How much oxygen is formed from 264 g of `CO_(2)` and 216 g of `H_(2)O` ?

Options

A. 96 g
B. 216 g
C. 264 g
D. 192 g

Explanation

To determine how much oxygen is formed from 264 g of CO₂ and 216 g of H₂O, we can follow these steps:

### Step 1: Write the balanced photosynthesis equation
The balanced equation for photosynthesis is:
\[ 6 \, CO_2 + 6 \, H_2O \rightarrow C_6H_{12}O_6 + 6 \, O_2 \]

### Step 2: Calculate the molar masses
- Molar mass of CO₂:
- Carbon (C) = 12 g/mol
- Oxygen (O) = 16 g/mol
- Molar mass of CO₂ = 12 + (16 × 2) = 44 g/mol

- Molar mass of H₂O:
- Hydrogen (H) = 1 g/mol
- Oxygen (O) = 16 g/mol
- Molar mass of H₂O = (1 × 2) + 16 = 18 g/mol

### Step 3: Calculate the number of moles of CO₂ and H₂O
- Moles of CO₂:
\[ \text{Moles of } CO_2 = \frac{\text{mass}}{\text{molar mass}} = \frac{264 \, g}{44 \, g/mol} = 6 \, moles \]

- Moles of H₂O:
\[ \text{Moles of } H_2O = \frac{\text{mass}}{\text{molar mass}} = \frac{216 \, g}{18 \, g/mol} = 12 \, moles \]

### Step 4: Determine the limiting reagent
From the balanced equation, we see that 6 moles of CO₂ react with 6 moles of H₂O to produce 6 moles of O₂. Since we have 6 moles of CO₂ and 12 moles of H₂O, CO₂ is the limiting reagent.

### Step 5: Calculate the amount of oxygen produced
According to the balanced equation, 6 moles of CO₂ produce 6 moles of O₂. Therefore, the moles of O₂ produced will also be 6 moles.

### Step 6: Calculate the mass of O₂ produced
- Molar mass of O₂:
\[ \text{Molar mass of } O_2 = 16 \times 2 = 32 \, g/mol \]

- Mass of O₂ produced:
\[ \text{Mass of } O_2 = \text{moles} \times \text{molar mass} = 6 \, moles \times 32 \, g/mol = 192 \, g \]

### Conclusion
The amount of oxygen formed from 264 g of CO₂ and 216 g of H₂O is **192 g**.

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