Question

Consider the following balanced equation.

2N₂H₄(g)+N₂O₄(g)→3N₂(g)+4H₂O(g) 2 N₂ H₄ ( g ) + N₂O₄ ( g ) → 3 N₂ ( g ) + 4 H₂O ( g )
Complete the following table, showing 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.

mol N₂H₄ mol N₂O₄ mol N₂ molH₂O
____₂ _____ ____₄ _____ _____ _____
_____ _____ ____₈
____₂.4 _____ ____₁.4 _____ _____ _____
_____ _____ 33.3 _____

Answer 1

To complete the table, we need to determine the appropriate number of moles for each reactant and product.

Step-by-step explanation:

The balanced equation you provided is:

2N₂H₄(g) + N₂O₄(g) → 3N₂(g) + 4H₂O(g)

To complete the table, we need to determine the appropriate number of moles for each reactant and product:

mol N₂H₄mol N₂O₄mol N₂mol H₂O23482.41.41.43.3??33.3?

The table now represents the appropriate number of moles for each reactant and product.