Charcoal is primarily carbon.
Determine the mass of CO_2 produced by burning enough carbon (in the form of charcoal) to produce 510 kJ of heat.
C + O2 --> CO2 Delta H = -393.5 kJ
393.5 kJ x (?g CO2/44) = 510 kJ. Solve for ?gCO2.
To determine the mass of CO2 produced, we can use the principle of stoichiometry, which relates the coefficients of balanced chemical equations to the quantities of substances involved. The given balanced chemical equation is C + O2 --> CO2.
First, let's calculate the number of moles of CO2 produced using the given heat release, given by ΔH = -393.5 kJ:
ΔH = -393.5 kJ
Energy released in the reaction = 510 kJ
We can set up a proportion to solve for the moles of CO2 produced:
ΔH / Energy released = Moles of CO2 / Moles of CO2 produced
Substituting the given values, we get:
-393.5 kJ / 510 kJ = 1 mol CO2 / Moles of CO2 produced
Next, we need to convert the moles of CO2 produced to mass. To do this, we need to know the molar mass of carbon (C) and carbon dioxide (CO2):
Molar mass of C = 12.01 g/mol
Molar mass of CO2 = (12.01 g/mol) + 2*(16.00 g/mol) = 44.01 g/mol
Now, we can set up another proportion:
Molar mass of CO2 / Moles of CO2 produced = Mass of CO2 / 1 mol CO2
Substituting the molar masses, we get:
44.01 g/mol / Moles of CO2 produced = Mass of CO2 / 1 mol CO2
By rearranging the equation, we can solve for the mass of CO2:
Mass of CO2 = (44.01 g/mol) * (Moles of CO2 produced)
Now, substitute the known values:
Mass of CO2 = (44.01 g/mol) * [(ΔH / Energy released)]
Calculating the mass of CO2 produced will give us the answer.