Final answer:
To find the new temperature of a gas when its volume and pressure change, the combined gas law is used. For the given data of the gas with an initial state of 1.1 atm, 7 L, and 285 K and the final state of 0.6 atm and 10 L, the new temperature is calculated to be approximately 213 Kelvin.
Step-by-step explanation:
The question you've asked is about determining the new temperature of a gas sample when its volume and pressure change. This type of problem can be solved using the combined gas law, which relates the pressure, volume, and temperature of a gas.
The combined gas law can be written as: (P1 * V1) / T1 = (P2 * V2) / T2, where P1 and P2 are the initial and final pressures, V1 and V2 are the initial and final volumes, and T1 and T2 are the initial and final temperatures in Kelvin, respectively.
Given your question:
- Initial pressure (P1) = 1.1 atm
- Initial volume (V1) = 7 L
- Initial temperature (T1) = 285 K
- Final pressure (P2) = 0.6 atm
- Final volume (V2) = 10 L
We rearrange the formula to solve for T2:
T2 = (P2 * V2 * T1) / (P1 * V1)
Plugging in the values:
T2 = (0.6 atm * 10 L * 285 K) / (1.1 atm * 7 L)
T2 = 1638 / 7.7
T2 ≈ 212.99 K
Therefore, the new temperature of the gas is approximately 213 Kelvin.