A. The balanced equation for the reaction is
2C₂H₂ + 5O₂ —> 4CO₂ + 2H₂O
B. The volume of the oxygen gas required to burn 0.700 L of acetylene gas is 1.75 L
C. The volume of carbon dioxide gas produced is 1.4 L
D. The volume of water vapor produced is 0.7 L
<h3>A. Balanced equation </h3>
The balanced equation for the reaction between acetylene gas (C₂H₂) and oxygen gas (O₂) is given below
2C₂H₂ + 5O₂ —> 4CO₂ + 2H₂O
<h3>B. How to determine the volume of oxygen </h3>
2C₂H₂ + 5O₂ —> 4CO₂ + 2H₂O
Since the reaction occurred at standard temperature and pressure, we can thus say that:
From the balanced equation above,
2 L of C₂H₂ reacted with 5 L O₂.
Therefore,
0.7 L of C₂H₂ will react with = (0.7 × 5) / 2 = 1.75 L of O₂
Thus, 1.75 L of O₂ is needed for the reaction
<h3>C. How to determine the volume of carbon dioxide </h3>
2C₂H₂ + 5O₂ —> 4CO₂ + 2H₂O
From the balanced equation above,
2 L of C₂H₂ reacted to produce 4 L of CO₂
Therefore,
0.7 L of C₂H₂ will react to produce = (0.7 × 4) / 2 = 1.4 L of CO₂
Thus, 1.4 L of CO₂ were produced
<h3>D. How to determine the volume of water. </h3>
2C₂H₂ + 5O₂ —> 4CO₂ + 2H₂O
From the balanced equation above,
2 L of C₂H₂ reacted to produce 2 L of H₂O
Therefore,
0.7 L of C₂H₂ will also react to produce 0.7 L of H₂O
Thus, 0.7 L of H₂O was produced
Learn more about stoichiometry:
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