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

1 Answer
Mar 16, 2018

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

Explanation:

"2H_2 O -----> 2H_2 + O_22H2O2H2+O2

FROM DATA

Moles of WATER
"75 g" / "18 g/mol" =75 g18 g/mol="4.167 mol of"" H_2O4.167 mol ofH2O

Mol of OXYGEN
O_2 / ("2 "H_2 O") 4.167=O22 H2O4.167="2.083 mol of"" O_22.083 mol ofO2

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

V = "nRT"/"P"V=nRTP

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