An hourly energy requirement of an astronaut can be satisfied by the energy released when 34 grams of sucrose (`C_(12)H_(22)O_(11)`) are burnt in his body. How many grams of oxygen would he need to be carried in space capsule to meet his requirement for one day ?

Explanation

To solve the problem of how many grams of oxygen an astronaut would need to carry in a space capsule to meet his energy requirement for one day, we can follow these steps:

### Step 1: Write the balanced chemical equation for the combustion of sucrose.
The combustion of sucrose (C₁₂H₂₂O₁₁) in the presence of oxygen (O₂) produces carbon dioxide (CO₂) and water (H₂O). The balanced equation is:

\[ C_{12}H_{22}O_{11} + 12 O_2 \rightarrow 12 CO_2 + 11 H_2O \]

### Step 2: Calculate the number of moles of sucrose in 34 grams.
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