If a pork roast must absorb 1700kJ to fully cook, and if only 13% of the heat produced by the barbeque is actually absorbed by the roast, what mass (g) of CO2 is emitted into the atmosphere during the grilling of the pork roast?
Hey there! So this just pretty simple actually, you just need to divide 1700 by 13% to get the actual heat needed. So after that, you will need to divide it by the heat of reaction to know how many moles of fuel you actually need. From there just use a mole ratio of the balanced equation and convert to mass to get the mass of O2. I hope this helps!