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 Photosynthesis Equation
The balanced equation for photosynthesis is:
\[ 6 \text{CO}_2 + 6 \text{H}_2\text{O} \rightarrow \text{C}_6\text{H}_{12}\text{O}_6 + 6 \text{O}_2 \]
This shows that 6 moles of carbon dioxide and 6 moles of water produce 6 moles of oxygen.

### Step 2: Convert Grams to Moles
To find out how many moles of CO₂ and H₂O we have, we use the formula:
\[ \text{Moles} = \frac{\text{mass (g)}}{\text{molar mass (g/mol)}} \]

#### For CO₂:
- Molar mass of CO₂ = 12 (C) + 16*2 (O) = 44 g/mol
- Moles of CO₂ =
\[ \frac{264 \text{ g}}{44 \text{ g/mol}} = 6 \text{ moles} \]

#### For H₂O:
- Molar mass of H₂O = 2 (H) + 16 (O) = 18 g/mol
- Moles of H₂O =
\[ \frac{216 \text{ g}}{18 \text{ g/mol}} = 12 \text{ moles} \]

### Step 3: Determine Limiting Reactant
From the balanced equation, we see that 6 moles of CO₂ react with 6 moles of H₂O. Since we have:
- 6 moles of CO₂
- 12 moles of H₂O

We can see that CO₂ is the limiting reactant because it will be completely consumed first.

### Step 4: Calculate Moles of Oxygen Produced
According to the balanced equation, 6 moles of CO₂ produce 6 moles of O₂. Therefore, from 6 moles of CO₂, we will produce:
- Moles of O₂ = 6 moles

### Step 5: Convert Moles of O₂ to Grams
Now, we convert the moles of O₂ back to grams:
- Molar mass of O₂ = 16*2 = 32 g/mol
- Mass of O₂ =
\[ \text{Moles} \times \text{Molar mass} = 6 \text{ moles} \times 32 \text{ g/mol} = 192 \text{ g} \]

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

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