For the balanced equation shown below, how many moles of CO2 will be produced, if 0.7316 moles of Cl2 are produced? 4C2H3O2Cl+7O2=>8CO2+6H2O+2Cl2

Answer 1

how many moles of CO2 will be produced, if 0.7316 moles of Cl2 are produced? 4C2H3O2Cl+7O2=>8CO2+6H2O+2Cl2

given:

0.7316 mol Cl2

desired:

?moles CO2

Consider this expression:

molA/coefficientA = molB/coefficientB

so, basically,

mol A = 0.7316 mol Cl2

coefficient A = coefficient of Cl2 in equation = 2

mol B = ? mol CO2

coefficient B = coefficient of Co2 in equation = 8

Therefore:

mol Cl2 / coefficient Cl2 = mol CO2 / coefficient CO2

0.7316 / 2 = x / 8

0.7316(8)/2=x

x=mol CO2

x=2.9264 mol CO2

Just a different way of doing the same thing, but making it algebra instead of factor-label/dimensional-analysis.

Answer 2

This is a simple mole to mole stoichiometry question.

1. First you are going to start with what you have: 0.7316 moles of Cl₂
2. Since you have a balanced equation, you can use the coefficients to determine the ratio of moles of CO₂ to moles of Cl₂ - 8 moles CO₂ : 2 moles Cl₂ (This becomes your conversion factor).
3. Now you can set up your equation:

0.7316 mol Cl₂ x (8 mol CO₂ / 2 mol Cl₂) = 2.926 mol CO₂