Give the following reaction,find the mass of oxygen required to produce 13grams of CO2; C3H8+5O2--->3CO2 + 4H2O

Here is a worked example of a stoichiometry problem.

http://www.jiskha.com/science/chemistry/stoichiometry.html

To determine the mass of oxygen required to produce 13 grams of CO2 using the given balanced chemical equation:

C3H8 + 5O2 -> 3CO2 + 4H2O

First, we need to determine the molar mass of CO2. The molar mass of carbon dioxide (CO2) can be calculated by adding the atomic masses of carbon (C) and two oxygen (O) atoms together.

Molar mass of CO2 = (molar mass of C) + 2 * (molar mass of O)
= (12.01 g/mol) + 2 * (16.00 g/mol)
= 12.01 g/mol + 32.00 g/mol
= 44.01 g/mol

Now let's calculate the number of moles of CO2 produced when 13 grams of CO2 are formed. To do this, we can use the formula:

Number of moles = Mass / Molar mass

Number of moles of CO2 = 13 g / 44.01 g/mol
≈ 0.295 moles

From the balanced equation, we can see that for every 3 moles of CO2 produced, 5 moles of oxygen (O2) are required. Therefore, we can set up a ratio:

5 moles O2 / 3 moles CO2

Now, we can calculate the moles of oxygen (O2) required to produce 0.295 moles of CO2:

Moles of O2 = (5 moles O2 / 3 moles CO2) * 0.295 moles CO2
≈ 0.492 moles O2

Finally, to find the mass of oxygen required, we multiply the moles of oxygen (O2) by its molar mass:

Mass of O2 = Moles of O2 * Molar mass of O2
≈ 0.492 moles * (16.00 g/mol)
≈ 7.87 grams

Therefore, approximately 7.87 grams of oxygen are required to produce 13 grams of CO2.