or products are favored, we can look at the yield of ammonia. Since the yield is only 1%, it indicates that the equilibrium lies heavily towards the reactants (hydrogen and nitrogen gases).

Based on Table 5, we can label the reaction arrow as <50% ↔. This means that the reaction is not favorable in the forward direction (towards products) and is biased towards the reactants.

Therefore, the equation should be written as:

2NH3 ↔ 3H2 + N2 (reactants favored: <50% ↔)

Hope this helps! Let me know if you have any further questions.