If a car produces 88g of CO2, how many grams of O2 are used up in the reaction?
To determine the number of grams of O2 used up in the reaction, we need to know the balanced chemical equation for the reaction involving the combustion of carbon in a car. However, assuming complete combustion of carbon to CO2, the reaction can be written as:
C + O2 -> CO2
From the equation, we can see that for every 1 mole of carbon (12 grams), 1 mole of CO2 (44 grams) is produced. This means that 88 grams of CO2 is equal to:
88 grams CO2 * (1 mole CO2 / 44 grams CO2) = 2 moles of CO2
Since the stoichiometric ratio between CO2 and O2 is 1:1, it means that 2 moles of O2 are used up in the reaction. To determine the number of grams of O2 used up, we need to multiply the number of moles of O2 by its molar mass.
Molar mass of O2 = 32 grams/mol
Therefore, the number of grams of O2 used up in the reaction is:
2 moles of O2 * (32 grams O2 / 1 mole O2) = 64 grams of O2
To find out how many grams of O2 are used up in the reaction, we first need to know the balanced chemical equation for the reaction. Without this information, it is not possible to determine the exact stoichiometry of the reaction.
However, we can make an assumption based on the reaction of a typical combustion of gasoline, which is often used as fuel in cars. The balanced equation for the combustion of one mole of octane (a component of gasoline) is:
2 C8H18 + 25 O2 -> 16 CO2 + 18 H2O
From this equation, we can see that for every 25 moles of O2 consumed, we produce 16 moles of CO2. Therefore, the molar ratio of O2 to CO2 is 25:16.
To convert the given amount of CO2 (88 grams) to moles, we need to know the molar mass of CO2, which is approximately 44 grams/mol. So, 88 grams of CO2 is equal to 88/44 = 2 moles of CO2.
Using the molar ratio of O2 to CO2, we can calculate the moles of O2 consumed:
(2 moles CO2) x (25 moles O2/16 moles CO2) = 3.125 moles O2
Finally, to convert moles of O2 to grams, we need to know the molar mass of O2, which is approximately 32 grams/mol. So, 3.125 moles O2 is equal to 3.125 x 32 = 100 grams of O2 used up in the reaction.
Therefore, based on the assumption of a typical combustion reaction, approximately 100 grams of O2 are used up when a car produces 88 grams of CO2.
If you work this the easy way you don't get the right answer. The easy way is to convert CO2 to O2; however, remember that a car using a hydrocarbon for gasoline and that produces CO2 AND H2O, both which contain oxygen. I think you need know what hydrocarbon is being burned. Then write the equation and follow the steps of this link below.
http://www.jiskha.com/science/chemistry/stoichiometry.html