An athlete is given 100 g of glucose (C6H12O6) of energy equivalent to 1560 kJ. He utilizes 50 percent 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 kJ/mol.

Question

An athlete is given 100 g of glucose (C6H12O6) of  energy equivalent to 1560 kJ. He utilizes 50 percent 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 kJ/mol.

Shiksha Nation · Accepted Answer

Energy left unutilized = (1560 / 2) kJ = 780 kJ

For losing 44 kJ of energy, water to be evaporated = 1 mole = 18 g

∴ For losing 780 kJ of energy, water to be evaporated = (18 / 44) × 780 g = 319 g

An athlete is given 100 g of glucose (C6H12O6) of energy equivalent to 1560 kJ. He utilizes 50 percent 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 kJ/mol.

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