HOW MANY GRAMS OF CO2 WOULD BE FORMED FROM 20 GRAMS OF C6H6 IN THE FOLLOWING REACTION?
2 C6H6 + 15O2=12CO2 +6 H2O
All of these types of stoichiometry problems are worked the same way.
1. Write the balanced equation. You have done that.
2. Convert what you have to moles. You have grams C6H6. moles = grams/molar mass.
3. Using the coefficients in the balanced equation, convert moles of what you have (in this case C6H6) to moles of what you want (in this case CO2).
4. Now convert moles CO2 to grams. grams = moles CO2 x molar mass CO2.
Post your work if you get stuck.
To calculate the amount of CO2 formed from 20 grams of C6H6 in the given reaction, we need to first calculate the mole ratio between C6H6 and CO2.
The balanced reaction equation shows that 2 moles of C6H6 (benzene) react with 12 moles of CO2. This means that the mole ratio between C6H6 and CO2 is 2:12, or simplified as 1:6.
1 mole of C6H6 is equal to its molar mass, which is approximately 78.11 grams.
Therefore, to find the number of moles of C6H6 from 20 grams, we divide the mass by the molar mass:
Number of moles of C6H6 = Mass of C6H6 / Molar mass of C6H6
= 20 g / 78.11 g/mol
≈ 0.256 moles of C6H6
Using the mole ratio between C6H6 and CO2, we can now calculate the moles of CO2 formed:
Number of moles of CO2 = Number of moles of C6H6 × Mole ratio C6H6:CO2
= 0.256 moles × (1/6)
≈ 0.043 moles of CO2
Finally, to convert the moles of CO2 to grams, we multiply by the molar mass of CO2:
Mass of CO2 = Number of moles of CO2 × Molar mass of CO2
= 0.043 moles × (12.01 g/mol + 16.00 g/mol × 2)
≈ 4.68 grams of CO2
Therefore, approximately 4.68 grams of CO2 would be formed from 20 grams of C6H6 in the given reaction.