Question

What volume of oxygen gas, at 30.0ºC and 1.50 atm, is produced when 75.0g of water is electrolyzed? 2H2O --> 2H2 + O2

Answer 1

`"34.55 L"` `"(9.13 gal)"`

Explanation:

`"2H_2 O -----> 2H_2 + O_2`

FROM DATA

Moles of WATER
`"75 g" / "18 g/mol" =` `"4.167 mol of"" H_2O`

Mol of OXYGEN
`O_2 / ("2 "H_2 O") 4.167=` `"2.083 mol of"" O_2`

CALCULATING OXYGEN VOLUME per IDEAL GAS LAW
(Relatively low pressure and temperature)

`V = "nRT"/"P"`

Where,
n: moles
R: Ideal gas constant, (0.0821 L. Atm/mol. L)
T: Temperature. (K)
P: Pressure, (Atm.)

Solving (Volume of Oxygen),

`V = "(2.083)(00821)(273 + 30)"/"1.5"` = `"34.55 L"` `"(9.13 gal)"`