Calculate the mass of coke needed to react with 0.302 kg of pure tin oxide (SnO2) given the reaction SnO2 + 2C -> Sn + 2CO and that coke is 80% carbon.

The molar mass of $\text{SnO}_2$ is the sum of the atomic mass of Sn and two times the atomic mass of O.

$$\text{Molar mass of SnO}_2 = (1 \times 119) + (2 \times 16) = 119 + 32 = 151 \text{ g/mol}$$

First, convert the mass of $\text{SnO}_2$ from kg to g.

$$\text{Mass of SnO}_2 = 0.302 \text{ kg} = 0.302 \times 1000 \text{ g} = 302 \text{ g}$$

Now, calculate the moles of $\text{SnO}_2$.

$$\text{Moles of SnO}_2 = \frac{\text{Mass of SnO}_2}{\text{Molar mass of SnO}_2} = \frac{302 \text{ g}}{151 \text{ g/mol}} = 2 \text{ mol}$$

From the balanced chemical equation, 1 mole of $\text{SnO}_2$ reacts with 2 moles of C.

$$\text{SnO}_2 + 2\text{C} \rightarrow \text{Sn} + 2\text{CO}$$

Since we have 2 moles of $\text{SnO}_2$, the moles of carbon required will be:

$$\text{Moles of C} = 2 \times (\text{Moles of SnO}_2) = 2 \times 2 \text{ mol} = 4 \text{ mol}$$

The molar mass of carbon is 12 g/mol.

$$\text{Mass of C} = \text{Moles of C} \times \text{Molar mass of C} = 4 \text{ mol} \times 12 \text{ g/mol} = 48 \text{ g}$$

Coke contains 80% carbon by mass. This means that the mass of carbon calculated (48 g) represents 80% of the total mass of coke.
Let the mass of coke be $x$.

$$0.80 \times x = 48 \text{ g}$$ $$x = \frac{48 \text{ g}}{0.80} = 60 \text{ g}$$

Finally, convert the mass of coke from g to kg.

$$\text{Mass of coke} = 60 \text{ g} = 0.060 \text{ kg}$$

Comparing this result with the given options:
A. 0.40 kg
B. 0.20 kg
C. 0.06 kg
D. 0.04 kg

The calculated mass of coke is 0.06 kg.

The final answer is $\boxed{\text{0.06 kg}}$