Final answer:
To find the pressure of the sample when it is heated to 127°C, we can use Gay-Lussac's Law. By plugging in the given temperatures and pressures into the formula, we can solve for the final pressure, which is 2.58 atm. So the correct answer is Option A.
Step-by-step explanation:
To solve this problem, we can use Gay-Lussac's Law, which states that the pressure of a gas is directly proportional to its temperature, assuming the volume and the amount of gas remain constant.
First, we need to convert the temperatures to Kelvin. To do this, we add 273 to both the initial temperature (37°C + 273 = 310 K) and the final temperature (127°C + 273 = 400 K).
Next, we can set up an equation using the temperatures and pressures:
P1/T1 = P2/T2
Plugging in the known values, we get:
(2 atm)/(310 K) = P2/(400 K)
Simplifying and solving for P2, we find:
P2 = (2 atm)(400 K)/(310 K) = 2.58 atm
Therefore, the pressure of the sample when heated to 127°C would be 2.58 atm.