Question

The burning of ethane produces both CO₂ and H₂O. If 600 mL of CO₂ is produced at 25°C and 730 torr, what volume of water vapor would be produced at 34°C and 810 torr?

Use the balanced equation: C₂​H₆​+O₂​→CO₂​+H₂​​O

Answer 1

The volume of water vapor produced will be equivalent to CO₂ volume under the same conditions as per the balanced equation. After applying the combined gas law and Gay-Lussac's law to convert and adjust volumes, we can find the volume of H₂O vapor at the required conditions.

Step-by-step explanation:

To determine the volume of water vapor produced from the combustion of ethane, we will use the chemical equation and the fact that gases at equivalent conditions of temperature and pressure occupy the same volume. The balanced equation is:

C2H6(g) + 7/2O2(g) → 2CO2(g) + 3H2O(g).

Since the combustion produces an equal number of moles of CO2 and H2O, if 600 mL of CO2 is produced, then 600 mL of H2O would initially be formed at the same temperature and pressure. However, when we adjust for the new conditions (34°C and 810 torr), we will use Gay-Lussac's law for combining volumes of gases and the combined gas law.

First, convert the initial conditions of CO2 to standard conditions using the combined gas law. Then, calculate the volume of water vapor at standard conditions. Finally, adjust the volume of water vapor to the final conditions of 34°C and 810 torr. The steps are as follows:

Describe the initial state of CO2.Use the combined gas law to find the volume of H2O at standard temperature and pressure (STP).Use Gay-Lussac's law to adjust the calculated volume of H2O to the given final conditions.