The heat of combusion of benzne determined in a bomb calorimeter is `-870Kcal mol^(-1)` at `298 K`. The value of `DeltaE` for the reaction is

Options

A. `-1740 kcal mol^(-1)`
B. `+870 kcal mol^(-1)`
C. `-870 kcal mol^(-1)`
D. `+1740 kcal mol^(-1)`

Explanation

To find the value of ΔE (change in internal energy) for the combustion of benzene, we can follow these steps:

### Step 1: Understand the context
The heat of combustion of benzene is given as -870 kcal/mol at 298 K. This value represents the heat released when one mole of benzene is completely burned in a bomb calorimeter.

### Step 2: Relate heat of combustion to ΔE
In a bomb calorimeter, the heat measured corresponds directly to the change in internal energy (ΔE) of the system because the process occurs at constant volume. Therefore, the heat of combustion (q) is equal to ΔE.

### Step 3: Write the equation
Since the heat of combustion is given as -870 kcal/mol, we can write:
\[ \Delta E = q = -870 \text{ kcal/mol} \]

### Step 4: Conclusion
Thus, the value of ΔE for the combustion of benzene is:
\[ \Delta E = -870 \text{ kcal/mol} \]

### Final Answer
The value of ΔE for the reaction is **-870 kcal/mol**.

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