Final answer:
Using Charles's law, the gas temperature raised from 23.0 °C to 31.5 °C at constant pressure will cause its volume to increase from an initial volume of 0.300 L to approximately 0.308 L.
Step-by-step explanation:
The student's question relates to Charles's law, which describes the relationship between the volume and temperature of a gas at constant pressure. In this case, we want to find the volume the gas would occupy if its temperature were raised from 23.0 °C to 31.5 °C at a constant pressure of 132 atm. To solve this, we must convert the temperatures to the Kelvin scale (adding 273.15) and then use the Charles's law equation V1/T1 = V2/T2.
First, convert temperatures from Celsius to Kelvin:
- T1 = 23.0 °C + 273.15 = 296.15 K
- T2 = 31.5 °C + 273.15 = 304.65 K
Next, apply Charles's law:
- V1 (initial volume) = assumed to be known as 0.300 L
Therefore, V2 (final volume) can be calculated by rearranging the equation to V2 = (V1 × T2) / T1:
V2 = (0.300 L × 304.65 K) / 296.15 K = 0.3078 L approximately
So, we expect the gas to occupy a volume of 0.308 L after the temperature increase at constant pressure.