Given the following reaction (it IS balanced), how many grams of CO2 are produced when 0.700 moles of toluene (C7H8) is allowed to completely combust?
C7H8 + 9 O2 �¨ 7 CO2 + 4 H2O
mols toluene = 0.700
Using the coefficients in the balanced equation, convert mols toluene to mols CO2.
Now convert mols CO2 to grams. g = mols CO2 x molar mass CO2
To find out how many grams of CO2 are produced when 0.700 moles of toluene combust, we need to use the balanced chemical equation and stoichiometry.
The balanced equation is:
C7H8 + 9 O2 -> 7 CO2 + 4 H2O
From the balanced equation, we can see that for every 1 mole of C7H8 combusted, 7 moles of CO2 are produced. This means the ratio of C7H8 to CO2 is 1:7.
Now, we can use the given number of moles of C7H8 (0.700) to calculate the moles (and then grams) of CO2 produced.
Step 1: Calculate the moles of CO2 produced.
Since the ratio of moles of C7H8 to CO2 is 1:7, the number of moles of CO2 produced can be calculated as:
0.700 moles C7H8 * (7 moles CO2 / 1 mole C7H8) = 4.9 moles CO2
Step 2: Convert moles of CO2 to grams.
To convert moles to grams, we need to use the molar mass of CO2, which is calculated by summing the atomic masses of carbon (C) and oxygen (O).
Molar mass of CO2 = (12.01 g/mol) + (2 * 16.00 g/mol) = 44.01 g/mol
Now, we can calculate the grams of CO2 produced:
4.9 moles CO2 * (44.01 g CO2 / 1 mole CO2) = 215.5 g CO2
Therefore, when 0.700 moles of toluene completely combusts, it will produce 215.5 grams of CO2.