Question

What mass of P2O5 would be produced if 0.0590 miles of H2O are produced? please show all work

Answer 1

Answer: The mass of
`P_2O_5` produced in the reaction is 5.56 grams

Step-by-step explanation:

We are given:

Moles of water produced = 0.0590 moles

The chemical equation for the decomposition of phosphoric acid follows:

`2H_3PO_4\rightarrow P_2O_5+3H_2O`

By Stoichiometry of the reaction:

When 3 moles of water are produced, the moles of
`P_2O_5` produced is 1 mole

So, when 0.0590 moles of water are produced, the moles of
`P_2O_5` produced will be
`(1)/(3)* 0.0590=0.0196mol`

To calculate the number of moles, we use the equation:

`\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}`

Molar mass of
`P_2O_5` = 283.89 g/mol

Moles of
`P_2O_5` = 0.0196 moles

Putting values in above equation, we get:

`0.0196mol=\frac{\text{Mass of }P_2O_5}{283.89g/mol}\\\\\text{Mass of }P_2O_5=(0.0196mol* 283.89g/mol)=5.56g`

Hence, the mass of
`P_2O_5` produced in the reaction is 5.56 grams