An athlete takes 100 g of glucose of energy equivalent to 1560 kJ. How much amount of energy is uptaken by 1 g molecule of glucose?

Options

A. `15.6 kJ`
B. `2808 kJ`
C. `1560 kJ`
D. `28.08 kJ`

Answer

To solve the problem, we need to determine how much energy is uptaken by one mole of glucose, given that 100 grams of glucose provides 1560 kJ of energy.

### Step-by-Step Solution:

1. **Identify the given data:**
- Energy provided by 100 g of glucose = 1560 kJ

2. **Calculate the energy provided by 1 g of glucose:**
- To find the energy per gram, we divide the total energy by the mass of glucose.
\[ \text{Energy per gram} = \frac{1560 \text{ kJ}}{100 \text{ g}} = 15.6 \text{ kJ/g} \]

3. **Determine the molar mass of glucose (C6H12O6):**
- The molar mass of glucose is calculated as follows:
- Carbon (C): 12.01 g/mol × 6 = 72.06 g/mol
- Hydrogen (H): 1.008 g/mol × 12 = 12.096 g/mol
- Oxygen (O): 16.00 g/mol × 6 = 96.00 g/mol
\[ \text{Total molar mass of glucose} = 72.06 + 12.096 + 96.00 = 180.156 \text{ g/mol} \approx 180 \text{ g/mol} \]

4. **Calculate the energy provided by 1 mole of glucose:**
- Since 1 mole of glucose weighs approximately 180 g, we can find the energy for 1 mole by multiplying the energy per gram by the molar mass.
\[ \text{Energy per mole} = 15.6 \text{ kJ/g} \times 180 \text{ g/mol} = 2808 \text{ kJ/mol} \]

5. **Conclusion:**
- The energy uptaken by 1 mole of glucose is 2808 kJ.

### Final Answer:
The amount of energy uptaken by 1 mole of glucose is **2808 kJ**.

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