Question

Butane burns as shown in the balanced chemical equation 2C4H10 + 1302 -> 1OH2O + 8CO2. If 6 mol of butane burn, ____ mol of carbon dioxide are produced.

Answer 1

24

Step-by-step explanation

We have a balanced chemical equation from the question that depicts the combustion of butane (C4H10) and formation of carbon dioxide (CO2) and water (H2O)

2C4H10 + 1302 -> 1OH2O + 8CO2.

We can clearly see from the equation that, the formation of 8 moles of carbon dioxide (CO2) molecules requires the input of 2 moles of butane (C4H10) and 13 mole of water (H2O).

So indirectly, it tells that the moles of water molecules will be four times the moles of butane (C4H10) molecules used in the reaction.

So if we say that 6 moles of butane (C4H10) is used and the reaction is going in such a way that Oxygen is not a limiting reactant, then 24 moles of water will be produced because 6 multiplied by 4 is 24.

Hope it help!