Question

When 0.105 mol propane, c3h8 is burned in an excess of oxygen, how many moles of oxygen are consumed? the products are carbon dioxide and water. you have to properly balance the equation before you can answer this question?

Answer 1

When 0.105 mol propane is burned, 0.525 mol of oxygen are consumed.

Step-by-step explanation:

In order to determine how many moles of oxygen are consumed when 0.105 mol of propane (C3H8) is burned, we need to balance the chemical equation first. The balanced equation for the complete combustion of propane is:

C3H8 + 5O2 → 3CO2 + 4H2O

From the balanced equation, we can see that 1 mol of propane reacts with 5 mol of oxygen. Therefore, to calculate the moles of oxygen consumed, we can use the ratio:

0.105 mol C3H8 × 5 mol O2/1 mol C3H8 = 0.525 mol O2

Answer 2

Propane on reaction with Oxygen produces CO₂ and water;

C₃H₈ + 10 O₂ → 3 CO₂ + 4 H₂O

According to Balance equation,

1 mole of C₂H₈ required = 10 moles of O₂

Then,

0.105 moles of C₂H₈ will require = X moles of O₂

Solving for X,

X = ( 10 mol × 0.105 mol) ÷ 1 mol

X = 1.05 mol of O₂

Result:
1.05 mol of O₂ is required to consume 0.105 mol of C₂H₈ completely.