How many grams C12H4CI6 are reacted when 108.53 g of CO2 are produced?
To determine the number of grams of C12H4CI6 reacted, we need to use stoichiometry.
The balanced chemical equation for the reaction is:
C12H4CI6 + 2CO2 -> 12CO + 6HCL
From the equation, we can see that for every 2 moles of CO2 produced, 1 mole of C12H4CI6 is reacted.
First, we need to convert the given mass of CO2 into moles.
Molar mass of CO2 = 12.01 g/mol (C) + 2 x 16.00 g/mol (O) = 44.01 g/mol
Moles of CO2 = 108.53 g CO2 / 44.01 g/mol = 2.4653 mol CO2
Since the ratio of CO2 to C12H4CI6 is 2:1, the moles of C12H4CI6 reacted will be half the moles of CO2 produced.
Moles of C12H4CI6 = 1/2 x 2.4653 mol CO2 = 1.23265 mol C12H4CI6
Now, we can convert moles of C12H4CI6 into grams using its molar mass.
Molar mass of C12H4CI6 = 12.01 g/mol (C) + 4 x 1.01 g/mol (H) + 6 x 35.45 g/mol (Cl) = 296.12 g/mol
Grams of C12H4CI6 = 1.23265 mol C12H4CI6 x 296.12 g/mol = 364.16 g
Therefore, 364.16 grams of C12H4CI6 are reacted when 108.53 g of CO2 are produced.