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Acetylene gas (C2H2) burns completely in the presence of oxygen gas (O2) to yield carbon dioxide
gas (CO2) and water vapor (H2O).

1a. Write a balanced equation for this reaction.

1b. Assuming that all volume measurements occur at the same temperature and pressure, how many
liters of oxygen will be required to completely burn 0.700 L of acetylene gas?

1c. Assuming that all volume measurements occur at the same temperature and pressure, how many
liters of carbon dioxide gas will be produced in the reaction?

1d. Assuming that all volume measurements occur at the same temperature and pressure, how many
liters of water vapor will be produced in the reaction?

Sagot :

Eduard22sly

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

A. Balanced equation

The balanced equation for the reaction between acetylene gas (C₂H₂) and oxygen gas (O₂) is given below

2C₂H₂ + 5O₂ —> 4CO₂ + 2H₂O

B. How to determine the volume of oxygen

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

C. How to determine the volume of carbon dioxide

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

D. How to determine the volume of water.

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:

https://brainly.com/question/14735801

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