MARKING BRAINLIEST!! - Ethane burns in oxygen gas to form gaseous carbon dioxide and water vapour according to the following equation: C2H6(g) + 3.5 O2(g) → 2 CO2(g) + 3 H2O(g) What volume of ethane, at constant pressure and temperature, would have reacted to produce 100 mL carbon dioxide?

50 mL of ethane, C2H6.

Explanation:

The balanced equation for the reaction is given below:

C2H6(g) + 3.5O2(g) → 2CO2(g) + 3H2O(g)

Since the reaction occurred at constant temperature and pressure, we can as well say that:

From the balanced equation above,

1 mL of C2H6 reacted with 3.5 mL of O2 to produce 2 mL of CO2 and 3 mL of H2O.

Finally, we shall determine the volume of C2H6 required to produce 100 mL of CO2.

This is illustrated below:

From the balanced equation above,

1 mL of C2H6 reacted to produce 2 mL of CO2.

Therefore XmL of C2H6 will react to produce 100 mL of CO2 i.e

XmL of C2H6 = (1 x 100)/2

XmL of C2H6 = 50 mL.

Therefore, 50 mL of ethane, C2H6 is required to produce 100 mL of carbon dioxide, CO2.

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