Question

Propane burns to form carbon dioxide and water. The equation for the reaction is:

C 3 H 8 (g)+5 O 2 (g) 3 CO 2 (g)+4 H 2 O(l)

3.60d * m ^ 3 carbon dioxide is produced when a sample of propane is burned in 7.25d * m ^ 3 oxygen.

Calculate the volume of unreacted oxygen. Give your answer in cm^ 3

Answer 1

Answer:

Propane burns to form carbon dioxide and water. The equation for the reaction is:

C3H8 (g)+5O2 (g) ->  3CO2 (g) + 4H2O(l)

Explanation:

From the balanced chemical equation, it is clear that:

1mol. of propane reacts with 5 mol. of O2 and forms 3 mol. of CO2.

In terms of volume, the above equation can be rewritten as:

1.0L. of propane reacts with 5.0L O2 and forms 3.0L of CO2.

Since,

$1dm^{3} =1.0L$

3.60dm^3 of CO2 is formed from how many dm^3 of O2?

$=>3.60dm^3 CO2 * \frac{5.0L O2}{3.0L CO2}\\=6.0dm^3 O2 \\=6.0L O2$

The volume of unreacted oxygen is:

$7.25dm^3 -6.0dm^3\\=1.25dm^3$

The volume of unreacted oxygen is 1.25L or 1250cm^3.

Since,

1dm^3=1000cm^3.