When 1 mol of glucose is burned, 2802.5 kJ of energy is released. If a high-level athlete burns 29 Mj of energy in a day, what is the mass (in Kg) of glucose the athlete would consume to obtain this amount of energy?
Added by Albert S.
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1 MJ = 1000 kJ Therefore, 29 MJ = 29,000 kJ Show more…
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As we exercise, our bodies metabolize glucose, converting it to $\mathrm{CO}_{2}$ and $\mathrm{H}_{2} \mathrm{O},$ to supply the energy necessary for physical activity. The simplified reaction is: $$ \mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}(a q)+6 \mathrm{O}_{2}(g) \longrightarrow 6 \mathrm{CO}_{2}(g)+6 \mathrm{H}_{2} \mathrm{O}(l)+2840 \mathrm{~kJ} $$ An individual weighing $68 \mathrm{~kg}$ jogging at $8 \mathrm{~km} / \mathrm{h}$ for 30 minutes would burn $1138 \mathrm{~kJ}$. How many moles of glucose would need to be metabolized to generate this required energy?
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