Liquid octane will react with gaseous oxygen to produce gaseous carbon dioxide and gaseous water . suppose 10.3 g of octane is mixed with 69. g of oxygen. calculate the maximum mass of carbon dioxide that could be produced by the chemical reaction. round your answer to significant digits.

Explanation:

We are given the masses of two reactants and asked to determine the mass of the product.

This looks like a limiting reactant problem.

1. Assemble the information

We will need a balanced equation with masses and molar masses, so let’s gather all the information in one place.  

MM:         114.23     32.00      44.01

               2C₈H₁₈ + 25O₂ ⟶ 16CO₂ + 18H₂O

Mass/g:     10.3        69.  

2. Calculate the moles of each reactant

3. Calculate the moles of CO₂ from each reactant

4. Calculate the mass of CO₂

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

i believe it is a.) released into

explanation: