Charcoal is primarily carbon. Determine the mass of CO2
produced
...

Question

Charcoal is primarily carbon. Determine the mass of CO2
produced
by burning enough carbon (in the form of charcoal)
to produce 5.00 * 102 kJ of heat.
C(s) + O2( g)¡CO2( g) ΔH °rxn = -393.5 kJ

Accepted Answer

Hey everyone welcome back. Our question here is asking us to calculate the mass of carbon dioxide emitted by the following combustion and we're given our balanced reaction and our standard entropy of our reaction. A key to this question is to recognize that our standard envelop is per two moles of carbon dioxide. Since we've produced two moles of carbon dioxide in our reaction. Moving forward with our question, we can go ahead and take our 2.21 times 10 to the third, killer jewels of heat And we can convert this to two moles of carbon dioxide by using our standard entropy of our reaction, which is 1,452 0.2 kg joules per two mols. And the reason why we exclude our negative sign is because our question is asking for the mass of carbon dioxide emitted. So converting our moles into g, we're going to get our molar mass of carbon dioxide, which is 44.01 g per mole. And when we calculate this out, we end up with a value of 134 g of carbon dioxide. So I hope this made sense. And let us know if you have any questions

Charcoal is primarily carbon. Determine the mass of CO2 produced by burning enough carbon (in the form of charcoal) to produce 5.00 * 102 kJ of heat. C(s) + O2( g)¡CO2( g) ΔH °rxn = -393.5 kJ

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