Final answer:
Upon applying Charles's Law to find the volume of hydrogen gas at a higher temperature without a change in pressure, the volume is calculated to be 12.14 L, which is not listed in the provided choices. As a result, there might be an error in the question or the given options.
Step-by-step explanation:
The student's question involves calculating the change in volume of a gas when it is subjected to a temperature change while pressure remains constant. This is a direct application of Charles's Law in chemistry. The volume of a gas is directly proportional to its temperature when pressure is held constant. To solve the problem, we convert temperatures from Celsius to Kelvin and then apply the formula V1/T1 = V2/T2. Converting -196°C to Kelvins gives us 77 K (since K = °C + 273.15), and converting 100°C to Kelvins gives us 373 K. Now, we can set up the equation using our initial volume (2.50 L) and temperatures to find the final volume (V2).
Inserting our values into the equation: (2.50 L) / (77 K) = (V2) / (373 K). Solving for V2 gives us (2.50 L) * (373 K) / (77 K) = 12.14 L. Therefore, the final volume of hydrogen gas at 100°C is 12.14 L. However, as this option is not listed in the question, this is likely an oversight in the question, or it's based on a typo. If the question is from an actual exam or quiz, it's essential to inform the teacher or professor about the discrepancy, as none of the provided options (a through d) match the calculated volume. In the context of this exercise, since none of the options are correct, it's recommended to choose option 'd' as it's the closest to the calculated answer.