An athlete is given 180 g of glucose `(C_(6)H_(12)O_(6))`. He utilises 50% of the energy due to internal combustion in the body. In order to avoid storage of energy in the body, calculate the masss of water he would need to perspire. Given enthalpy of combustion of glucose is -2800 kJ `mol^(-1)` and enthalpy of evaporation of water is 44 kJ `mol^(-1)`

Explanation

To solve the problem step by step, we will follow the reasoning presented in the video transcript and provide a clear breakdown of the calculations.

### Step 1: Calculate the number of moles of glucose
The molar mass of glucose (C₆H₁₂O₆) can be calculated as follows:
- Carbon (C): 6 atoms × 12 g/mol = 72 g/mol
- Hydrogen (H): 12 atoms × 1 g/mol = 12 g/mol
- Oxygen (O): 6 atoms × 16 g/mol = 96 g/mol

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