Thermodynamics and Thermochemistry 1 Question 71
73. An athlete is given $100 \mathrm{~g}$ of glucose $\left(\mathrm{C}{6} \mathrm{H}{12} \mathrm{O}_{6}\right)$ of energy equivalent to $1560 \mathrm{~kJ}$. He utilizes 50 per cent of this gained energy in the event. In order to avoid storage of energy in the body, calculate the weight of water he would need to perspire. The enthalpy of evaporation of water is $44 \mathrm{~kJ} / \mathrm{mol}$.
(1989, 2M)
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Solution:
- Moles of $\mathrm{H}_{2} \mathrm{O}$ needs to perspire $=\frac{1560}{2 \times 44}=17.72$
Weight of water needs to perspire $=17.72 \times 18=318.96 \mathrm{~g}$
