To determine the heat released when 35.2 g of CO₂ is formed from carbon and oxygen gas, we will follow these steps:

1. Calculate the number of moles of CO₂:

The molar mass of CO₂ can be calculated as follows:

Carbon (C): 12.01 g/mol

Oxygen (O): 16.00 g/mol

So, the molar mass of CO₂ is:

$$12.01 + (16.00 \times 2) = 12.01 + 32.00 = 44.01 \, \text{g/mol}$$

The number of moles of CO₂ in 35.2 g is calculated using:

$$\text{Number of moles} = \frac{\text{Mass}}{\text{Molar Mass}} = \frac{35.2 \, \text{g}}{44.01 \, \text{g/mol}} \approx 0.8 \, \text{moles}$$

2. Calculate the heat released for 0.8 moles of CO₂:

The heat of combination given is -393.5 kJ/mol. This is the energy released when 1 mole of CO₂ is formed:

$$\text{Heat released} = \text{Number of moles} \times \text{Heat of combination}$$

$$\text{Heat released} = 0.8 \, \text{moles} \times -393.5 \, \text{kJ/mol} = -314.8 \, \text{kJ}$$

After rounding, the heat released is approximately -315 kJ.

Answer: Option D $-$ 315 kJ.