Answer: The mass of [tex]P_2O_5[/tex] produced in the reaction is 5.56 grams
Explanation:
We are given:
Moles of water produced = 0.0590 moles
The chemical equation for the decomposition of phosphoric acid follows:
[tex]2H_3PO_4\rightarrow P_2O_5+3H_2O[/tex]
By Stoichiometry of the reaction:
When 3 moles of water are produced, the moles of [tex]P_2O_5[/tex] produced is 1 mole
So, when 0.0590 moles of water are produced, the moles of [tex]P_2O_5[/tex] produced will be [tex]\frac{1}{3}\times 0.0590=0.0196mol[/tex]
To calculate the number of moles, we use the equation:
[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}[/tex]
Molar mass of [tex]P_2O_5[/tex] = 283.89 g/mol
Moles of [tex]P_2O_5[/tex] = 0.0196 moles
Putting values in above equation, we get:
[tex]0.0196mol=\frac{\text{Mass of }P_2O_5}{283.89g/mol}\\\\\text{Mass of }P_2O_5=(0.0196mol\times 283.89g/mol)=5.56g[/tex]
Hence, the mass of [tex]P_2O_5[/tex] produced in the reaction is 5.56 grams
