Electrolysis of 36 g of water 1. Mass of hydrogen produced 2. Volume of oxygen produced (oxygen density 1.29 g/m3)

Electrolysis of 36 g of water 1. Mass of hydrogen produced 2. Volume of oxygen produced (oxygen density 1.29 g/m3)

4G 22.4L 2H2O = energized =2 H2↑+ O2↑
2 2 1
2 2 1
V (O2)= nXVm=1X22.4=22.4L

4G 22.4L 2H2O = Energized =2 H2↑+ O2↑
2 2 1
2 2 1
V (O2)= nXVm=1X22.4=22.4L

Electrolyze 9 grams of water. How many liters of oxygen and hydrogen can be produced under standard conditions? Density drops of oxygen and hydrogen are used

Let X g of oxygen and Y g of hydrogen be generated.
2H2O=2H2+O2
20 4 16
9G yg xg
4/Y =20/9
Y =1.8
16/X =20/9
X =7.2
Answer:7.2 grams of oxygen and 1.8 grams of hydrogen are produced.