Final answer:
The new pressure is estimated to be 6 atm. Celsius-Kelvin conversion: doubling temperature equals 273.15 K; Boyle's Law: halved volume, pressure becomes 6 atm (Option B).
Step-by-step explanation:
When the Celsius temperature doubles, it is equivalent to a change in temperature of 273.15 degrees Kelvin because the two scales have a difference of 273.15.
When the gas is transferred to a container with twice the volume, the pressure is halved according to Boyle's Law.
Therefore, since the original pressure was 12 atm, the new pressure would be 6 atm. Therefore, a good estimate for the new pressure is 6 atm (option B).
The relationship between Celsius and Kelvin temperatures involves a fixed offset of 273.15, as the Kelvin scale starts at absolute zero. When Celsius temperature doubles, it reflects a change of 273.15 K on the Kelvin scale. This fundamental conversion is vital in scientific contexts.
According to Boyle's Law, when the volume of a gas doubles, its pressure is halved, maintaining an inverse relationship. If the original pressure is 12 atm, doubling the volume results in a halved pressure, leading to an estimated new pressure of 6 atm.
This estimation aligns with Boyle's Law principles, making option B, representing a new pressure of 6 atm, a reasonable and accurate conclusion based on the given scientific principles and their application to the scenario.