A person inhales `640g ` of `O_(2)` per day. If all the `O_(2)` is used for converting sugar into `CO_(2)` and `H_(2)O`, how much sucrose `(C_(12)H_(22)O_(11))` is consumed in the body in one day and what is the heat evolved ?
`(DeltaH_("combination of sucrose ")=-5645kJ mol^(-1))`

Explanation

To solve the problem, we need to follow these steps:

### Step 1: Write the balanced chemical equation for the combustion of sucrose.
The combustion of sucrose (C₁₂H₂₂O₁₁) can be represented as:
\[ C_{12}H_{22}O_{11} + 12 O_2 \rightarrow 12 CO_2 + 11 H_2O \]
The enthalpy change (ΔH) for this reaction is given as -5645 kJ/mol.

### Step 2: Calculate the moles of O₂ inhaled per day.
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