Final answer:
When the temperature of a gas that originally has a volume of 0.102 dm³ at 201 K is doubled, the new volume will be 204 cm³, following Gay-Lussac's law of direct proportionality between temperature and volume at constant pressure.
Step-by-step explanation:
The question is related to predicting the change in volume of a gas when its temperature is changed, while keeping pressure constant. According to Gay-Lussac's law of gases, which is part of the combined gas law, the volume of a gas at constant pressure is directly proportional to its Kelvin temperature. Therefore, if you double the temperature of a gas, you double its volume, assuming the pressure and the amount of gas remain unchanged.
Given that the initial volume of the gas is 0.102 dm³ (which is equivalent to 102 cm³) at a temperature of 201 K, if the temperature is doubled to 402 K, the new volume can be calculated. Using the direct proportionality (V1/T1 = V2/T2), we find that V2 = V1 * (T2/T1) which equals 102 cm³ * (402 K / 201 K) = 204 cm³. Hence, the new volume of the gas when the temperature is doubled will be 204 cm³.