Final answer:
Using Charles's Law, the final volume of the oxygen gas when cooled from 95.6°C to 0.5°C can be found by converting the temperatures to Kelvin, then using the formula V2 = V1 (T2/T1). After calculations, the final volume appears to be 1.195 mL, but this is not reflected in the provided answer choices, suggesting a potential error in the question set.
Step-by-step explanation:
The question is asking to determine the final volume of oxygen gas after a change in temperature, assuming that the pressure and amount of gas remains constant. This scenario can be analyzed using the Charles's Law, which states that for a given mass and constant pressure, the volume of a gas is directly proportional to its Kelvin temperature. The formula for Charles's Law is given by V1/T1 = V2/T2 where V1 and T1 are the initial volume and temperature, and V2 and T2 are the final volume and temperature, respectively.
To solve for the final volume V2, we must convert the given temperatures from Celsius to Kelvin, which is done by adding 273.15 to the Celsius temperature. For the initial temperature, T1 = 95.6°C + 273.15 = 368.75 K, and for the final temperature, T2 = 0.5°C + 273.15 = 273.65 K.
Now, using Charles's Law with the initial volume V1 = 1.61 mL, we rearrange the formula to solve for V2:
V2 = V1 (T2/T1)
Plugging in the temperatures:
V2 = 1.61 mL × (273.65 K / 368.75 K)
V2 = 1.61 mL × 0.742 = 1.195 mL
However, since none of the answer choices in the question match the calculated value of 1.195 mL, it seems there may have been an error in the question or the answer choices provided. The student should double-check the provided information and the answer choices or consider reporting an issue with the question.