Determine the mass of CO2 produced by burning enough
of each fuel...

Question

Determine the mass of CO2 produced by burning enough
of each fuel to produce 1.00 * 102 kJ of heat. 
a. CH4( g) + 2 O2( g)¡CO2( g) + 2 H2O( g)
ΔH °rxn = -802.3 kJ

Accepted Answer

Hey everyone welcome back! Our question here is asking us to calculate the mass of carbon dioxide emitted by the combustion of plantain and were given the following balance reaction with a standard entropy listed below. Now, the key to this question is to recognize that our standard entropy is per five moles of carbon dioxide and this is because we produce five moles in our reaction. Now moving forward with our question, we can go ahead and start off with our 5.96 times 10 squared killer joules of heat and we can go ahead and convert this into moles of carbon dioxide by taking our 3509 kg joules per five moles of carbon dioxide. And the reason why we remove our negative sign is because our question is asking us for the mass of carbon dioxide emitted by our combustion To convert this into grams of carbon dioxide. We can go ahead and take the molar mass of carbon dioxide, which is 44.01 g per one mole. And when we calculate this out and cancel out our units, we're going to end up with a value of 37.4 g of carbon dioxide. And this is going to be our final answer. So I hope this made sense. And let us know if you have any questions

Determine the mass of CO2 produced by burning enough of each fuel to produce 1.00 * 102 kJ of heat. a. CH4( g) + 2 O2( g)¡CO2( g) + 2 H2O( g) ΔH °rxn = -802.3 kJ

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