When `12.0g` of `C` reacted with a limited quantity of oxygen, `57.5 kcal `of heat was produced. Calculate the number of `CO` and number of moles of `CO_(2)` produced.
Given `C +O_(2) rarr CO_(2), Delta_(f)H = - 94.05 kcal`
`C +1//2O_(2) rarr CO, Delta_(f)H =- 21.41 kcal `

Explanation

To solve the problem, we need to determine the number of moles of carbon monoxide (CO) and carbon dioxide (CO₂) produced when 12.0 g of carbon reacts with a limited quantity of oxygen, producing 57.5 kcal of heat. We will use the given enthalpy changes of formation for both reactions.

### Step 1: Calculate the number of moles of carbon (C)
The molar mass of carbon (C) is approximately 12.01 g/mol.

\[ \text{Number of moles of } C = \frac{\text{mass of } C}{\text{molar mass of } C} = \frac{12.0 \text{ g}}{12.01 \text{ g/mol}} \approx 1.00 \text{ mol} \]
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