Question

How many moles of carbon dioxide are produced when 5.12 mol of propane gas is burned in excess oxygen? C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(l)

Answer 1

Answer:

15.36 moles of carbon dioxide are produced when 5.12 mol of propane gas is burned in excess oxygen

Explanation:

The Balanced Chemical equation is :

$C_3 H_8 (g) + 5O_2 (g) > 3CO_2 (g) + 4H_2 O(l)$

Mole ratio of $C_3 H_8:CO_2$ is 1 : 3

That is, 1 mole of propane gas produces 3 moles of carbon dioxide gas.

Using mole ratio we can solve this  

$5.12mol C_3 H_8 \times \frac {(3mol CO_2)}{(1mol C_3 H_8 )}$

$=15.36 mol CO_2$ is produced.

(Answer)

Please note  :

To convert moles to mass, we multiply by molar mass  

To convert mass to moles, we divide by molar mass

Molar mass is the mass of 1 mole of the substance

For example molar mass of $CO_2$ is

$(12.0+2\times16)=44 g/mol$

(we just add the atomic mass of the atoms to get the molar mass of the substance)

Answer 2

Answer:

15.4 mol CO₂

Explanation:

5.12 mol C₃H₈ × (3 mol CO₂ / mol C₃H₈) ≈ 15.4 mol CO₂