Question

PLEASE ANSWER QUICKLY!

How many grams of H3PO4 are produced when 12.81 moles of water react with an excess of P4O10?
Select one:
a. 837
b. 1880
c. 471
d. 8.54

Answer 1

c

c

Step-by-step explanation:

`h3po4 + 12.81 - p40.10`

Answer 2

A. 837 grams of
`H_3PO_4` are produced when 12.81 moles of water react with an excess of
`P_4O_(10)`

Step-by-step explanation:

The balanced chemical equation is

`P_4 O_10  + 6 H_2 O > 4 H_3 PO_4`

Mole ratio of
`H_2 O:H_3 PO_4` is 6 : 4 or 3 : 2

As per the Equation

6 moles of water produces 4 moles of Phosphoric acid

So let us convert

12.81 moles
`H_2 O` to moles
`H_3 PO_4` by using mole ratio and then to mass
`H_3 PO_4` by multiplying with molar mass
`H_3 PO_4`

`12.82 mol H_2 O * \frac {(4mol H_3 PO_4)}{(6molH_2 O)} * \frac {(98gH_3 PO_4)}{(1mol H_3 PO_4 )}`

`=837g H_3 PO_4` is produced

Please note:

Molar mass is the mass of 1 mole of the substance and its unit is g/mol

We find the molar mass by adding the atomic mass of the atoms present in it.

For example
`H_3  PO_4` contains 3 atoms of H, 1 atom of P and 4 atoms of O

So the molar mass

`=(3*1.008)+(31*1)+(4*16)=98 g/mol`