Question

According to the following reaction, how many grams of water are required for the complete reaction of 31.2 grams of diphosphorus pentoxide?

Answer 1

The reaction indicates that 63.99 grams of water are required for the complete reaction of 31.2 grams of diphosphorus pentoxide.

Step-by-step explanation:

In the given reaction, the stoichiometric coefficients represent the mole ratio between diphosphorus pentoxide
`(\(P_2O_5\)) and water (\(H_2O\)).`The balanced chemical equation for the reaction is:

`\[ P_2O_5 + 6H_2O \rightarrow 4H_3PO_4 \]`

This equation indicates that one mole of
`\(P_2O_5\)` reacts with six moles of
`\(H_2O\). To find the molar mass of \(P_2O_5\)`, we add the atomic masses of two phosphorus atoms and five oxygen atoms:

`\[ 2 * \text{P} + 5 * \text{O} = 2 * 30.97 + 5 * 16.00 = 62 + 80 = 142 \, \text{g/mol} \]`

Now, we can set up a proportion to find the grams of water required for 31.2 grams of \(P_2O_5\):

`\[ \frac{31.2 \, \text{g}}{1} * \frac{6 \, \text{mol}}{1 \, \text{mol}} * \frac{18.02 \, \text{g}}{1 \, \text{mol}} = 63.99 \, \text{g} \]`

Therefore, 63.99 grams of water are required for the complete reaction of 31.2 grams of diphosphorus pentoxide based on the stoichiometry of the balanced chemical equation.