Acetylene C2H2 burns in air forming carbon dioxide CO2 and water vapour H2O .Calculate the volume of air required to completely burn 50 cc of acetylene. Assume air contains 20% oxygen...
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4
C2H5 + 2.5 O2→2CO2 + H2O
for burning 1 mole of C2H5, 2.5 moles of oxygen is required
so, 2.5 x 22.4 = 56000cm3 of O2
total required air = M
20% of air = 56000 cm3 of O2
20 M/100 = 56000 cm3 of O2
M = 56000 x 100/20
= 280,000cm3
for burning 1 mole of C2H5, 2.5 moles of oxygen is required
so, 2.5 x 22.4 = 56000cm3 of O2
total required air = M
20% of air = 56000 cm3 of O2
20 M/100 = 56000 cm3 of O2
M = 56000 x 100/20
= 280,000cm3
Answered by
0
C2h2 + 5/202 = 2 co2 + h2O
Burning of 1 mole of c2h2 requires 2.5 mole O2
That means 2.5 x 22.4L = 56000 cm 3 o2
Let total air required be M
20% of air = 56000 cm3o2
20 m/100 = 56000cm3o2
M = 56000 x 100/20 = 280000 cm raise to power 3
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