Amount of `CO_2` abosorbed by plant to produce 180 gm of glucose

Options

A. 216 gm
B. 264 gms
C. 192 gm
D. 108 gms

Answer

To solve the problem of how much CO₂ is absorbed by a plant to produce 180 grams of glucose, we can follow these steps:

### Step 1: Understand the Photosynthesis Reaction
The process of photosynthesis can be summarized by the following chemical equation:
\[ 6 \, CO_2 + 6 \, H_2O \xrightarrow{\text{light energy}} C_6H_{12}O_6 + 6 \, O_2 \]
This equation shows that 6 molecules of carbon dioxide (CO₂) and 6 molecules of water (H₂O) are used to produce one molecule of glucose (C₆H₁₂O₆) and oxygen.

### Step 2: Determine the Molecular Weight of Glucose
To find out how much CO₂ is needed for 180 grams of glucose, we first need to confirm the molecular weight of glucose:
- Carbon (C): 12 g/mol
- Hydrogen (H): 1 g/mol
- Oxygen (O): 16 g/mol

For glucose (C₆H₁₂O₆):
\[ \text{Molecular weight} = (6 \times 12) + (12 \times 1) + (6 \times 16) = 72 + 12 + 96 = 180 \, \text{g/mol} \]

### Step 3: Calculate the Amount of CO₂ Required
From the photosynthesis equation, we know that to produce 1 molecule of glucose, 6 molecules of CO₂ are required. Since 180 grams of glucose corresponds to 1 mole of glucose, we need to find out how much CO₂ is needed for this amount.

### Step 4: Determine the Molecular Weight of CO₂
Next, we calculate the molecular weight of carbon dioxide (CO₂):
- Carbon (C): 12 g/mol
- Oxygen (O): 16 g/mol

For CO₂:
\[ \text{Molecular weight} = 12 + (2 \times 16) = 12 + 32 = 44 \, \text{g/mol} \]

### Step 5: Calculate the Total Weight of CO₂ Needed
Since 6 moles of CO₂ are required to produce 1 mole of glucose:
\[ \text{Weight of CO₂} = 6 \times 44 \, \text{g} = 264 \, \text{g} \]

### Conclusion
Therefore, the amount of CO₂ absorbed by the plant to produce 180 grams of glucose is **264 grams**.