Hot carbon reacts with steam to produce an equimolar rnixture of CO(g) and `H_2(g)` known as water gas. What is the energy released as water gas is used as fuel?
`CO(g) +1/2O_2(g) to CO_2(g) , Delta H = -282.985kJ`
`H_2(g) + 1/2 O_2(g) to H_2O(g), Delta H = -241.818 kJ`

Explanation

To find the energy released when water gas (a mixture of CO and H₂) is used as fuel, we need to consider the combustion reactions of both components (CO and H₂) and their respective enthalpy changes.

### Step-by-Step Solution:

1. **Identify the Reactions**:
- The combustion of carbon monoxide (CO):
\[
\text{CO(g)} + \frac{1}{2} \text{O}_2(g) \rightarrow \text{CO}_2(g) \quad \Delta H = -282.985 \text{ kJ}
...