The standard heat of combustion of `Al` is `-837.8 kJ mol^(-1)` at `25^(@)C`. If `Al` reacts with `O_(2)` at `25^(@)C`, which of the following release `250kJ` of heat?

Options

A. The reaction of `0.624 mol of AI`
B. The formation fo `0.624 mol of AI_(2)O_(3)`
C. The reaction of `0.312 mol of AI`
D. The formation of `0.150 mol of AI_(2)O_(3)`

Explanation

To solve the problem, we need to determine how much aluminum (Al) is required to release 250 kJ of heat based on the standard heat of combustion of aluminum, which is given as -837.8 kJ/mol at 25°C.

### Step-by-Step Solution:

1. **Understand the Heat of Combustion**:
The heat of combustion of aluminum is -837.8 kJ/mol. This means that when 1 mole of aluminum combusts, it releases 837.8 kJ of heat.

2. **Set Up the Proportion**:
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