Question

For the preceding question, which of the following equations best

represents the reaction?

${\mathbf{\text{a.6N}}}_{\mathbf{2}}\mathbf{+}\mathbf{6}{\mathbf{H}}_{\mathbf{2}}\to \mathbf{4}{\mathbf{NH}}_{\mathbf{3}}\mathbf{+}\mathbf{4}{\mathbf{N}}_{\mathbf{2}}$

${\mathbf{\text{b.N}}}_{\mathbf{2}}\mathbf{+}{\mathbf{H}}_{\mathbf{2}}\to {\mathbf{NH}}_{\mathbf{3}}$

$\mathbf{\text{c.N+3H}}\text{→}{\mathbf{\text{NH}}}_{\mathbf{3}}$

${\mathbf{\text{d.N}}}_{\mathbf{2}}\mathbf{+}\mathbf{3}{\mathbf{H}}_{\mathbf{2}}\to \mathbf{2}{\mathbf{NH}}_{\mathbf{3}}$

${\mathbf{\text{e.2N}}}_{\mathbf{2}}\mathbf{+}\mathbf{6}{\mathbf{H}}_{\mathbf{2}}\to \mathbf{4}{\mathbf{NH}}_{\mathbf{3}}$

Justify your choice. For those you did not choose, explain why they are incorrect.

Short answer

Equation${\text{d.N}}_2+3H_2\to 2N{H}_3$best represents the reaction.

Step-by-step solution

Representation of reaction (a)

This is incorrect. In the ammonia formation, there should not be any leftover nitrogen as the product. It cannot be reduced.

Representation of reaction (b)

There is no balance in the equation. It is not the best representation of the reaction.

Representation of reaction (c)

This is not the best representation. The equation is correctly balanced and contains hydrogen and nitrogen.

Representation of reaction (d)

In the lowest reduced form, it is correctly balanced. It also includes correct products and reactants.

Representation of reaction (e)

This is not the best representation. It is the same as equation (d)where coefficients of product and reactants are twice that of equation (d). It can be reduced by dividing the coefficients by 2.

Hence, the correct answer is an option (d).