An automobile gasoline tank holds 45 kg of gasoline. When the gasoline burns, 158 kg of oxygen are consumed and carbon dioxide and water are produced.What is the total combined mass of carbon dioxide and water that is produced?

Answer 1

gasoline is octane ... C8H18

2 C8H18 + 25 O2 ---> 16 CO2 + 18 H2O

the reaction equation gives the molar ratios

find the moles of O2 consumed, then calculate the moles of products produced

Answer 2

24

Answer 3

Using the coefficients of the balanced chemical equation:

2 moles of C8H18 react with 25 moles of O2 to produce 16 moles of CO2 and 18 moles of H2O.

So, if 158 kg of O2 is consumed, we can calculate the amount of gasoline used:

25 moles of O2 are needed for 2 moles of C8H18 to react.

158 kg of O2 is equal to (158/32) moles of O2.

So, the moles of C8H18 used would be (2/25) x (158/32) = 2.51 moles.

Using the same molar ratios, we can find the moles of CO2 produced:

16 moles of CO2 are produced for every 2 moles of C8H18 used.

So, the moles of CO2 produced would be (16/2) x 2.51 = 20.08 moles.

Similarly, we can find the moles of H2O produced:

18 moles of H2O are produced for every 2 moles of C8H18 used.

So, the moles of H2O produced would be (18/2) x 2.51 = 22.55 moles.

Now, we need to convert these moles into mass.

The molar mass of CO2 is 44 g/mol, so the mass of CO2 produced would be 20.08 x 44 = 883.52 g or 0.88352 kg.

The molar mass of H2O is 18 g/mol, so the mass of H2O produced would be 22.55 x 18 = 405.9 g or 0.4059 kg.

So, the total combined mass of carbon dioxide and water that is produced is 0.88352 kg + 0.4059 kg = 1.28942 kg, or approximately 1.29 kg.