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

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Answer 1 · 2018-03-16T18:33:48

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

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

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),

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

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