Liquid octane ch3ch26ch3 will react with gaseous oxygen o2 to produce gaseous carbon dioxide co2 and gaseous water h2o . suppose 94. g of octane is mixed with 100. g of oxygen. calculate the maximum mass of carbon dioxide that could be produced by the chemical reaction. round your answer to 3 significant digits.

88.0g of

Explanation:

Step 1: Write balanced chemical equation for combustion

Step 2: Determine moles of octane and oxygen

where 'n' is the number of moles, 'm' is the mass and 'M' is the molar mass

Step 3: Determine which is the limiting reactant

1 mole of octane requires 12.5 moles of oxygen for complete combustion

0.825 moles of octane will require 10.3125 moles of oxygen for complete combustion.

As there are not sufficient moles of oxygen for complete combustion of octane, the completion of the reaction will depend on when all moles of oxygen are consumed. Thus, oxygen is the limiting reactant

Step 4: Determine number of moles of carbon dioxide produced

12.5 moles of oxygen will produce 8 moles of carbon dioxide

3.125 moles of oxygen will produce 2.00 moles of carbon dioxide

Step 5: Determine mass of carbon dioxide produced

1. 1 mole of anything contains 6.022x10^23 pieces  

d  

2. a  

3. c, number  

5. 1.24x10^24atoms / 6.022x10^23atoms/mole = 2moles h2 atoms  

6. fe2br3 mass = 2moles x mass fe + 3 moles x mass br  

molar mass = grams / number of moles = g/mole  

to find moles = g / molar mass  

to find mass = g = molar mass / moles

answers: to make sure that all of the broken pieces of tablet were added to the water, to allow for fair comparison of all three trials, with different particle sizes to avoid experimental error