Charcoal is primarily carbon. What mass of CO2 is produced if you burn enough carbon (in the form of charcoal) to produce 4.85×102kJ of heat? The balanced chemical equation is as follows:
C(s)+O2(g)→CO2(g),ΔH∘rxn=−393.5kJ
44 g CO2 x (485/393.5) = ?
Well, well, well! Burning some charcoal, are we? That's one way to get fired up! Now, let's calculate the mass of CO2 that'll be as hot as your enthusiasm for barbecuing!
First, we need to find the number of moles of carbon burnt, which we can do using the equation provided. We know that the reaction produces 4.85×10² kJ of heat, and the balanced equation tells us that it releases -393.5 kJ of energy per mole of carbon.
So, let's do some math magic:
4.85×10² kJ / -393.5 kJ/mol = -1.23 moles of carbon
Now, since we have a one-to-one ratio between carbon and CO2, the number of moles of CO2 produced will also be -1.23 moles.
To calculate the mass of CO2, we need to know the molar mass. Carbon has a molar mass of 12.01 g/mol, while oxygen has a molar mass of 16.00 g/mol.
So, the molar mass of CO2 would be:
12.01 g/mol (for carbon) + 2 * 16.00 g/mol (for oxygen) = 44.01 g/mol
Now, to find the mass of CO2 produced, we multiply the number of moles by the molar mass:
-1.23 moles * 44.01 g/mol = -54.14 grams
But wait! Negative mass doesn't make any sense! So, let's take a step back and remember that energy release is negative (-393.5 kJ in this case). That means we have to flip the signs back.
So, the actual mass of CO2 produced would be 54.14 grams.
Voila! There you have it. Approximately 54.14 grams of CO2 are produced when you burn enough charcoal to generate 4.85×10² kJ of heat. Time to fire up that grill and start some carbon-based chemistry!
To determine the mass of CO2 produced when burning charcoal, we first need to calculate the number of moles of carbon burned using the given heat of reaction:
ΔH∘rxn = -393.5 kJ
Heat produced = 4.85x10^2 kJ
Now, we can use the equation ΔH = nΔH∘rxn to calculate the number of moles of carbon burned:
n = Heat produced / ΔH∘rxn
n = 4.85x10^2 kJ / -393.5 kJ
Calculating the value of n:
n = -1.23 moles of carbon
According to the balanced chemical equation, each mole of carbon reacts with one mole of CO2 produced.
Therefore, the number of moles of CO2 produced is also -1.23 moles.
Next, we need to determine the molar mass of CO2, which is the sum of the molar masses of carbon (12.01 g/mol) and oxygen (16.00 g/mol):
Molar mass of CO2 = 12.01 g/mol + (16.00 g/mol x 2)
Molar mass of CO2 = 44.01 g/mol
Finally, we can calculate the mass of CO2 produced using the number of moles and molar mass:
Mass of CO2 = number of moles x molar mass
Mass of CO2 = -1.23 moles x 44.01 g/mol
Calculating the value:
Mass of CO2 = -54.13 g
Since mass cannot be negative, the mass of CO2 produced is 54.13 g.
Therefore, 54.13 grams of CO2 is produced when burning enough carbon (charcoal) to produce 4.85x10^2 kJ of heat.
To find the mass of CO2 produced when burning charcoal, we can use the principle of stoichiometry and the given balanced chemical equation. This involves using the molar ratio from the equation to convert between the amount of carbon (in moles) and the amount of CO2 produced (also in moles), and then converting the moles of CO2 to grams using the molar mass of CO2.
The molar ratio from the balanced equation is: 1 mole of carbon (C) reacts to produce 1 mole of carbon dioxide (CO2).
Step 1: Convert the given energy change (ΔH∘rxn) from kilojoules (kJ) to joules (J):
4.85×10^2 kJ = 4.85×10^2 × 10^3 J = 4.85×10^5 J
Step 2: Calculate the number of moles of CO2 produced using the energy change:
ΔH∘rxn = -393.5 kJ/mol
moles of CO2 = energy change (J) / ΔH∘rxn (J/mol)
moles of CO2 = 4.85×10^5 J / -393.5 kJ/mol
Step 3: Calculate the mass of CO2 produced:
To calculate the mass of CO2, we use its molar mass, which is the sum of the atomic masses of carbon and two oxygens:
Molar mass of CO2 = (12.01 g/mol) + (2 × 16.00 g/mol) = 44.01 g/mol
mass of CO2 = moles of CO2 × molar mass of CO2
Now, let's plug in the numbers and calculate:
moles of CO2 = 4.85×10^5 J / -393.5 kJ/mol = -1.23×10^3 mol
mass of CO2 = -1.23×10^3 mol × 44.01 g/mol = -5.40×10^4 g
Since mass cannot be negative, it seems there might be an error in the given amount of energy change. Double-check the given energy change value and recalculate the mass of CO2 using the correct value if necessary.