To determine the amount of C12H4CI6 reacted, we need to use stoichiometry and the molar mass of C12H4CI6.
The balanced equation tells us that the ratio between C12H4CI6 and CO2 is 2:24 (or 1:12). This means that for every 12 moles of CO2 produced, 1 mole of C12H4CI6 is reacted.
We can calculate the moles of CO2 produced using its molar mass of 44.01 g/mol:
moles of CO2 = mass of CO2 / molar mass of CO2
moles of CO2 = 108.53 g / 44.01 g/mol ≈ 2.464 moles
From the ratio, we can see that 12 moles of CO2 corresponds to 1 mole of C12H4CI6.
Thus, the moles of C12H4CI6 reacted can be calculated as:
moles of C12H4CI6 = moles of CO2 / 12
moles of C12H4CI6 = 2.464 moles / 12 ≈ 0.205 moles
Finally, we can convert moles of C12H4CI6 to grams using its molar mass of 376.64 g/mol:
grams of C12H4CI6 = moles of C12H4CI6 * molar mass of C12H4CI6
grams of C12H4CI6 = 0.205 moles * 376.64 g/mol ≈ 77.25 g
Therefore, approximately 77.25 grams of C12H4CI6 are reacted when 108.53 g of CO2 are produced.
2C12H4CI6+23O2+2H2O->24CO2+12HCI (d) how many grams of C12H4CI6 are reacted when 108.53 g of CO2 are produced? Note: use three significant digits in your answer. g C12H4CI6
1 answer