10 g of hydrogen and 64g of oxygen were filled in a steel vessel and exploded . volume of gaseous product after reaction
Answers
Answer: hello buddy friend the answer is :-
The balanced equation for this reaction is as follows:
2H₂ + O₂ -------> 2H₂O
Find the moles of the reacting gases.
10g of hydrogen
moles = mass/molar mass
= 10g / 2
= 5 moles
64g of oxygen
mass/molar mass
moles = 64/32
= 2 moles
The mole reaction for the equation above is H₂ : O₂ is 2 :1
Therefore 5 moles of H₂ will require 2.5 moles of oxygen - this makes oxgen the limiting reagent.
We therefore use the moles of oxygen to find those of H₂O:
mole ratio O₂ : H₂O is 1 : 2
That means 2 moles of oxygen will produce 4 moles of H₂O
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Calculate volume of 4 moles of H₂O gas.
Ideal gas law states that 1 mole of an ideal gas occupies exactly 22.4 liters by volume.
If 1 mole = 22.4 liters
Then 4 moles = 22.4 × 4/1
= 89.6 liters
The volume of H₂O produced is 89.6 liters.
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answer
4 gram H2 requires 36 g of O2
then 10 g h2 requires 90 g of oxygen.so oxygen is limiting reagent
