The volume of oxygen at STP required would be 252.0 mL.
<h3>Stoichiometic problem</h3>
The equation for the complete combustion of C2H2 is as below:

The mole ratio of C2H2 to O2 is 2:5.
1 mole of a gas at STP is 22.4 L.
At STP, 100.50 mL of C2H2 will be:
100.50 x 1/22400 = 0.0045 mole
Equivalent mole of O2 according to the balanced equation = 5/2 x 0.0045 = 0.01125 moles
0.01125 moles of O2 at STP = 0.01125 x 22400 = 252.0 mL
Thus, 252.0 mL of O2 gas will be required at STP.
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Answer:
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Answer:
4NH₃(g) +3O₂(g) ⇒2N₂(g) +6H₂O(g)
Explanation:
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Single bonds are those that bond with one atom, and sigma bonds are the strongest type of covalent bonds that are single bonded.
That means NO, not all single bonds are sigma bond, but all sigma bonds are single bonds.