Question

A major component of gasoline is octane (C&H₁g). When liquid octane is burned in air it reacts with oxygen (0₂) gas to produce carbon dioxide

gas and water vapor. Calculate the moles of carbon dioxide produced by the reaction of 0.095 mol of oxygen. Be sure your answer has a unit
symbol, if necessary, and round it to 2 significant digits.

Answer 1

Using the balanced chemical equation for the combustion of octane and setting up a ratio, it is calculated that 0.095 mol of oxygen will produce approximately 0.061 mol of carbon dioxide (CO2).

Step-by-step explanation:

To calculate the moles of carbon dioxide produced by the reaction of 0.095 mol of oxygen, we need to refer to the balanced equation for the combustion of octane (C8H18).

The balanced chemical equation for the combustion of octane is:

2 C8H18(l) + 25 O2(g) → 16 CO2(g) + 18 H2O(g)

From the balanced equation, we can see that it takes 25 moles of O2 to react with 2 moles of octane to produce 16 moles of CO2. To find out how many moles of CO2 are produced from 0.095 mol of O2, we can set up a ratio:

(16 mol CO2 / 25 mol O2) = x mol CO2 / 0.095 mol O2

Solving for x gives us:

x = (16 mol CO2 / 25 mol O2) * 0.095 mol O2 = 0.061 mol CO2

Therefore, the combustion of 0.095 mol of oxygen will produce approximately 0.061 mol of carbon dioxide (CO2). We round this to two significant digits, so the final answer is 0.061 mol CO2.