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Consider the following balanced equation:

[tex]\[2 N_2H_4(g) + N_2O_4(g) \rightarrow 3 N_2(g) + 4 H_2O(g)\][/tex]

Complete the following table by filling in the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, as well as the moles of each product formed. If the number of moles of a product is provided, fill in the required amount of each reactant to make that amount of product, as well as the amount of the other product that is made.

[tex]\[
\begin{tabular}{|l|l|l|l|}
\hline
Mol $N_2H_4$ & Mol $N_2O_4$ & Mol $N_2$ & Mol $H_2O$ \\
\hline
4 & & & \\
\hline
& 5 & & \\
\hline
& - & & 18 \\
\hline
4.5 & - & & \\
\hline
& 4.5 & - & \\
\hline
& & 11.8 & \\
\hline
\end{tabular}
\][/tex]

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