Propane is used in BBQs and burns according to the following equation: C3H8 + 5O2 -> 3CO2 + 4H2O. If 2.2 moles of carbon dioxide are produced, how many moles of oxygen gas reacted?

2.2* (5/3)

Well, it seems like propane is really heating things up! According to the balanced equation, we know that 1 mole of propane (C3H8) reacts with 5 moles of oxygen gas (O2) to produce 3 moles of carbon dioxide (CO2). So, if 2.2 moles of carbon dioxide were produced, we can use some mathematical magic to determine the number of moles of oxygen gas that reacted.

Let's do the calculations:
For every 3 moles of carbon dioxide, we need 5 moles of oxygen gas.
Therefore, for every 2.2 moles of carbon dioxide, we would need (2.2/3) * 5 moles of oxygen gas to react.

After crunching the numbers, we find that approximately 3.67 moles of oxygen gas reacted. And there you have it - the oxygen gas gave its all to create that fiery BBQ!

To determine how many moles of oxygen gas reacted, we can use the stoichiometry of the balanced chemical equation.

According to the equation: C3H8 + 5O2 -> 3CO2 + 4H2O

From the equation, we can see that 3 moles of CO2 are produced for every 5 moles of O2 consumed.

We are given that 2.2 moles of CO2 are produced.

To calculate the moles of O2 consumed, we can set up a proportion using the ratio from the balanced equation:

(3 moles CO2 / 5 moles O2) = (2.2 moles CO2 / x moles O2)

Cross-multiplying the equation, we get:

3 moles CO2 * x moles O2 = 2.2 moles CO2 * 5 moles O2

3x = 11 moles O2

Dividing both sides of the equation by 3, we find:

x = 11 moles O2 / 3

x ≈ 3.67 moles O2

Therefore, approximately 3.67 moles of oxygen gas reacted.