To correct the given equation, we need to balance the number of atoms on both sides. The original equation is:
\[ 1N_2 + 4H_2 \rightarrow 2NH_3 + 1H_2 \]
If we look at the products on the right side, we have 2 moles of ammonia (NH3), which requires 2 moles of nitrogen (N) and 6 moles of hydrogen (H), plus 1 mole of leftover diatomic hydrogen (H2).
On the left side, there is only 1 mole of nitrogen (from N2) and 4 moles of hydrogen (from H2), totaling only 4 hydrogen atoms.
Thus, to balance the equation properly, the correct balanced equation should be:
\[ N_2 + 3H_2 \rightarrow 2NH_3 \]
This shows that 1 mole of nitrogen reacts with 3 moles of hydrogen to produce 2 moles of ammonia, with no hydrogen left over.
Given the provided responses, the correct choice would be:
Remove a H2 molecule from both the left and right sides of the equation.
However, the best course of action is clarifying that instead of having leftover hydrogen, we simply need to balance the reactants properly to arrive at the proper stoichiometry.
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