Final answer:
Based on Gay-Lussac's Law, the pressure of a gas increases with temperature when volume is constant. Doing the conversion to Kelvin and calculations, the closest approximate new pressure of the gas would be 15.4 atm.
Step-by-step explanation:
The question concerns the properties of gases, namely the relationship between their pressure and temperature. This relationship is described by Gay-Lussac's Law, which states that the pressure of a gas is directly proportional to its temperature, assuming the volume remains constant. Since only a minor temperature change from 97°C to 100°C is given, this means the pressure would slightly increase as well.
However, we should remember to use the absolute scale in gas laws. Converting degrees Celsius to Kelvin (K = 273 + °C) gives the initial temperature as 370 K and final as 373 K. Applying the law (P1/T1 = P2/T2) gives P2 = P1*(T2/T1). Substituting known values (15 atm, 370 K, 373 K) gives us approximately 15.2 atm. But since this choice is not in the list, the closest option is therefore 15.4 atm
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